๐References & Further Reading (10)
Book
Chemistry: Part I (NCERT Textbook for Class XII)
By: National Council of Educational Research and Training (NCERT)
The official mandatory textbook covering basic chemical equilibrium and qualitative application of Le Chatelierโs Principle to concentration, pressure, and temperature changes.
Note: Mandatory reference for CBSE Board exams and the foundational theory required for JEE Main. Provides clear examples, including the Haber process and Contact process applications.
Website
Industrial Chemistry: Optimizing Yields using Le Chatelier's Principle
By: Royal Society of Chemistry (RSC) Learn Chemistry
Focuses specifically on the real-world industrial applications, detailing the high-pressure/moderate-temperature requirements for processes like the Haber synthesis.
Note: High relevance for application-based questions in both JEE Main and Advanced, particularly those asking for optimal conditions (a classic application scenario).
PDF
NCERT Exemplar Problems and Solutions: Chemical Equilibrium
By: NCERT/CBSE
Collection of challenging multiple-choice and short-answer questions approved by the CBSE board, testing the direct application of equilibrium concepts.
Note: Excellent source for standard, moderately difficult MCQs relevant to both CBSE (theory) and JEE Main (basic numerical application) standards.
Article
Le Chatelier's Principle: Historical Context and Modern Misconceptions
By: Dr. E. P. G. Harris
Explores the historical development of the principle and clarifies common teaching errors, especially regarding the effect of adding an inert gas or a solid component.
Note: Useful for teachers and advanced students to avoid subtle conceptual mistakes. Clarifies the precise mathematical boundaries of the principle.
Research_Paper
Modeling the Effect of Temperature and Pressure on High-Yield Ammonia Synthesis Catalysis
By: H. R. Chen and P. L. Davies
A practical computational study modeling the exact shifts in equilibrium conversion for the Haber process under varied industrial conditions, directly applying Le Chatelierโs insights.
Note: Provides quantitative data supporting the qualitative predictions of Le Chatelier's Principle in a major industrial reaction. Helps relate theory to realistic quantitative problems involving conversions.
โ ๏ธCommon Mistakes to Avoid (60)
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
โ
Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
โ
Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th
โ
Ignoring the System Boundary Condition (Constant V vs. Constant P) when Adding Inert Gas
Students frequently confuse the effect of adding an inert gas (like Helium or Argon) on the equilibrium position, often assuming a shift occurs regardless of the conditions. This overlooks the critical distinction between constant volume and constant pressure conditions.
๐ญ Why This Happens:
This error stems from focusing only on the increase in total system pressure ($P_{total}$) caused by the inert gas, and failing to recognize that the equilibrium constant ($K_p$) depends solely on the partial pressures of the reacting species.
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Correct Approach:
The correct approach involves analyzing the effect on partial pressures or concentrations (
$P_i$ or $[i]$):
| Condition | Effect on Partial Pressures/Concentrations | Shift? |
|---|
| Constant Volume (V) | Partial pressures of reactants/products remain unchanged. | No Shift |
| Constant Pressure (P) | Volume must increase. All reacting concentrations decrease (dilution effect). System shifts towards the side with a larger number of moles of gas (higher $Delta n_g$). | Shift Possible (if $Delta n_g
e 0$) |
๐ Examples:
โ Wrong:
For the reaction $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume will cause the equilibrium to shift to the right to counteract the pressure increase.
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Correct:
For $PCl_5(g)
ightleftharpoons PCl_3(g) + Cl_2(g)$, adding Argon at constant volume results in no change in the equilibrium position because the ratio of partial pressures (Qp) is unchanged. The total pressure increase is irrelevant to the established equilibrium.
๐ก Prevention Tips:
Always check the experimental conditions given in the JEE problem (Constant V or Constant P). This is a common advanced level trick.
Remember: Le Chatelier's principle responds to changes in the partial pressure/concentration of species included in the $K_p$ or $K_c$ expressions, not to the pressure exerted by an unreactive (inert) gas when volume is constant.
Treat adding inert gas at constant P exactly like increasing the volume (dilution effect).
CBSE_12th