Consider the following equilibrium for which AH = -84.9: SO₂(g) + Cl₂(g) = SO₂Cl₂(9) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction? (a) Cl₂(g) is added to the system. The equilibrium will shift toward reactant and Keq will decrease. (b) The reaction mixture is cooled. ---Select--- (c) The volume of the reaction vessel is reduced by 50%. ---Select--- (d) A catalyst is added to the reaction mixture. ---Select--- (e) The total pressure of the system is increased by adding a noble gas. ---Select--- (f) SO₂(g) is removed from the system. ---Select---
Consider the following equilibrium for which AH = -84.9: SO₂(g) + Cl₂(g) = SO₂Cl₂(9) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction? (a) Cl₂(g) is added to the system. The equilibrium will shift toward reactant and Keq will decrease. (b) The reaction mixture is cooled. ---Select--- (c) The volume of the reaction vessel is reduced by 50%. ---Select--- (d) A catalyst is added to the reaction mixture. ---Select--- (e) The total pressure of the system is increased by adding a noble gas. ---Select--- (f) SO₂(g) is removed from the system. ---Select---
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![## Equilibrium Analysis of SO₂(g) + Cl₂(g) ⇌ SO₂Cl₂(g)
### Consider the following equilibrium for which ΔH = -84.9:
**Reaction:**
\[ \text{SO}_2(\text{g}) + \text{Cl}_2(\text{g}) \rightleftharpoons \text{SO}_2\text{Cl}_2(\text{g}) \]
### How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?
1. **(a) Cl₂(g) is added to the system.**
- **Effect:** The equilibrium will shift toward the reactant and Keq will decrease.
- **Selection:** Drop-down menu to choose the effect.
2. **(b) The reaction mixture is cooled.**
- **Effect:** [Select from drop-down menu]
3. **(c) The volume of the reaction vessel is reduced by 50%.**
- **Effect:** [Select from drop-down menu]
4. **(d) A catalyst is added to the reaction mixture.**
- **Effect:** [Select from drop-down menu]
5. **(e) The total pressure of the system is increased by adding a noble gas.**
- **Effect:** [Select from drop-down menu]
6. **(f) SO₂(g) is removed from the system.**
- **Effect:** [Select from drop-down menu]
### Explanation:
- **Graphical/Diagram Description:**
- No explicit graphs or diagrams are provided. The problem set is textual, focusing on chemical equilibrium shifts based on Le Chatelier's principle.
This exercise involves understanding how changes in concentration, temperature, pressure, and the presence of catalysts affect the position of chemical equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2Ff8127e3e-8723-4ad3-94d1-4a6c0d5fcc61%2F5qagq_processed.png&w=3840&q=75)
Transcribed Image Text:## Equilibrium Analysis of SO₂(g) + Cl₂(g) ⇌ SO₂Cl₂(g)
### Consider the following equilibrium for which ΔH = -84.9:
**Reaction:**
\[ \text{SO}_2(\text{g}) + \text{Cl}_2(\text{g}) \rightleftharpoons \text{SO}_2\text{Cl}_2(\text{g}) \]
### How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?
1. **(a) Cl₂(g) is added to the system.**
- **Effect:** The equilibrium will shift toward the reactant and Keq will decrease.
- **Selection:** Drop-down menu to choose the effect.
2. **(b) The reaction mixture is cooled.**
- **Effect:** [Select from drop-down menu]
3. **(c) The volume of the reaction vessel is reduced by 50%.**
- **Effect:** [Select from drop-down menu]
4. **(d) A catalyst is added to the reaction mixture.**
- **Effect:** [Select from drop-down menu]
5. **(e) The total pressure of the system is increased by adding a noble gas.**
- **Effect:** [Select from drop-down menu]
6. **(f) SO₂(g) is removed from the system.**
- **Effect:** [Select from drop-down menu]
### Explanation:
- **Graphical/Diagram Description:**
- No explicit graphs or diagrams are provided. The problem set is textual, focusing on chemical equilibrium shifts based on Le Chatelier's principle.
This exercise involves understanding how changes in concentration, temperature, pressure, and the presence of catalysts affect the position of chemical equilibrium.
Expert Solution
Step 1 Theory
If concentration of any reactant or product is changed then equilibrium will shift in such a way to counteract the effect of change.
Increase in pressure shifts the equilibrium towards lesser number of moles.
If reaction is endothermic then increase in temperature increases the value of equilibrium constant.
If reaction is exothermic then decrease in temperature will increase the value of equilibrium constant.
Catalyst does not affect the equilibrium system.
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