4. Consider the equilibrium below and predict the direction that the equilibrium will shift for each of the following change. C (s) + H;0 (g) + heat CO (g) + H2 (g) a) Cooling b) Removing CO (g) c) Adding H2 (g) d) Adding H;0 (g)
4. Consider the equilibrium below and predict the direction that the equilibrium will shift for each of the following change. C (s) + H;0 (g) + heat CO (g) + H2 (g) a) Cooling b) Removing CO (g) c) Adding H2 (g) d) Adding H;0 (g)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Equilibrium and Reaction Shift Analysis**
**Problem Statement:**
Consider the chemical equilibrium below and predict the direction that the equilibrium will shift for each of the following changes:
\[ \text{C (s) + H}_2\text{O (g) + heat} \rightleftharpoons \text{CO (g) + H}_2\text{ (g)} \]
**Changes to Consider:**
a) Cooling
b) Removing CO (g)
c) Adding H\(_2\) (g)
d) Adding H\(_2\)O (g)
**Explanation:**
- **Cooling:** Decreases the temperature. In an endothermic reaction (heat is a reactant), cooling shifts the equilibrium to the left to generate more heat.
- **Removing CO (g):** Reduces product concentration. The equilibrium shifts to the right to increase CO.
- **Adding H\(_2\) (g):** Increases product concentration. The equilibrium shifts to the left to reduce H\(_2\).
- **Adding H\(_2\)O (g):** Increases reactant concentration. The equilibrium shifts to the right to consume H\(_2\)O.
This analysis uses Le Châtelier's principle to predict the direction of the equilibrium shift for each perturbation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81ac168b-024d-494f-99de-3f3384ea3f4e%2F3d644092-0694-4e4f-8f40-3ea8c5756720%2Fz64edkl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium and Reaction Shift Analysis**
**Problem Statement:**
Consider the chemical equilibrium below and predict the direction that the equilibrium will shift for each of the following changes:
\[ \text{C (s) + H}_2\text{O (g) + heat} \rightleftharpoons \text{CO (g) + H}_2\text{ (g)} \]
**Changes to Consider:**
a) Cooling
b) Removing CO (g)
c) Adding H\(_2\) (g)
d) Adding H\(_2\)O (g)
**Explanation:**
- **Cooling:** Decreases the temperature. In an endothermic reaction (heat is a reactant), cooling shifts the equilibrium to the left to generate more heat.
- **Removing CO (g):** Reduces product concentration. The equilibrium shifts to the right to increase CO.
- **Adding H\(_2\) (g):** Increases product concentration. The equilibrium shifts to the left to reduce H\(_2\).
- **Adding H\(_2\)O (g):** Increases reactant concentration. The equilibrium shifts to the right to consume H\(_2\)O.
This analysis uses Le Châtelier's principle to predict the direction of the equilibrium shift for each perturbation.
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