Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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![### Chemical Equilibrium and Temperature Changes
**5. Consider the following reaction at equilibrium:**
\[ \text{M} + \text{N} \rightleftharpoons \text{Q} + \text{R} \quad \Delta H = +350 \text{ kJ} \]
---
#### **Questions:**
**a) What would happen to this system if it was placed in an ice water bath? Explain your reasoning.**
**b) What would happen to this system if it was placed in a hot water bath? Explain your reasoning.**
---
### Explanation:
#### a) Effect of an Ice Water Bath:
Placing the system in an ice water bath effectively lowers the temperature. According to Le Chatelier's Principle, if a stress is applied to a system at equilibrium, the system will shift in a direction to relieve that stress. In this context, lowering the temperature will cause the endothermic reaction (which absorbs heat) to decrease in rate. As a result, the equilibrium will shift to the left to favor the exothermic direction (reverse reaction).
**Reasoning:**
Lowering temperature decreases the rate of the endothermic forward reaction (M + N → Q + R), which requires heat input. Therefore, equilibrium shifts to the left, favoring the formation of reactants (M and N).
#### b) Effect of a Hot Water Bath:
Placing the system in a hot water bath increases the temperature. According to Le Chatelier's Principle, increasing the temperature will cause the equilibrium to shift in a direction that absorbs heat, which in this case, is the endothermic forward reaction.
**Reasoning:**
Raising temperature increases the rate of the endothermic forward reaction (M + N → Q + R), which absorbs heat (+350 kJ). Therefore, equilibrium shifts to the right, favoring the formation of products (Q and R).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdabc7e8b-d42d-4c7a-8b8c-eac102cb510a%2Ffaa19637-0b19-402a-8059-e85ea3b256d9%2F0vo3ano_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium and Temperature Changes
**5. Consider the following reaction at equilibrium:**
\[ \text{M} + \text{N} \rightleftharpoons \text{Q} + \text{R} \quad \Delta H = +350 \text{ kJ} \]
---
#### **Questions:**
**a) What would happen to this system if it was placed in an ice water bath? Explain your reasoning.**
**b) What would happen to this system if it was placed in a hot water bath? Explain your reasoning.**
---
### Explanation:
#### a) Effect of an Ice Water Bath:
Placing the system in an ice water bath effectively lowers the temperature. According to Le Chatelier's Principle, if a stress is applied to a system at equilibrium, the system will shift in a direction to relieve that stress. In this context, lowering the temperature will cause the endothermic reaction (which absorbs heat) to decrease in rate. As a result, the equilibrium will shift to the left to favor the exothermic direction (reverse reaction).
**Reasoning:**
Lowering temperature decreases the rate of the endothermic forward reaction (M + N → Q + R), which requires heat input. Therefore, equilibrium shifts to the left, favoring the formation of reactants (M and N).
#### b) Effect of a Hot Water Bath:
Placing the system in a hot water bath increases the temperature. According to Le Chatelier's Principle, increasing the temperature will cause the equilibrium to shift in a direction that absorbs heat, which in this case, is the endothermic forward reaction.
**Reasoning:**
Raising temperature increases the rate of the endothermic forward reaction (M + N → Q + R), which absorbs heat (+350 kJ). Therefore, equilibrium shifts to the right, favoring the formation of products (Q and R).
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