### 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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. Consider the following reaction at equilibrium: M + N Q + R AH = + 350 kJ

Chemistry

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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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Question

### 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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