**Chemical Equilibrium and Temperature Influence**Consider the following system at equilibrium where \( \Delta H^\circ = -10.4 \, \text{kJ} \) and \( K_c = 55.6 \) at 698 K:\[\text{H}_2 (g) + \text{I}_2 (g) \rightleftharpoons 2 \text{HI} (g)\]**Question: Temperature Increase Impact**If the **temperature** on the equilibrium system is suddenly **increased**:1. **The value of \( K_c \)**: - A. Increases - B. Decreases - C. Remains the same2. **The value of \( Q_c \)**: - A. Is greater than \( K_c \) - B. Is equal to \( K_c \) - C. Is less than \( K_c \)3. **The reaction must**: - A. Run in the forward direction to reestablish equilibrium - B. Run in the reverse direction to reestablish equilibrium - C. Remain the same. Already at equilibrium4. **The concentration of \( \text{I}_2 \) will**: - A. Increase - B. Decrease - C. Remain the sameThese questions examine the concept of chemical equilibrium and how it responds to temperature changes according to Le Chatelier's principle. The reaction is exothermic, which means increasing temperature shifts the equilibrium to favor the endothermic direction (reverse reaction).

Answered: Image /qna-images/answer/c020ae03-6a5e-4ddd-87c9-d58fa73d7978.jpg

Consider the following system at equilibrium where AH° = -10.4 kJ, and K, = 55.6 , at 698 K: %3D H2 (g) + I2 (g)=2 HI (g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K, A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K. C. Is less than K. A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The reaction must: The concentration of I, will: A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium where AH° = -10.4 kJ, and K, = 55.6 , at 698 K: %3D H2 (g) + I2 (g)=2 HI (g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K, A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K. C. Is less than K. A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The reaction must: The concentration of I, will: A. Increase. B. Decrease. C. Remain the same.

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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