Consider the following system at equilibrium where ΔH° = -87.9 kJ, and Kc = 83.3, at 500 K.\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]If the VOLUME of the equilibrium system is suddenly increased at constant temperature:1. The value of Kc: - A. increases. - B. decreases. - C. remains the same.2. The value of Qc: - A. is greater than Kc. - B. is equal to Kc. - C. is less than Kc.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. It is already at equilibrium.4. The number of moles of Cl2 will: - A. increase. - B. decrease. - C. remain the same.Buttons available:- Submit Answer- Retry Entire Group(Note: "8 more group attempts remaining" is mentioned on the screen.)

Answered: Consider the following system at…

Consider the following system at equilibrium where AH =-87.9 kJ, and K. 83.3, at 500 K. PCI3(g) + C2(g) =PCL,(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature:

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

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Question

Consider the following system at equilibrium where ΔH° = -87.9 kJ, and Kc = 83.3, at 500 K.

\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]

If the VOLUME of the equilibrium system is suddenly increased at constant temperature:

1. The value of Kc:
- A. increases.
- B. decreases.
- C. remains the same.

2. The value of Qc:
- A. is greater than Kc.
- B. is equal to Kc.
- C. is less than Kc.

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. It is already at equilibrium.

4. The number of moles of Cl2 will:
- A. increase.
- B. decrease.
- C. remain the same.

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