Consider the following system at equilibrium where H° = -108 kJ, and Kc = 77.5,
ID: 951713 • Letter: C
Question
Consider the following system at equilibrium where H° = -108 kJ, and Kc = 77.5, at 600 K. CO(g) + Cl2(g) COCl2(g)
If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:
The value of Kc:
A. increases. B. decreases. C. remains the same.
The value of Qc:
A. is greater than Kc. B. is equal to Kc. C. is less than Kc.
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.
The number of moles of Cl2 will:
A. increase. B. decrease. C. remain the same.
Explanation / Answer
CO(g) + Cl2(g) ------------> COCl2(g)
If the VOLUME of the equilibrium system is suddenly decreased at constant temperature
The value of Kc remains the same
The value of Qc is less than Kc
The reaction must run in the forward direction to reestablish equilibrium
The number of moles of Cl2 will decrease.