consider the following system at equilibrium where ah 108 kj and kc 129x10 2at 600 k coclzg cog

1. The reaction is endothermic (ΔH > 0), so when the temperature increases, the equilibrium will

Question

Consider the following system at equilibrium where ΔH = 108 kJ, and Kc = 1.29x10^-2, at 600 K: COCl2(g) ⇌ CO(g) + Cl2(g) If the temperature of the equilibrium system is suddenly increased: 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, already at equilibrium The concentration of Cl2 will: A. Increase B. Decrease C. Remain the same

          Consider the following system at equilibrium where ΔH = 108 kJ, and Kc = 1.29x10^-2, at 600 K:
COCl2(g) ⇌ CO(g) + Cl2(g)

If the temperature of the equilibrium system is suddenly increased:

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, already at equilibrium

The concentration of Cl2 will:
A. Increase
B. Decrease
C. Remain the same

Added by Kathryn T.

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