Consider the following system at equilibrium where H° = 108 kJ, and Kc = 1.29×10
ID: 487659 • Letter: C
Question
Consider the following system at equilibrium where H° = 108 kJ, and Kc = 1.29×10-2, at 600 K: COCl2(g) CO(g) + Cl2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: 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 restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Cl2 will: A. Increase. B. Decrease. C. Remain the same.
Explanation / Answer
H° = 108 kJ, and Kc = 1.29×10-2, at 600 K
This is an equilbrium of endothermic reaction
a) On lowering the Temperature: the value of Kc will decrease (Kc is Temperature Dependant)
b) If we decrease the temperature, the reaction will go in backward direction and hence there will be less concentration of products and more of reactants so the Qc will decrease
c) The reaction will run in backward direction to establish the equilbrium