Consider the following system at equilibrium where Ho = 108 kJ, and Kc = 1.29E-2
ID: 628650 • Letter: C
Question
Consider the following system at equilibrium where Ho = 108 kJ, and Kc = 1.29E-2, at 600 K: COCl2(g) CO(g) + Cl2(g) When 0.19 moles of COCl2(g) are removed from the equilibrium system at constant temperature: The value of Kc 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 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 CO will: A. Increase. B. Decrease. C. Remain the same.Explanation / Answer
value of Kc remains same as it is a function of temperature so option C
value of Q is greater as Kc is inversely proporitonal to cocl2 and it decreases so Q increases so option A
run in backward to establish so as to lower Q to equalize Kc option B
CO will decrease as it runs in reverse direction option B