A mixture at equilibrium at 400 K for the reaction C(g) ⇌ D(g) has [C] = 0.25 M and…
CHEMISTRY · Single correct · AP · Chemistry · Equilibrium · Equilibrium
Problem
A mixture at equilibrium at 400 K for the reaction C(g) ⇌ D(g) has [C] = 0.25 M and [D] = 1.00 M, consistent with K = 4.0 at that temperature. The temperature is then raised to 450 K, where the new equilibrium constant is K = 1.2. At the same moment, 0.50 M of D is rapidly removed, leaving [C] unchanged. Which statement best predicts the net direction of reaction as the system approaches the new equilibrium at 450 K?
(a) Q is now less than K, so the forward reaction is favored and [D] will increase.
(b) Q equals K, so the mixture remains at equilibrium with no net change.
(c) Q is now greater than K, so the reverse reaction is favored and [C] will increase.
(d) Q is now greater than K, so the forward reaction is favored and [C] will decrease.