Question

Consider the following equilibrium reaction at a given temperature: A (aq) + 3B (aq) ⇌ 3C (aq) + D (aq) Kc = 0.259 If initially the concentrations of the reactants and products are as follows: [A]0 = 0.332 M [B]0 = 0.802 M [C]0 = 0.692 M [D]0 = 0.707 M to which direction will the reaction run to reach equilibrium?

The answer choices are:

A. The reaction runs to the right because Q_c > K_c

B. The reaction runs to the right because Q_c < K_c

C. The reaction runs to the left because Q_c < K_c

D. The reaction is at equilibrium because Q_c = K_c

E. The reaction runs to the left because Q_c > K_c

_{I keep getting my Q value to be larger than the K value but the answer is B}

Answer 1