Given that the equilibrium concentrations of [N₂] = 0.035 M, [C₂H₂] = 0.057 M, and [HCN] = 6.8 × 10^-4 M, find the value of the equilibrium constant expression for the reaction:
N₂(g) + C₂H₂(g) ⇌ 2 HCN

Question

Quizplus · Accepted Answer

The equilibrium expression for the given reaction is: Kc = [HCN]^2 / [N₂] [C₂H₂] Substituting the given equilibrium concentrations: Kc = (6.8 × 10^-4)^2 / (0.035 M) (0.057 M) Kc = 2.3 × 10^-4 Therefore, the correct answer is D.

Given That the Equilibrium Concentrations of [N2] = 0

Given That the Equilibrium Concentrations of [N₂] = 0