Consider the following reaction: CH₄(g) + 2H₂S(g) ⇌ CS₂(g) + 4H₂(g)
A reaction mixture initially contains 0.50 mol L^-1 CH₄ and 0.75 mol L^-1 H₂S. If the equilibrium concentration of H₂ is 0.44 mol L^-1, find the equilibrium constant (mol L^-1) for the reaction.

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the given reaction is: Kc = [CS₂][H₂]^4/[CH₄][H₂]^2 Kc = [CS₂][H₂]^2/[CH₄] At equilibrium, the concentration of H₂ is 0.44 mol L^-1. Putting the values in the equilibrium constant expression, we get: Kc = [CS₂][0.44 mol L^-1]^2/[0.50 mol L^-1] Kc = 0.038 mol² L^-2 Therefore, the correct answer is B, 0.038 mol² L^-2.

Consider the Following Reaction: CH4(g) + 2H2S(g) ⇌ CS2(g)

Consider the Following Reaction: CH₄(g) + 2H₂S(g) ⇌ CS₂(g)