Consider the following equilibrium: 2 H₂(g) + S₂(g) ⇌ 2 H₂S(g) K_c = 1.08 × 10⁷ at 700°C (b) Does the equilibrium mixture contain mostly H₂ and S₂ or mostly H₂S?

Verified step by step guidance

1. Understand the equilibrium expression: For the reaction 2 H2(g) + S2(g) ⇌ 2 H2S(g), the equilibrium constant expression is Kc = [H2S]^2 / ([H2]^2[S2]).
2. Interpret the value of Kc: The equilibrium constant Kc = 1.08 × 10^7 is a very large number, indicating that at equilibrium, the concentration of the products (H2S) is much greater than the concentration of the reactants (H2 and S2).
3. Analyze the equilibrium position: A large Kc value suggests that the reaction strongly favors the formation of products. Therefore, the equilibrium mixture will contain mostly H2S.
4. Consider the implications of Kc: Since Kc is significantly greater than 1, the reaction proceeds almost to completion, meaning that the concentrations of H2 and S2 will be very low compared to H2S at equilibrium.
5. Conclude based on Kc: Given the large Kc value, the equilibrium mixture will predominantly consist of H2S, with very little H2 and S2 remaining.