Question

For the reaction 2H₂S(g) ⇌ 2H₂(g) + S₂(g), with Kc = 1.67×10⁻⁷ at 800°C, the equilibrium favors:

a) Formation of H₂S
b) Decomposition of H₂S
c) Formation of H₂ and S₂
d) Decomposition of H₂ and S₂

Answer 1

The equilibrium favors the decomposition of H2S into H2 and S2.

Step-by-step explanation:

The equilibrium favors: b) Decomposition of H2S.

To determine which direction the equilibrium favors, we can look at the value of the equilibrium constant, Kc. In this case, Kc is very small (1.67×10⁻⁷). A small Kc value indicates that there are very few products compared to reactants at equilibrium. Therefore, the reaction favors the formation of reactants, which is the decomposition of H2S into H2 and S2.