Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [HCl]_eq = 0.13 mol L^-1, [HI]_eq = 5.6 × 10^-16 mol L^-1, [Cl₂]_eq = 0.0019 mol L^-1. 2HCl(g) + I₂(s) ⇌ 2HI(g) + Cl₂(g)

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the reaction is Kc = [HI]^2[Cl2]/[HCl]^2. Plugging in the given concentrations: Kc = (5.6 × 10^-16)^2 * (0.0019) / (0.13)^2 = 3.5 × 10^-32 M.

Determine the Value of Kc for the Following Reaction If

Determine the Value of K_c for the Following Reaction If