Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M.
H₂(g) + I₂(g) ⇌ 2 HI(g)

Question

Determine the value of K_c for the following reaction if the equilibrium concentrations are as follows: [H₂]_eq = 0.14 M,[I₂]_eq = 0.39 M,[HI]_eq = 1.6 M. H₂(g)+ I₂(g)⇌ 2 HI(g)

Quizplus · Accepted Answer

The equilibrium constant expression for the reaction is: K_c = [HI]_eq / ([H₂]_eq x [I₂]_eq]) Substitute the given equilibrium concentrations into the expression: K_c = (1.6 M)_eq / [(0.14 M)_eq x (0.39 M)_eq] K_c = 46.86 ≈ 47 Therefore, the answer is choice C, 47.

Determine the Value of Kc for the Following Reaction If

Determine the Value of K_c for the Following Reaction If