Question

Given the concentrations, calculate the equilibrium constant for this reaction: i2(g) + cl2(g) ⇌ 2icl(g). At equilibrium, the molar concentrations for reactants and products are found to be [i2] = 0.50 M, [cl2] = 0.60 M, and [icl] = 5.0 M. What is the equilibrium constant (Kc) for this reaction?

Answer 1

The equilibrium constant, Kc, for the given reaction can be calculated by using the molar concentrations of the reactants and products at equilibrium. In this case, the equilibrium constant is (5.0^2) / (0.50 * 0.60).

Step-by-step explanation:

The equilibrium constant, Kc, can be calculated using the concentrations of the reactants and products at equilibrium. In this reaction, i2(g) + cl2(g) ⇌ 2icl(g), the concentrations are given as [i2] = 0.50 M, [cl2] = 0.60 M, and [icl] = 5.0 M. The equilibrium constant, Kc, is calculated by using the molar concentrations of the products raised to the power of their stoichiometric coefficients, divided by the molar concentrations of the reactants raised to the power of their stoichiometric coefficients. Therefore, the equilibrium constant for this reaction is (5.0^2) / (0.50 * 0.60).