At 35ºC, the equilibrium constant for the reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) is K_c = 1.6 * 10^-5. An equilibrium mixture was found to have the following concentrations of Cl₂ and NOCl: [Cl₂] = 1.2 * 10^-2 M; [NOCl] = 2.8 * 10^-1 M. Calculate the concentration of NO(g) at equilibrium.

Question

Quizplus · Accepted Answer

Given the equilibrium constant (Kc) and the concentrations of Cl2 and NOCl, we can use the stoichiometry of the reaction to find the concentration of NO. Since the reaction produces 2 moles of NO for every mole of Cl2 produced, the concentration of NO will be twice that of Cl2 at equilibrium. Given [Cl2] = 1.2 x 10^-2 M, the concentration of NO will be 2 x 1.2 x 10^-2 M = 2.4 x 10^-2 M, which matches option B.

At 35ºC, the Equilibrium Constant for the Reaction 2NOCl(g) ⇌\rightleftharpoons⇌ 2NO(g) + Cl2(g) Is Kc = 1

At 35ºC, the Equilibrium Constant for the Reaction 2NOCl(g) $\rightleftharpoons$ 2NO(g) + Cl₂(g) Is K_c = 1