Question

What is the equilibrium constant (Kc) expression for the reaction N2(g) + O2(g) ⇌ 2NO(g)? If the initial concentrations for N2, O2, and NO are 0.25 M, 0.15 M, and 0.05 M, respectively, what is the value of Kc for the reaction at equilibrium?

Answer 1

The equilibrium constant  Kc  expression for the reaction N2 g  + O2 g   2NO g  can be written as:Kc = [NO]^2 /  [N2] * [O2] To find the value of Kc at equilibrium, we need to know the equilibrium concentrations of N2, O2, and NO. The initial concentrations are given, but we need to determine the changes in concentration as the reaction proceeds to equilibrium.Let x be the change in concentration for N2 and O2, and 2x for NO. At equilibrium, the concentrations will be:[N2] = 0.25 - x[O2] = 0.15 - x[NO] = 0.05 + 2xNow, substitute these equilibrium concentrations into the Kc expression:Kc = [ 0.05 + 2x ^2] /  [ 0.25 - x  *  0.15 - x ] Unfortunately, without knowing the value of Kc or the equilibrium concentrations, we cannot solve for x and determine the value of Kc. Additional information is needed to solve this problem.