Question

Calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ C(g) + D(g), if the concentration of A is 0.25 M, the concentration of B is 0.10 M, the concentration of C is 0.30 M and the concentration of D is 0.20 M at equilibrium.

Answer 1

To calculate the equilibrium constant  Kc  for the given reaction, we need to use the formula:Kc = [C]^c * [D]^d /  [A]â * [B]^b where [A], [B], [C], and [D] are the equilibrium concentrations of the respective species, and a, b, c, and d are the stoichiometric coefficients in the balanced chemical equation.For the reaction 2A g  + B g   C g  + D g , the stoichiometric coefficients are a = 2, b = 1, c = 1, and d = 1.Given the equilibrium concentrations:[A] = 0.25 M[B] = 0.10 M[C] = 0.30 M[D] = 0.20 MPlug these values into the Kc formula:Kc = [0.30]^1 * [0.20]^1 /  [0.25]^2 * [0.10]^1 Kc =  0.30 * 0.20  /  0.0625 * 0.10 Kc = 0.06 / 0.00625Kc  9.6Therefore, the equilibrium constant  Kc  for the given reaction is approximately 9.6.