Question

Calculate the equilibrium constant, Kc, for the reaction:2SO2(g) + O2(g) ⇌ 2SO3(g) at a temperature of 600 K, given that the initial concentrations of SO2, O2, and SO3 were 0.025 M, 0.014 M, and 0 M, respectively, and at equilibrium [SO2] = 0.015 M, [O2] = 0.008 M, and [SO3] = 0.025 M.

Answer 1

To calculate the equilibrium constant, Kc, for the given reaction, we need to use the equilibrium concentrations of the reactants and products. The general expression for Kc for this reaction is:Kc = [SO3]^2 /  [SO2]^2 * [O2] At equilibrium, the concentrations are given as [SO2] = 0.015 M, [O2] = 0.008 M, and [SO3] = 0.025 M. Plugging these values into the Kc expression, we get:Kc =  0.025 ^2 /   0.015 ^2 *  0.008  Kc = 0.000625 /  0.000225 * 0.008 Kc = 0.000625 / 0.0000018Kc  347.22Therefore, the equilibrium constant, Kc, for the given reaction at 600 K is approximately 347.22.