Given the following equilibrium equations and their corresponding equilibrium constants:2 CO2 (g) + H2O (g) 2 O2 (g) + CH2CO (g) Kc = 6.1 x 10 8CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g) Kc = 1.2 x 1014Find Kc for the reaction: CH4 (g) + CO2 (g) CH2CO (g) + H2O (g)

The following equilibrium constants were determined at 1123 K: C (s) + CO2 (g) ⇌ 2CO (g) KC1 = 1.4 × 1012 CO (g) + Cl2 (g) ⇌ COCl2 (g) KC2 = 5.5 × 101 Write the equilibrium constant expression Kc and calculate the equilibrium constant at 1123 K for the following reaction. C (s) + CO2 (g) + 2Cl2 (g) ⇌2COCl2 (g)

The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq = 6.2 × 10-27.9262.72792 M.

The equilibrium constant, KC, for the following reaction is 2.5 × 10-3N2(g) + O2(g) ⇌ 2NO(g)If [N2]eq = 0.75 M and [NO]eq = 0.090, then [O2]eq

sessment3. Determine the correct expression for the equilibrium constant, Kc, for each reaction. Drag each formula to the correct column on the chart. All reactant and product concentrations are equilibrium concentrations.ReactionKcO2(l) ⇋ O2(g)2O3(g) ⇋ 3O2(g)2SO2(g) + O2(g) ⇋ 2SO3(g)2SO3(g) ⇋ 2SO2(g) + O2(g) Kc = [O2]3/ [O3]2Kc = [SO3]2 / [SO2]2 [O2]Kc = [SO2]2 [O2] / [SO3]2Kc = [O2]

The equilibrium constant, KC, for the following reaction at 726.85 °C is 2.71 × 102.2SO2(g) + O2(g) ⇌ 2SO3(g)The KP for this reaction at the same temperature is