For the reaction: ch3oh (g) ⇌ co (g) + 2h2 (g), with the equilibrium concentrations for [ch3oh]=0.20 m, [co]=0.44 m, and [h2]=2.7 m, determine the gas phase equilibrium constant (kp) at 400 0c?

Question

Kaylie Chambers

Chemistry

10 February, 02:51

For the reaction: ch3oh (g) ⇌ co (g) + 2h2 (g), with the equilibrium concentrations for [ch3oh]=0.20 m, [co]=0.44 m, and [h2]=2.7 m, determine the gas phase equilibrium constant (kp) at 400 0c?

+5

Answers (1)

Know the Answer?

Grant Morrow · Answer 1

The concentration equilibrium constant is calculated as:

Kc = [CO][H2]^2 / [CH3OH] = (0.44 M) (2.7 M) ^2 / (0.20 M) = 16.038 M^2

The degree of the reaction is the sum of the product coefficients minus that of the reactants: n = 1 (CO) + 2 (H2) - 1 (CH3OH) = 2

Then the pressure equilibrium constant is calculated as:

Kp = Kc * (RT) ^ (n) = (16.038 M^2) * [ (0.08206 atm/M-K) (673.15 K) ]^ (2) = 48,936.95 atm^2

Remember to use absolute temperature of 400+273.15 K, not the 400 C itself.