Question

Methanol is produced commercially by the catalysed reaction of carbon monoxide and hydrogen: CO(g) + 2H2(g)  CH3OH(g). An equilibrium mixture in a 2.00 L vessel is found to contain 0.0406 mol CH3OH, 0.170 mol CO, and 0.302 mol H2 at 500 K. Calculate Kp at this temperature.
(Answer = 6.22  10-3)

Answer 1

(CO) = mols/L = ?
(H2) = mols/L = ?
(CH3OH) = mols/L = ?

Substitue the concentrations into the Kc expression and sole for Kc. Convert to Kp by Kp = Kc(RT)^delta n. 6.22E-3 is the right answer.

Answer 2

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