Question

Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:
CO(g)+2H2(g)⇌CH3OH(g).
An equilibrium mixture in a 2.50 L vessel is found to contain 0.0243 mol CH3OH, 0.160 mol CO, and 0.301 mol H2 at 500 K.
Calculate Kc at this temperature.

Answer 1

Question #81895, Chemistry / General Chemistry | for completion

Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:

$\mathrm{CO(g) + 2H2(g)\rightleftharpoons CH3OH(g)}$

An equilibrium mixture in a 2.50 L vessel is found to contain 0.0243 mol CH3OH, 0.160 mol CO, and 0.301 mol H2 at 500 K.

Calculate Kc at this temperature.

Answer:

$\mathrm{C_{CH3OH} = 0.0243 mol / 2.5 L = 0.00972 M}$

$\mathrm{C_{CO} = 0.16 mol / 2.5 L = 0.064 M}$

$\mathrm{C_{H2} = 0.301 mol / 2.5 L = 0.1204 M}$

Formula: $K_{C} = C_{CH3OH} / C_{CO} \times (C_{H2})^{2}$

$K_{C} = 0.00972 / 0.064 \times (0.1204)^{2} = 10.48$

$K_{C} = 10.48$

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