Methanol, ch3oh, is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen. co (g) + 2 h2 (g) equilibrium reaction arrow 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.

Question

Chemistry

Goober

30 July, 11:36

Methanol, ch3oh, is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen. co (g) + 2 h2 (g) equilibrium reaction arrow 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.

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Andreas Austin · Answer 1

6.0588 x 10⁻⁷.

Explanation:

For the reaction: CO + 2H₂ ↔ CH₃OH,

Kc = [products]/[reactants] = [CH₃OH]/[CO][H₂]².

[CH₃OH] = no. of moles/V = (0.0406 mol) / (2.0 L) = 0.0203 mol/L.

[CO] = no. of moles/V = (0.170 mol) / (2.0 L) = 0.085 mol/L.

[H₂] = no. of moles/V = (0.302 mol) / (2.0 L) = 0.151 mol/L.

∴ Kc = [CH₃OH]/[CO][H₂]² = (0.0203 mol/L) / (0.085 mol/L) (0.151 mol/L) ² = 10.47.

∵ Kp = Kc (RT) ∧Δn.

R is the general gas constant = 8.314 J/mol. K.

T is the temperature of the vessel = 500.0 K.

Δn = no. of moles of gases in products - no. of moles of gases in the reactants = 1 - 3 = - 2.

∴ Kp = Kc (RT) ∧Δn = (10.47) [ (8.314) (500.0) ]⁻² = 6.0588 x 10⁻⁷.