Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2 O (g) ⇌ 3H2 (g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C?

Question

Amelie Brock

Chemistry

2 January, 21:04

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2 O (g) ⇌ 3H2 (g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C?

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Answers (1)

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Zander · Answer 1

6.28

Explanation:

Let's consider the following reaction at equilibrium.

CH₄ (g) + H₂O (g) ⇌ 3 H₂ (g) + CO (g)

The concentration equilibrium constant (Kc) is the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.

Kc = [H₂]³ * [CO] / [CH₄] * [H₂O]

Kc = 1.15³ * 0.126 / 0.126 * 0.242

Kc = 6.28