Answer to Question #286141 in Chemistry for khryst

Question

Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures.

CH₄ (g) + H₂O (g) ⇌ H₂ (g) + CO (g)

What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations, at a temperature of 760 °C?

CH₄ = 0.126 M

H₂O = 0.242 M

CO = 0.126 M

H₂ = 1.15 M

Answer 1

[CH₄] = 0.126 M

[H₂O] = 0.242 M

[CO] = 0.126 M

[H₂] = 1.15 M

Solution:

Balanced chemical equation:

CH₄(g) + H₂O(g) ⇌ 3H₂(g) + CO(g)

The equilibrium expression for the reaction system:

K_c = ([CO] × [H₂]³) / ([H₂O] × [CH₄])

K_c = (0.126 × 1.15³) / (0.242 × 0.126) = (0.19163) / (0.030492) = 6.28

K_c = 6.28 M²

Answer: The equilibrium constant (K_c) for the reaction is 6.28