H2 (g) + CO2 (g) + 10 kcal H2O (g) + CO (g)

In another experiment involving the above reaction at 1,000°C, the equilibrium concentrations were found to be:

H2 (g) = 2.0 moles per liter

H2O (g) = 4.0 moles per liter

CO2 (g) = 5.0 moles per liter

CO (g) = 4.0 moles per liter

What is the equilibrium constant, Keq, for this reaction?

Question

Chemistry

Joshua Bauer

10 February, 05:15

H2 (g) + CO2 (g) + 10 kcal H2O (g) + CO (g)

In another experiment involving the above reaction at 1,000°C, the equilibrium concentrations were found to be:

H2 (g) = 2.0 moles per liter

H2O (g) = 4.0 moles per liter

CO2 (g) = 5.0 moles per liter

CO (g) = 4.0 moles per liter

What is the equilibrium constant, Keq, for this reaction?

+5

Answers (1)

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Blevins · Answer 1

The equilibrium contant for the reaction is 1.6. Solution: [H2]=2.0 mol/L [CO2] = 5.0 mol/L [H2O] = 4.0 mol/L [CO] = 4.0 mol/L K = [H2O][CO] / [H2][CO2] K = (4.0) (4.0) / (2.0) (5.0) K = 1.6 Ans [ = 1.6 ]