Question

A mixture of 1 mole of H₂O and 1 mole of CO is taken in a 10 liter container and heated to 725 K. At equilibrium, 10 M of water by mass reacts with carbon monoxide according to the equation: \[ CO(g) + H_2O(g) \rightleftharpoons CO_2(g) + H_2(g) \] The equilibrium constant \( K_c \times 10^7 \) for the reaction is ______

Hint:

To calculate the equilibrium constant, use the relationship between the concentrations of the products and reactants at equilibrium.

Answer 1

Correct Answer: 44

From the given equation, the change in concentrations is: \[ \text{At equilibrium} \quad 1 - 0.4 = 0.6 \quad 0.4 \quad 0.4 \] \[ K_c = \frac{0.4 \times 0.4}{0.6 \times 0.6} = \frac{0.16}{0.36} = 0.444 \approx 44 \] Thus, the equilibrium constant is \( 44 \times 10^7 \).