The chemical equation for the *water-gas shift reaction* is CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g). What is the value of molal equilibrium constant Kp at 700 K if the partial pressures in an equilibrium mixture at 700 K are 1.31 atm of CO, 10.0 atm of water, 6.12 atm of carbon dioxide, and 20.3 atm of hydrogen gas?

Given:

Partial pressure of CO = 1.31 atm

Partial pressure of water = 10.0 atm

Partial pressure of carbon dioxide = 6.12 atm

Partial pressure of hydrogen gas = 20.3 atm

Step 2

The ratio of mathematical product of equilibrium partial pressure of products to the mathematical product of equilibrium partial pressure of reactants raised to power equal to their stoichiometric coefficient in the balanced chemical equation is known as equilibrium constant (Kp).

The given reaction is:

CO(g) + H2O(g) ⇌ CO2(g) + H2(g)

The equilibrium constant (Kp) expression for the reaction is:

Substitute the given values in equation (1).

Therefore, the value of molal equilibrium constant Kp at 700 K is **9.48.**