One mole of H2O and one mole of CO are placed in a 10 L vessel and heated to 725 K. At equilibrium 40% of the water (by mass) has reacted with carbon monoxide: H2O(g) + CO(g) H2(g) + CO2(g). Find the equilibrium constant Kc for the reaction.

Question

One mole of H2O and one mole of CO are placed in a 10 L vessel and heated to 725 K. At equilibrium 40% of the water (by mass) has reacted with carbon monoxide: H2O(g) + CO(g) <=> H2(g) + CO2(g). Find the equilibrium constant Kc for the reaction.

Accepted Answer

4/9. With x = 0.4 reacted, equilibrium moles are H2O = 0.6, CO = 0.6, H2 = 0.4, CO2 = 0.4, giving Kc = (0.4*0.4)/(0.6*0.6) = 0.16/0.36 = 4/9.

One mole of H2O and one mole of CO are placed in a 10 L vessel and heated to 725 K. At equilibrium 40% of the water (by mass) has reacted with carbon monoxide: H2O(g) + CO(g) <=> H2(g) + CO2(g). Find the equilibrium constant Kc for the reaction.

Solution

Related JEE Advanced Chemistry questions