# A mixture of 1 mol CO, and 1 mol of water vapour is undergoing the water gas shift reaction at a temperature of 1100K and a pressure of 1 bar. CO (g) + H2O (g) –> CO2 + H2 (g) The equilibrium constant for the reaction is K=1. Assume that the gas mixture behaves as ideal gas. Calculate (a) the fractional dissociation of steam.

Question-AnswerCategory: Chemical ThermodynamicsA mixture of 1 mol CO, and 1 mol of water vapour is undergoing the water gas shift reaction at a temperature of 1100K and a pressure of 1 bar. CO (g) + H2O (g) –> CO2 + H2 (g) The equilibrium constant for the reaction is K=1. Assume that the gas mixture behaves as ideal gas. Calculate (a) the fractional dissociation of steam.

A mixture of 1 mol CO, and 1 mol of water vapour is undergoing the water gas shift reaction at a temperature of 1100K and a pressure of 1 bar.
CO (g) + H2O (g) –> CO2 + H2 (g)
The equilibrium constant for the reaction is K=1. Assume that the gas mixture behaves as ideal gas. Calculate
(a) the fractional dissociation of steam.