A mixture of 2 mol CO & 2 mol water vapour is undergoing the water-gas shift reaction at a temperature of 1200 K and a pressure of 1 bar. CO (g) + H2O (g) → CO2 (g) + 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. b) The fractional dissociation of steam if the reactant steam is diluted with 4 mol nitrogen.

Question-Answer › Category: Chemical Thermodynamics › A mixture of 2 mol CO & 2 mol water vapour is undergoing the water-gas shift reaction at a temperature of 1200 K and a pressure of 1 bar. CO (g) + H2O (g) → CO2 (g) + 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. b) The fractional dissociation of steam if the reactant steam is diluted with 4 mol nitrogen.

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GCT asked 1 year ago

A mixture of 2 mol CO & 2 mol water vapour is undergoing the water-gas shift reaction at a
temperature of 1200 K and a pressure of 1 bar.

CO (g) + H2O (g) → CO2 (g) + 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. b) The fractional dissociation of steam if the
reactant steam is diluted with 4 mol nitrogen.

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