Chemical Engineering > GATE 2019 > Chemical Equilibrium
Carbon monoxide (CO) reacts with hydrogen sulphide (H2S) at a constant temperature of 800 K and a constant pressure of 2 bar as:
CO + H2S ⇌ COS + H2
The Gibbs free energy of the reaction Δg°rxn = 22972.3 J/mol and universal gas constant R=8.314 J/(mol K). Both the reactants and products can be assumed to be ideal gases. If initially only 4 mol of H2S and 1 mol of CO are present, the extent of the reaction (in mol) at equilibrium is ______ (rounded off to two decimal places).
CO + H2S ⇌ COS + H2
The Gibbs free energy of the reaction Δg°rxn = 22972.3 J/mol and universal gas constant R=8.314 J/(mol K). Both the reactants and products can be assumed to be ideal gases. If initially only 4 mol of H2S and 1 mol of CO are present, the extent of the reaction (in mol) at equilibrium is ______ (rounded off to two decimal places).
Correct : 0.28
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