?The water-gas shift reaction \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g)
Chapter 15, Problem 15.68(choose chapter or problem)
The water-gas shift reaction \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons\) \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) is used industrially to produce hydrogen. The reaction enthalpy is \(\Delta H^{\circ}=-41 \mathrm{~kJ}\).
(a) To increase the equilibrium yield of hydrogen would you use high or low temperature?
(b) Could you increase the equilibrium yield of hydrogen by controlling the pressure of this reaction? If so would high or low pressure favor formation of \(\mathrm{H}_{2}(g)\) ?
Text Transcription:
CO(g)+H_2 O(g) \rightleftharpoons
CO_2(g)+H_2(g)
Delta H^circ=-41 kJ
H_2(g)
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