Question

The water-gas shift reaction CO(g)+H2O(g)⇌CO2(g)+H2(g) is used industrially to produce hydrogen. The reaction enthalpy is ΔH∘=−41kJ.Part A

To increase the equilibrium yield of hydrogen would you use high or low temperature?
Drag the terms on the left to the appropriate blanks on the right to complete the sentences
high
exothermic
low
endothermic
decreasing
increasing
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Part 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 H2(g)?
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 ?A) Yes. Low pressure would favor formation of H2(g).
B) Yes. High pressure would favor formation of H2(g).
C) No. We cannot increase the equilibrium yield of hydrogen by controlling the pressure of this reaction.

Answer 1

The answers are in the explanation

Step-by-step explanation:

A. For the reaction:

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g); ΔH°=−41kJ.

As the reaction is exothermic ( ΔH°<0), you need to use low temperature to increase the equilibrium yield of hydrogen -LeChatelier's principle-.

We would use low temperature. For an exothermic reaction such as this, decreasing temperature increases the value of K and the amount of products at equilibrium.

B.

c. No. We cannot increase the equilibrium yield of hydrogen by controlling the pressure of this reaction.

It is possible to increase the equilibrium yield of reaction by controlling the amount of reactants added. As reactants and products are gases, the pressure of the reaction will not change the amount of reactants or products in the equilibrium.

I hope it helps!