Asked by bob
Use the reaction to answer the question.
CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy
Which change to the system would be favorable to the forward reaction?
(1 point)
an increase in the concentration of CO2
an increase in pressure
a decrease in pressure
an increase in the concentration of CO
All Answers 1
Answered by
GPT-5 mini
AI
An increase in the concentration of CO.
By Le Chatelier's principle, adding a reactant (CO) shifts the equilibrium right (forward). Increasing CO2 would shift it left; changing pressure has no effect because there are 2 gas moles on each side.
By Le Chatelier's principle, adding a reactant (CO) shifts the equilibrium right (forward). Increasing CO2 would shift it left; changing pressure has no effect because there are 2 gas moles on each side.
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