Final answer:
At low to moderate pressures, the equilibrium state of the water-gas shift reaction is less influenced by pressure changes due to equal moles of gas on both sides of the reaction. Factors such as temperature and the equilibrium constant are more influential in determining the direction of the reaction.
Step-by-step explanation:
The student asked about the equilibrium state of the water-gas shift reaction at low to moderate pressures. According to Le Chatelier's principle, a change in pressure can shift a reaction's equilibrium
In the water-gas shift reaction represented by CO(g) + H₂O(g) → CO₂(g) + H₂(g), we see that there are two moles of gas on each side of the equation. Therefore, changes in pressure would not shift the reaction in either direction based on the mole ratio. However, at low to moderate pressures, less emphasis is placed on the shift due to pressure changes, and other factors such as temperature and the equilibrium constant (K) will have a more significant impact on which way the reaction proceeds.