Which of the changes listed will shift the equilibrium to the right for the following reversible reaction? CO(g)+ H₂O(g) CO₂(g)+ H₂(g)+ heat

Question

Which of the changes listed will shift the equilibrium to the right for the following reversible reaction? CO(g)+ H₂O(g)  CO₂(g)+ H₂(g)+ heat

Quizplus · Accepted Answer

Le Chatelier's principle states that an increase in the concentration of a reactant will shift the equilibrium to the side with fewer moles of gas. In this case, increasing the concentration of CO will favor the forward reaction because it only has one mole of gas compared to the three moles of gas on the product side. The other options, such as increasing [CO2] or increasing temperature, would shift the equilibrium to the left, favoring the reverse reaction. Increasing the volume would have no effect since there are an equal number of moles of gas on both sides. Adding a catalyst would increase the rate of both the forward and reverse reactions, but would not affect the position of the equilibrium.

Which of the Changes Listed Will Shift the Equilibrium to the Right