For the reaction CO_{(g)} + H_2O_{(g)} rightl | vedclass

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(D) According to Le Chatelier's principle,if the concentration of one of the reactants is increased,the equilibrium shifts in the forward direction to

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Increasing the amount of $CO_{(g)}$

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(D) According to Le Chatelier's principle,if the concentration of one of the reactants is increased,the equilibrium shifts in the forward direction to counteract the change.Since $CO_{(g)}$ is a reactant,increasing its amount will shift the equilibrium to the right,thereby increasing the production of the products $CO_{2(g)}$ and $H_{2(g)}$.Adding a catalyst does not change the equilibrium position.Adding an inert gas at constant volume has no effect on the equilibrium.Decreasing the volume of the container has no effect on this reaction because the total number of moles of gaseous reactants equals the total number of moles of gaseous products $(1 + 1 = 1 + 1)$.

For the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ at a given temperature,the equilibrium amount of $CO_{2(g)}$ can be increased by

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