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

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(D) The given reaction is $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$.$1$. Adding a catalyst does not change the equilibrium posit

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

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(D) The given reaction is $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$.$1$. Adding a catalyst does not change the equilibrium position; it only speeds up the rate of reaching equilibrium.$2$. Adding an inert gas at constant volume has no effect on the equilibrium. At constant pressure,since $\Delta n_g = (1+1) - (1+1) = 0$,adding an inert gas also has no effect.$3$. Decreasing the volume of the container increases the pressure,but for reactions where $\Delta n_g = 0$,the equilibrium position remains unchanged.$4$. According to Le Chatelier's principle,increasing the concentration of a reactant $(CO_{(g)})$ shifts the equilibrium in the forward direction,thereby increasing the amount of products ($CO_{2(g)}$ and $H_{2(g)}$).

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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