In which of the following reactions will the | vedclass

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(D) According to Le Chatelier's principle,an increase in pressure shifts the equilibrium towards the side with a smaller number of gaseous moles.For o

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$CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_2O_{(g)}$

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(D) According to Le Chatelier's principle,an increase in pressure shifts the equilibrium towards the side with a smaller number of gaseous moles.For option $A$: $\Delta n_g = 2 - (1+1) = 0$. Pressure has no effect.For option $B$: $\Delta n_g = (1+1) - (1+1) = 0$. Pressure has no effect.For option $C$: $\Delta n_g = (1+1) - 1 = 1$. Equilibrium shifts backward.For option $D$: $\Delta n_g = (1+1) - (1+3) = 2 - 4 = -2$. Since $\Delta n_g < 0$,the number of moles decreases in the forward direction. Therefore,increasing the pressure will increase the yield of the product.

In which of the following reactions will the yield of the product increase with an increase in pressure?

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