The gas phase reaction 2NO_{2(g)} rightleftha | vedclass

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Question

(A) The decomposition reaction is $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.Since the forward reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ i

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addition of an inert gas at constant pressure

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(A) The decomposition reaction is $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.Since the forward reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is exothermic,the reverse reaction (decomposition) is endothermic.According to Le Chatelier's principle:$(a)$ Addition of an inert gas at constant pressure increases the total volume of the system,which shifts the equilibrium towards the side with a greater number of moles of gas. Here,the product side $(2NO_2)$ has more moles than the reactant side $(N_2O_4)$,so the decomposition of $N_2O_4$ increases.$(b)$ Lowering the temperature favors the exothermic direction,which is the formation of $N_2O_4$,not its decomposition.$(c)$ Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas,favoring the formation of $N_2O_4$.$(d)$ Addition of an inert gas at constant volume does not change the partial pressures of the reacting species,so it has no effect on the equilibrium.

The gas phase reaction $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is an exothermic reaction. The decomposition of $N_2O_4$ in an equilibrium mixture of $NO_{2(g)}$ and $N_2O_{4(g)}$ can be increased by:

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