For the reaction PCl_{5(g)} rightleftharpoons | vedclass

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(C) According to Le Chatelier's principle:$(1)$ Adding an inert gas at constant volume does not change the partial pressures of the reactants or produ

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$(3), (4), (5)$

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(C) According to Le Chatelier's principle:$(1)$ Adding an inert gas at constant volume does not change the partial pressures of the reactants or products,so the equilibrium remains unaffected.$(2)$ Adding $Cl_{2(g)}$ at constant volume increases the concentration of the product,which shifts the equilibrium in the backward direction.$(3)$ Adding an inert gas at constant pressure increases the total volume of the system,which decreases the partial pressure of each gas. Since the number of moles of products $(2)$ is greater than the number of moles of reactants $(1)$,the equilibrium shifts in the forward direction.$(4)$ Increasing the volume of the container decreases the total pressure. According to Le Chatelier's principle,the equilibrium shifts towards the side with more moles of gas,which is the product side (forward direction).$(5)$ Adding $PCl_{5(g)}$ at constant volume increases the concentration of the reactant,which shifts the equilibrium in the forward direction.Therefore,the forward reaction is favored by $(3), (4),$ and $(5)$.

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