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

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(C) The given reaction is $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$.According to Le Chatelier's principle,the equilibrium shifts in the d

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Adding an inert gas at constant pressure

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(C) The given reaction is $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$.According to Le Chatelier's principle,the equilibrium shifts in the direction that counteracts the change.Adding an inert gas at constant volume does not change the partial pressures of the reacting species,so the equilibrium remains unaffected.Adding $Cl_2$ (a product) increases the concentration of the product,which shifts the equilibrium in the backward direction.Adding an inert gas at constant pressure increases the total volume of the system.Since the number of moles of gaseous products $(2)$ is greater than the number of moles of gaseous reactants $(1)$,increasing the volume shifts the equilibrium towards the side with more moles of gas,which is the forward direction.

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,at constant temperature,the reaction proceeds in the forward direction by:

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