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(A) The given reaction is $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$.For this reaction,the change in the number of moles of gaseous produc

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Dissociation decreases

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(A) The given reaction is $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$.For this reaction,the change in the number of moles of gaseous products and reactants is $\Delta n = (1 + 1) - 1 = 1$.According to Le Chatelier's principle,an increase in pressure shifts the equilibrium in the direction where the number of moles of gas decreases.Since $\Delta n > 0$,the forward reaction involves an increase in the number of moles of gas.Therefore,increasing the pressure will shift the equilibrium in the backward direction,which decreases the dissociation of $PCl_5$.

What is the effect of increasing pressure on the dissociation of $PCl_5$ according to the equation $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)} - x \ cal$?

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