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(B) The given reaction is $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$.Since the reaction is endothermic,increasing the temperature will shif

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Adding $He$ to the system at constant pressure

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(B) The given reaction is $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$.Since the reaction is endothermic,increasing the temperature will shift the equilibrium to the right,increasing the degree of dissociation.According to Le Chatelier's principle,adding an inert gas like $He$ at constant pressure increases the volume of the system.This decrease in partial pressure of the reactants and products shifts the equilibrium toward the side with more moles of gas.In this reaction,the product side has $2$ moles of gas ($CO$ and $Cl_2$) while the reactant side has $1$ mole of gas $(COCl_2)$.Therefore,adding $He$ at constant pressure shifts the equilibrium to the right,increasing the degree of dissociation of $COCl_2$.

The dissociation of phosgene,which occurs according to the reaction $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$,is an endothermic process. Which of the following will increase the degree of dissociation of $COCl_2$?

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