Suppose the reaction PCl_{5(s)} rightleftharp | vedclass

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(C) The reaction is $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$.Since $PCl_{5(s)}$ and $PCl_{3(s)}$ are in the solid state,their active mas

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(C) The reaction is $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$.Since $PCl_{5(s)}$ and $PCl_{3(s)}$ are in the solid state,their active masses are taken as $1$.The equilibrium constant expression is $K_c = [Cl_{2(g)}]$.Because the equilibrium constant $K_c$ depends only on temperature,and the temperature is constant,the concentration of $Cl_{2(g)}$ at equilibrium remains unchanged regardless of the amount of solid $PCl_5$ added,provided some solid is present.

Suppose the reaction $PCl_{5(s)} \rightleftharpoons PCl_{3(s)} + Cl_{2(g)}$ is in a closed vessel at equilibrium. What is the effect on the equilibrium concentration of $Cl_{2(g)}$ by adding $PCl_{5(s)}$ at constant temperature?

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