In a vessel,the following two systems are in | vedclass

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(C) $1$. According to Le Chatelier's principle,adding $CO$ to the second equilibrium $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$ will shift

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$PCl_5$ concentration decreases

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(C) $1$. According to Le Chatelier's principle,adding $CO$ to the second equilibrium $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$ will shift the equilibrium to the left to consume the added $CO$.$2$. This shift causes the concentration of $Cl_2$ to decrease.$3$. Now,consider the first equilibrium $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$. Since the concentration of $Cl_2$ has decreased,the system will shift to the right to produce more $Cl_2$ to restore equilibrium.$4$. As the first equilibrium shifts to the right,$PCl_5$ dissociates to form more $PCl_3$ and $Cl_2$.$5$. Consequently,the concentration of $PCl_5$ decreases.

In a vessel,the following two systems are in simultaneous equilibrium: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ and $COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$. If some $CO$ is added to the vessel at constant volume,then at the new equilibrium:

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