On heating a mixture of SO_2Cl_2 and CO,two e | vedclass

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(D) According to Le Chatelier's principle,adding $SO_2$ to the first equilibrium $(SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)})$ will shift

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Amount of $SO_2Cl_2$ and $CO$ will increase

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(D) According to Le Chatelier's principle,adding $SO_2$ to the first equilibrium $(SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)})$ will shift the reaction in the backward direction.This leads to a decrease in the concentration of $Cl_{2(g)}$.Now,considering the second equilibrium $(CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)})$,a decrease in the concentration of $Cl_{2(g)}$ will shift this reaction in the backward direction to compensate for the loss.As a result,the amount of $CO_{(g)}$ will increase,and the amount of $COCl_{2(g)}$ will decrease.

On heating a mixture of $SO_2Cl_2$ and $CO$,two equilibria are simultaneously established:
$SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$
$CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$
On adding more $SO_2$ at equilibrium,what will happen?

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On heating a mixture of $SO_2Cl_2$ and $CO$,two equilibria are simultaneously established:$SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$$CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$On adding more $SO_2$ at equilibrium,what will happen?