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 $SO_2$ (a product of the first equilibrium) will shift the first equilibrium $(SO_2Cl_{2(g)} \rightle

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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 $SO_2$ (a product of the first equilibrium) will shift the first equilibrium $(SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)})$ to the left.This results in a decrease in the concentration of $Cl_2$.Since $Cl_2$ is a reactant in the second equilibrium $(CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)})$,a decrease in $Cl_2$ concentration will shift the second equilibrium to the left.Consequently,the amount of $COCl_2$ will decrease,and the amount of $CO$ will increase.

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?