At 25 , ^oC,the equilibrium SO_2Cl_2(g) right | vedclass

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(A) According to Le Chatelier's Principle,if a system at equilibrium is subjected to a change in concentration,the system will shift in a direction th

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$1, 3$

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(A) According to Le Chatelier's Principle,if a system at equilibrium is subjected to a change in concentration,the system will shift in a direction that counteracts the change.When $Cl_2(g)$ is added to the equilibrium mixture,the concentration of the product increases.To counteract this,the equilibrium shifts to the left (backward direction).As a result,$SO_2(g)$ reacts with $Cl_2(g)$ to form more $SO_2Cl_2(g)$.Therefore,the concentration of $SO_2$ decreases and the concentration of $SO_2Cl_2$ increases.Statement $(1)$ is true because the concentrations of both $SO_2$ and $SO_2Cl_2$ change.Statement $(3)$ is true because the backward reaction consumes $SO_2$ and produces $SO_2Cl_2$.Statement $(2)$ is false because adding $Cl_2$ shifts the equilibrium to the left,consuming $Cl_2$ rather than producing more.

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