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

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(A) According to Le Chatelier's principle,if a product $(Cl_2)$ is added to the system at equilibrium,the equilibrium will shift in the backward direc

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$1, 3$

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(A) According to Le Chatelier's principle,if a product $(Cl_2)$ is added to the system at equilibrium,the equilibrium will shift in the backward direction to counteract the change.$(1)$ The addition of $Cl_2$ leads to a change in the concentrations of all species ($SO_2$,$Cl_2$,and $SO_2Cl_2$) as the system re-establishes equilibrium.$(2)$ Since the reaction shifts backward,$Cl_2$ is consumed,not produced. Thus,statement $(2)$ is incorrect.$(3)$ As the reaction shifts backward,$SO_2$ reacts with $Cl_2$ to form more $SO_2Cl_2$. Therefore,the concentration of $SO_2$ decreases and the concentration of $SO_2Cl_2$ increases. Thus,statement $(3)$ is correct.Therefore,statements $(1)$ and $(3)$ are correct.

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