The equilibrium SO_2Cl_{2(g)} rightleftharpoo | vedclass

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(A) When an inert gas is added to an equilibrium mixture at constant volume,the total pressure of the system increases,but the partial pressures of th

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$a, b, c, d$

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(A) When an inert gas is added to an equilibrium mixture at constant volume,the total pressure of the system increases,but the partial pressures of the reacting species remain unchanged.Since the partial pressures (and thus concentrations) of the reactants and products do not change,the reaction quotient $Q_c$ remains equal to the equilibrium constant $K_c$.Therefore,the equilibrium position does not shift.Consequently,the concentrations of $SO_2, Cl_2,$ and $SO_2Cl_2$ do not change,no additional chlorine is formed,the concentration of $SO_2$ is not reduced,and no additional $SO_2Cl_2$ is formed.All the given statements $(a), (b), (c),$ and $(d)$ are incorrect.

List-$I$ (Equilibrium)	List-$II$ (Conditions for the process)
$P. A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$ (Endothermic)	$1. \text{High temperature}$
$Q. 2AB_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{3(g)}$ (Exothermic)	$2. \text{Low temperature}$
$R. 2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ (Endothermic)	$3. \text{High temperature}$
	$4. \text{Low temperature}$
	$5. \text{Independent of pressure}$

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