For the given endothermic reaction,

$A (g) ⇌ 2 B (g)$

The variation in concentration due to different changes is plotted. In column II various changes are given and you are supposed to match the entries in column I with possible changes the system has undergone.

Neglect the slope of change in concentration when the system approaches equilibrium. Assume that changes are carried out very fast.

Column-I
Column-II (The effect is)
(P) Effect - I
(1) Addition of inert gas at constant pressure
(Q) Effect - II
(2) Decrease in total equilibrium pressure by changing the volume
(R) Effect - III
(3) Decreases in temperature at constant volume
(S) Effect - IV
(4) Addition of B only at constant volume

P - 3, Q - 4, R - 1, S - 2

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P - 1, Q - 2, R - 4, S - 3

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P - 4, Q - 2, R - 3, S - 1

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P - 3, Q - 1, R - 2, S - 4

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Solution

The correct option is D $P - 3, Q - 1, R - 2, S - 4$
Effect I correspond to a decrease in temperature at constant volume. The reaction will proceed in the backward direction, the reactant concentration will increase and the product concentration will decrease.
Effect II corresponds to the addition of inert gas at constant pressure. The equilibrium will remain unaffected and the concentrations of A and B will not be affected by this change.
Effect III corresponds to a decrease in total equilibrium pressure by changing the volume. The equilibrium will shift in the forward direction so that the pressure increases.
Effect IV corresponds to the addition of B only at constant volume. The reaction will proceed in the backward direction, the reactant concentration will increase and the product concentration will decrease.

Therefore, the correct option is $D$

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List-II

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Column-I	Column-II (The effect is)
(P) Effect - I	(1) Addition of inert gas at constant pressure
(Q) Effect - II	(2) Decrease in total equilibrium pressure by changing the volume
(R) Effect - III	(3) Decreases in temperature at constant volume
(S) Effect - IV	(4) Addition of B only at constant volume