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The gas phase reaction PCl(5)(g)<=> PCl...

The gas phase reaction `PCl_(5)(g)<=> PCl_(3)(g)+Cl_(2)(g)` is an endothermic reaction. The formation of `PCl_(5)` in equilibrium mixture of `PCl_(5)(g), PCl_(3)(g) and Cl_(2)(g)` can be decreased by :

A

Decreasing the temperature

B

Addition of an inert gas at constant pressure

C

Decreasing the volume

D

Addition of an inert gas at constant volume

Text Solution

Verified by Experts

The correct Answer is:
B

`to` By decreasing the temperature, reaction will proceed in backward direction as per Le-Chatelier’s principle.
`to` By adding inert gas at constant pressure, volume will increase, so Crowding will decrease so the reaction will proceed in that direction in which the crowding is more i.e. forward direction.
`to` When the volume is decreased, crowding increases due to which reaction proceeds backward as per Le – Chatelier’s principle.
`to` no effect.
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Knowledge Check

  • For the reaction : PCl_(5) (g) rarrPCl_(3) (g) +Cl_(2)(g) :

    A
    (a) Equal volumes of `PCl_(5),PCl_(3)andCl_(2)` are present.
    B
    (b) Equal masses of `PCl_(5),PCl_(3)andCl_(2)` are present.
    C
    (c) The concentrations of `PCl_(5),PCl_(3)andCl_(2)` become constant.
    D
    (d) Reaction stops

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