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At 473K, equilibrium constant, K(c) for ...

At 473K, equilibrium constant, `K_(c)` for decomposition of phosphorus pentachloride, `PCl_(5)` is `8.3xx10^(-3)`. If decomposition is depicted as :
`PCl_(5(g))hArrPCl_(3(g))+Cl_(2(g)),Delta_(r)H^(@)=124.0" kJ mol"^(-1)`
what would be the effect on reaction if the temperature is increased ?

A

Reaction will shift in the backward direction.

B

Reaction will shift in the forward direction.

C

Reaction is in equilibrium.

D

Reaction first moves forward and then remains at equilibrium.

Text Solution

Verified by Experts

The correct Answer is:
B
`K_(c)=([PCl_(3(g))][Cl_(2(g))])/([PCl_(5(g))])`
As the reaction is endothermic, the increase in temperature will favour the forward reaction. More `PCl_(5)` will dissociate to from `PCl_(3)and Cl_(2)`.
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