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Question

At 473K, equilibrium constant, Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3×103. If decomposition is depicted as:
PCl5(g)PCl3(g)+Cl2(g);rH0=124.0kmol1 what would be the effect on reaction if the temperature is increased?

A
Reaction will shift in the backward direction.
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B
Reaction will shift in the forward direction.
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C
Reaction is equilibrium
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D
Reaction first moves forward and then remains at equilibrium.
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Solution

The correct option is B Reaction will shift in the forward direction.
The given reaction is :-
PCl5(g)PCl3(g)+Cl2(g);H0=124Kmol1
This reaction is endothermic reaction. So, if the temperature is increased then by applying Lechaterlier's principle, it can seen that forward reaction gets favoured.
So, more of PCl5 will get dissociated to form PCl3&Cl2.

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