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Question

For the following reaction:
PCl5 (g)PCl3 (g)+Cl2 (g)
0.4 mol of PCl5 (g), 0.2 mol of PCl3 (g) and 0.6 mol of Cl2 (g) are taken in a 1 L flask.
If Kc=0.2, then the direction in which reaction proceeds is :

A
Towards reactant side
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B
Towards products side
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C
Reaction is at equilibrium
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D
None of the above
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Solution

The correct option is A Towards reactant side
Given Reaction is:
PCl5 (g)PCl3 (g)+Cl2 (g)
Concentration=MolesVolume
[PCl5]=0.41=0.4 M[PCl3]=0.21=0.2 M[Cl2]=0.61=0.6 M
Finding Qc
Qc=[PCl3][Cl2][PCl5]

puttting the values,
Qc=0.2×0.60.4=0.3 M>Kc(=0.2)
Since, Q>Kc the reaction proceeds in backward direction i.e. reactant (PCl5) side.

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