2 mol of PCl5 were heated to 327oC in a closed 2 L vessel and when equilibrium was achieved, PCl5 was found to be 40% dissociated into PCl3 and Cl2. Calculate the equilibrium constant (KC) for the reaction
A
1.267molL−1
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B
0.267molL−1
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C
1.967molL−1
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D
2.967molL−1
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Solution
The correct option is B0.267molL−1
PCl5⇌PCl3+Cl2Initially:200
Degree of dissociation: (α)=40 %=0.4
After dissociation,
Moles at equilibrium: PCl5=2−(2×0.4)=1.2molPCl3=2×α=0.8molCl2=2×α=0.8mol
so, PCl5⇌PCl3+Cl2
At
equilibrium: 1.20.80.8
as Concentration=MolesVolume[PCl5]=1.22=0.6molL−1[PCl3]=0.82=0.4molL−1[Cl2]=0.82=0.4molL−1