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Question

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
1.267 mol L1
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B
0.267 mol L1
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C
1.967 mol L1
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D
2.967 mol L1
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Solution

The correct option is B 0.267 mol L1

PCl5PCl3+Cl2Initially: 2 0 0
Degree of dissociation: (α)=40 % =0.4
After dissociation,
Moles at equilibrium:
PCl5=2(2×0.4)=1.2 molPCl3=2×α=0.8 molCl2=2×α=0.8 mol
so,
PCl5PCl3+Cl2
At
equilibrium: 1.2 0.8 0.8
as Concentration=MolesVolume[PCl5]=1.22=0.6 mol L1[PCl3]=0.82=0.4 mol L1[Cl2]=0.82=0.4 mol L1

Kc=[PCl3][Cl2][PCl5]
=0.4×0.40.6
=1.66=0.83
=0.267 mol L1


Theory:

Writing Kc:

Example 1:
N2(g)+3H2(g)2NH3(g)
Kc=[NH3]2eq[N2]eq[H2]3eq

Example 2:
12H2(g)+12I2HI(g)

Kc=[HI]eq[H2]12eq[I2]12eq


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