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Question

For the reaction:
AB(g)A(g)+B(g)
AB is 33% dissociated at a total pressure of p. Then pKp will be equal to :

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Solution

Let Pi= initial pressure of AB. Also, let x be the change in pressure of AB to reach equilibrium. The equilibrium pressure of AB will be
Pix. The equilibrium pressures of A and B will be x and x respectively.
The total pressure is p=(Pix)+x+x
p=(Pi+x).....(1)
AB is 33% dissociated at a total pressure of p
So x= 33 100 ×Pi=0.33Pi....(2)
Substitute this in equation (1)
p=(Pi+0.33Pi)
p=1.33Pi
Pi=p1.33
Substitute this in equation (2)
x=0.33Pi
x=0.33×p1.33
x=0.248p
The equilibrium pressures of A and B will be 0.248 p and 0.248 p respectively.
The equilibrium pressure of AB will be Pix=p1.330.248p=0.504p
Kp=PAPBPAB
Kp=0.248p×0.248p0.504p
Kp=0.248p×0.248p0.504p
Kp=0.122p
pKp=10.122=8

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