At temperature T K, PCl5is 50% dissociated at an equilibrium pressure of 4 atm At what pressure it would - Chemistry - Equilibrium

Question

At temperature T K, PCl5is 50% dissociated at an
equilibrium pressure of 4 atm At what pressure it would dissociate
to the extent of 80% at the same temperature:-

a) 0 05 atm
​b) 0 60 atm
c) 0 75 atm
​d) 2 50 atm
​ Kindly answer sir/mam

Geetha · Accepted Answer

The given decomposition reaction is                            PCl5  ↔    PCl3    +    Cl2Initial moles         1                   0                 0 At eqm                   1-x             x               xTotal moles = 1-x + x +x = 1 +x Partial press         1-x1+x P     x1 + xP    x1 + xPKP = pPCl3 × pCl2pPCl5      = x1 + xP x1 + xP1-x1+x P  = x2 P12 - x2      = (0
5)2 × 41 - (0 5)2 =1
333      (since x = 50 % dissociation)For 80 % dissociation KP = x2 P12 - x2 1
33 = (0 8)2 × P1- (0
8)2P = 1 33 × 0 360 64 = 0
75 atmThe pressure required for 80 % dissociation = 0
75 atm
Option c is correct

At temperature T K, PCl5is 50% dissociated at an equilibrium pressure of 4 atm. At what pressure it would dissociate to the extent of 80% at the same temperature:- a) 0.05 atm ​b) 0.60 atm c) 0.75 atm ​d) 2.50 atm ​ Kindly answer sir/mam.

At temperature T K, PCl₅is 50% dissociated at an equilibrium pressure of 4 atm. At what pressure it would dissociate to the extent of 80% at the same temperature:-

a) 0.05 atm
b) 0.60 atm
c) 0.75 atm
d) 2.50 atm
Kindly answer sir/mam.