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Full question::::if a given quantity of phosphorus pentachloride was heated to 250 degree Celsius and allowed to come to equilibrium at atmospheric pressure it is found to be dissociated to the extent of 80% into Phosphorus trichloride and chlorine if now the pressure on this mixture is increased so that final equilibrium mixture occupy only one half of its original volume temperature maintained constant .a) what will be the percentage dissociation at the new pressure?b) what would be the effect of adding helium gas keeping the volume fixed at the V/2?😎

Full question::::if a given quantity of phosphorus pentachloride was heated to 250 degree Celsius and allowed to come to equilibrium at atmospheric pressure it is found to be dissociated to the extent of 80% into Phosphorus trichloride and chlorine if now the pressure on this mixture is increased so that final equilibrium mixture occupy only one half of its original volume temperature maintained constant .a) what will be the percentage dissociation at the new pressure?b) what would be the effect of adding helium gas keeping the volume fixed at the V/2?😎

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1 Answers

Arun
25750 Points
6 years ago
It's a Partial Pressure question 
P1+P2+P3=Ptotal 
ICE Table TIME!!! 
PCl5 ----------------> PCl3 + Cl2 
I 1 0 0 
C 1 -.80 +0.8 +0.8 
E 1-0.8 0.8 0.8 

Kp = 0.8^2/(1-0.8) 

Once you find the Kp you can use the same ice table format to find the new dissociation partial pressures and figure out the percent dissociated. Remember that the pressure will increase with decomposition. The pressure wont just stay the same

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