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Question

At some temperature and under a pressure of 4 atm, PCl5 is 10% dissociated. Calculated the pressure at which PCl5 will be 20% dissociated temperature remaining same.
  1. 0.96 atm
  2. 0.68 atm
  3. 0.54 atm
  4. 0.81 atm


Solution

The correct option is A 0.96 atm
Let initially 100 moles were present and after 10% dissociation at equilibrium only 90% are remaining.
At 4 atm pressure and 10% dissociation.
PCl5PCl3Cl2Equibm mole901010Equilibrium partial pressures90110×410110×410110×4
Hence, Kp=PPCl5PPCl5PPCl5=499
At 20 % dissociation,
PCl5PCl3Cl2Equilibrium mole802020Equilibrium partial pressures80120×P20120×P20120×PKp=PPCl3PCl2PPCl5=124×P
Thus, 124×P=499 or P=0.96 atm

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