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Question

An aqueous solution containing 20% by weight of liquid 'X' (mol.wt.=140 g/mol) has a vapour pressure of 160 mm Hg at 60C. Calculate the vapour pressure of pure liquid 'X' if the vapour pressure of water is 150 mm Hg at 60C (in mm Hg upto two decimal).

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Solution

Partial pressure of each component of an ideal mixture of liquids is equal to the vapour pressure of the pure component multiplied by its mole fraction in the mixture.
psolute=Xsolute×posolute
psolvent=Xsolvent×posolvent
Ptotal=Xsolute×posolute+Xsolvent×posolvent
Given solution contains 20% by weight of liquid 'X'
Thus, weight of solute = 20 g
Weight of solvent = 80 g
nsolute=MassMolar mass =20140
nsolvent=8018
Mole fraction of solute =No. of moles of soluteTotal no. of moles
Xsolute=2014020140+8018=0.14284.587=0.031Psolution=Xsolute psolute+Xsolvent pSolvent160=0.0311×psolute+(10.031)×150160145.35=0.031psolute14.650.031=psolutepsolute=472.58 mm of Hg

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