SolutionHard

Question

An ideal mixture of liquids A and B with 2 moles of A and 2 moles of B has a total vapour pressure of 1 atm at a certain temperature. Another mixture with 1 mole of A and 3 moles of B has a vapour pressure greater than 1 atm. But if 4 moles of C are added to the second mixture, the vapour pressure comes down to 1 atm. Vapour pressure of C, Pc0 = 0.8 atm. Calculate the vapour pressures of pure A and pure B.

Options

A.PA0 = 1.4 atm, PB0 = 0.7 atm
B.PA0 = 1.2 atm, PB0 = 0.6 atm
C.PA0 = 1.4 atm, PB0 = 0.6 atm
D.PA0 = 0.6 atm, PB0 = 1.4 atm

Solution

= 1 atm      ⇒    PAo + PBo  = 2 atm
> 1 atm        ⇒    PAo + 3PBo  > 4 atm
&   = 1 atm    ⇒    PAo + 3PBo  + 4 PCo  = 8 atm
so     PAo + 3PBo  = (8 - 4 × 0.8) atm = 4.8 atm
Hence  PBo = 1.4 atm
            PAo = 0.6 atm

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