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Question

The vapour pressure of pure liquids 1 and 2 are 450 mm Hg and 700 mm Hg respectively at 350 K. At a point when total vapour pressure is 600 mm Hg, choose the correct option(s) :

A
Mole fraction of component 2 in vapour phase is 0.3
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B
Mole fraction of component 1 in liquid phase is 0.4
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C
Mole fraction of component 1 in liquid phase is 0.6
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D
Mole fraction of component 2 in vapour phase is 0.7
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Solution

The correct option is D Mole fraction of component 2 in vapour phase is 0.7
By Raoult's Law :
PT=p1χ1+p2χ2
where
PT is the total pressure of the solution.
p1 is the vapour pressure of pure component 1
p2 is the vapour pressure of pure component 2
χ1 is the mole fraction of component 1 in liquid phase.
χ2 is the mole fraction of component 2 in liquid phase.

Putting the values:
600=450χ1+700χ2600=450χ1+700(1χ1)600=700250χ1χ1=0.4
χ2=10.4=0.6
Hence option (a) is correct and (d) is incorrect.
Also, from dalton's law we can write,
y1×PT=p1χ1

where,
y1=Mole fraction of component 1 in vapour phase
Putting values:
y1=450×0.4600y1=0.3y2=1y1=0.7
Hence option (c) is correct and (b) is incorrect.

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