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Question

Liquids A and B form an ideal solution in the entire compositon range. At 350 K, the vapor pressures of pure A and pure B are 7×103 Pa and 12×103 Pa, respectively. The composition of the vapor in equilibrium with a solution containing 40 mole percent of A at this temperature is:

A
XA=0.28;XB=0.72
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B
XA=0.76;XB=0.24
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C
XA=0.37;XB=0.63
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D
XA=0.4;XB=0.6
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Solution

The correct option is A XA=0.28;XB=0.72
Given:
Vapour pressure of pure A (P0A)=7×103 Pa
Vapour pressure of pure B (P0B)=12×103 Pa
Moles of A=40%=0.4
Moles of B=60%=0.6
χA=0.40.4+0.6=0.4,
χB=0.6
Composition of vapour (XA)=PAPTotal=P0AχAP0AχA+P0BχB
=7×103×0.47×103×0.4+12×103×0.6=2.810=0.28
XB=10.28=0.72

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