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A)
Benzene - A and water - B
are immiscible
So
At boiling point
P = Pas + Pbs
Pas - vapor pressure of benzene
Pbs - vapor pressure of water
P = 1 atm = 760 mmHg
The boiling point ofod mixture will be less than boiling point of either of two pure components
The vapor pressures are given in table above
Vapor pressures are calculated by interpolation
Temperature | V.P(mmHg) (water) | V.P(mmHg) (benzene) |
35.3 | 43 | 150 |
52.7 | 106 | 300 |
72.6 | 261 | 600 |
80.1 | 356 | 760 |
The sum of both vapor pressures should be equal to 760 mmHg
760 = Pas+ Pbs
At 52.7°C
Pas =300 mmHg
Pbs = 106 mmHg
Pas + Pbs = 406 mmHg which is lesser than 760 mmHg
At 72.6°C
Pas = 261 mmHg
Pbs = 600 mmHg
Pas + Pbs = 861 mmHg which is greater than 760 mmHg
This shows that booking point of mixture lies between 52.7°C to 72.6°C
At 52.7°C - sum of vapor presssures = 406 mmHg
At 72.6°C - sum of vapor presssures = 861 mmHg
By interpolation ,
At Pas + Pbs = 760 mmHg
Boiling temperature of mixture = 68.182 °C
At 68.182°C
Pas = 533.4065 mmHg
Pbs = 226.593 mmHg
Applying raoults law
yP = Pas
y (760) = 533.4065
y = 0.70185
Benzene - 0.70185
(1-y) = 0.29815
Water - 0.29815
Both are immiscible
B) . Amount of benzene to be vaporized = 10 mol
For steam distillation
Benzene to be evaporated = 10 mol
WA/MA = 10 mol
M. W of water = 18 g /mol
M. W of benzene = 78 g/mol
MB/WB = 4. 24803 moles
Moles of steam requires to evaporate 10 mol benzene
Mass of steam required = 4.24804(18) =
76.464 g
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