The vapour pressure of pure benzene and tolue | vedclass

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(C) Given: $P_{benzene}^{\circ} = 160 \ torr$,$P_{toluene}^{\circ} = 60 \ torr$. Since the solution is equimolar,the mole fractions are $x_{benzene} =

Vedclass · Accepted Answer

$0.27$

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(C) Given: $P_{benzene}^{\circ} = 160 \ torr$,$P_{toluene}^{\circ} = 60 \ torr$. Since the solution is equimolar,the mole fractions are $x_{benzene} = 0.5$ and $x_{toluene} = 0.5$. The partial pressure of benzene is $P_{benzene} = P_{benzene}^{\circ} 	imes x_{benzene} = 160 	imes 0.5 = 80 \ torr$. The partial pressure of toluene is $P_{toluene} = P_{toluene}^{\circ} 	imes x_{toluene} = 60 	imes 0.5 = 30 \ torr$. The total pressure is $P_{total} = P_{benzene} + P_{toluene} = 80 + 30 = 110 \ torr$. The mole fraction of toluene in the vapour phase $(Y_{toluene})$ is given by $Y_{toluene} = \frac{P_{toluene}}{P_{total}} = \frac{30}{110} \approx 0.27$.

The vapour pressure of pure benzene and toluene are $160 \ torr$ and $60 \ torr$ respectively. The mole fraction of toluene in the vapour phase in contact with an equimolar solution of benzene and toluene is:

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