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Benzene and toluene form an ideal soluti...

Benzene and toluene form an ideal solution. The vapor pressures of pure benzene and pure toluene are `75 mmHg` and `25 mmHg` at `20^(@)C`. If the mole fractions of benzene and toluene in vapor phase are `0.63` and `0.37` respectively, then the vapor pressure of the ideal mixture will be

A

`49.78 mmHg`

B

`78.67 mmHg`

C

`58.76 mmHg`

D

`39.68 mmHg`

Text Solution

Verified by Experts

The correct Answer is:
4
If `Y_("benzene")` and `Y_("toluene")` repersent the mole fraction of benzene and toluene in the vapor phase respectively, we have from Dalton's law of partial pressure:
`Y_("benzene")=P_("bensene")/P_("total")`
`Y_("toluene")=P_("toluene")/P_("total")`
From which we can drive the following relation:
`1/P_("total")=Y_("benzene")/P_("benzene")^(0)+Y_("toluene")/P_("toluene")^(0)`
`1/P_("total")=0.63/(75 mmHg)+0.37/(22 mmHg)`
`=(13.86+27.75)/1650`
`1/P_("total")=0.0252 mmHg`
or `P_("total")=39.68 mmHg`
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Knowledge Check

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