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March 28, 2017

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At a given temperature, you have a mixture of benzene (vapor pressure of pure benzene = 745 torr) and toluene (vapor pressure of pure toluene = 290 torr). The mole fraction of benzene in the vapor above the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the solution.
Answer

  • chemistry - ,

    PA=XAP'A

  • chemistry - ,

    0.213

  • chemistry - ,

    Since the benzene comes out better you will need more Toluene in the solution
    to get its mol fraction above the solution
    .59 = Pb/[(Pb)(Pt)}
    Assumming 1 atm external pressure

    .59 = (1-x)745/(1-x)745 + x(290)
    =0.641

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