Chemistry

Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 °C, the vapor pressure of pure benzene is 100.84 torr. What is the vapor pressure of a solution made from dissolving 10.7 g of biphenyl in 33.9 g of benzene?

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  1. moles biphenyl = grams/molar mass
    moles benzene = grams/molar mass
    mol fraction benzene = Xbenzene = mol benzene/total moles.

    partial pressure benzene = Xbenzene*Pnormal v.p.

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  2. I did what you said and didn't get the correct answer :(

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  3. Post your work and I'll try to find your error.

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  4. Can someone confirm the answer for this. I worked it out and got an answer of 85.5 torr. Is this right? Can someone please put the answer to this so I can check. Thanks. That would be helpful.

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  5. I worked it and obtained 86.9 torr which is close to your number but not quite the same. I used 154 for the molar mass of biphenyl and I used 78 for the molar mass of benzene.
    If you will post your work I'll look at it. Please make a new post of it--this one is getting a little far from the front page.

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