Asked by Sarah
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?
Answers
Answered by
DrBob222
moles biphenyl = grams/molar mass
moles benzene = grams/molar mass
mol fraction benzene = Xbenzene = mol benzene/total moles.
partial pressure benzene = Xbenzene*P<sub>normal v.p.</sub>
moles benzene = grams/molar mass
mol fraction benzene = Xbenzene = mol benzene/total moles.
partial pressure benzene = Xbenzene*P<sub>normal v.p.</sub>
Answered by
Sarah
I did what you said and didn't get the correct answer :(
Answered by
DrBob222
Post your work and I'll try to find your error.
Answered by
Alyssa
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.
Answered by
DrBob222
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.
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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