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kupik [55]
3 years ago
9

Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 ∘C, the vapor pressure of pure be

nzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 11.5 g of biphenyl in 31.9 g of benzene?
Chemistry
1 answer:
Kisachek [45]3 years ago
3 0

Answer:

P_{solution} = 85.3Torr

Explanation:

Raoult's law is a tool that allows to determine vapour pressure of solutions. The formula is:

P_{solution} = X_{solvent}P_{solvent} <em>(1)</em>

Where

P is Pressure of solution and solvent and X is mole fraction.

Moles of solute and solvent are:

Biphenyl:

11.5g×(1mol /154.21g) = <em>0.0746mol</em>

Benzene

31.9g×(1mol /78.11g) = <em>0.408mol</em>

Mole fraction of benzene is:

\frac{0.408mol}{0.408mol + 0.0746mol} = <em>0.846</em>

Replacing in (1):

P_{solution} = 0.846*100.84Torr

P_{solution} = 85.3Torr

I hope it helps!

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