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The boiling point of pure ethanol at 760. torr is 82.0 degrees celsius. What would bet...

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Chemistry

The boiling point of pure ethanol at 760. torr is 82.0 degreescelsius. What would bet the vapor pressure of ethanol over asolution containing 2.13 mole of nonvolatile hydrocarbon and 15.30moles of ethanol at 85.9 degrees celsius?

Answer & Explanation Solved by verified expert
4.2 Ratings (761 Votes)

Solution :-

formula to calculate the vapor pressure of the solution is as follows

Vapor pressure of solution = mole fraction of solvent * vapor pressure of pure solvent

lets first calculate the mole fraction of the ethanol

mole fraction of ethanol = moles of ethanol / total moles

                                  = 15.30 mol / (15.30 mol + 2.13 mol )

                                 = 0.8778

now lets calculate the vapor pressure of the solution

Vapor pressure of solution = mole fraction of solvent * vapor pressure of pure solvent

                                       = 0.8778 * 760 torr

                                       = 667 torr

Therefore vapor pressure of the solution = 667 torr
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