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A solution contains 0.0442 mol of ethanol and 0.715 mol of water at 25 oC. The...

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Chemistry

A solution contains 0.0442 mol of ethanol and 0.715 mol of waterat 25 oC. The vapor pressures of pure ethanol and pure water at 25oC are 44.6 torr and 23.8 Torr, respectively.

a) Assuming ideal behavior, calculate the total vapor pressureabove the solution.

b) If the actual vapor pressure above the solution is found tobe 28.3 Torr, is the solution behaving ideally? If not, whatinteractions are favored (the solute-solute and solvent-solventinteractions, or the solute interactions)?

Answer & Explanation Solved by verified expert
3.6 Ratings (399 Votes)
a Vapor pressure of solution vapor pressure of pure ethanol x mole fraction ethanol vapor pressure of water x mole fraction cyclohexanone mole fraction ethanol 00442 00442 0715 00442 07592 00582 mole fraction water 0715    See Answer
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