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a solution contains 25.0 g ethanol (c2h5oh; molar mass 46.07 g/mol) in 500. g h2o (molar mass 18.02 g/mol) at 23oc. if the vapor pressure of pure h2o at this temperature is 20.57 torr, what is the vapor pressure of the solution?



Answer :

pstnonsonjoku

The partial pressure of the solution is  0.39 torr.

What is Raoult's Law?

The Raoult's Law states that, the partial pressure of the solution is equal to the product of the mole fraction of the solute and the partial pressure of the pure solvent.

Hence;

Partial pressure of the pure solvent =  20.57 torr

Moles of water = 500 g/18 g/mol = 27.8 moles

Moles of ethanol = 25.0 g/46 g/mol = 0.54 moles

Total number of moles = 27.8 moles + 0.54 moles = 28.34 moles

Hence;

Partial pressure of solution = 0.54 moles/28.34 moles * 20.57 torr

= 0.39 torr

Learn more about Raoult's Law: https://brainly.com/question/28304759

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