Learning Goal:To understand deviations from the ideal vaporpressure for solutions of two liquids.How to apply Raoult's law to real solutionsRaoult's law is used to predict the vapor pressure ofan ideal solution that contains one or more volatilecomponents. For a solution with only onecomponentConsider mixing a liquid with a vapor pressure of 100 torr with an equimolar amount of a liquid with a vapor pressure of 200torr. The resulting solution would be predicted to have a vapor pressure of 150 torr if it behaved ideally.If, however, the interactions between the different components are not similar we can see positive or negative deviations from thecalculated vapor pressure. An actual vapor pressure greater than that predicted by Raoult's law is said to be a positive deviationand an actual vapor pressure lower than that predicted by Raoult's law is a negative deviation.Psoln = Prolv X Xolvwhere Psoln is the vapor pressure of gaseoussolvent above the solution, Psoly is the vaporpressure of the pure solvent, and Xsolv is the molefraction of the solvent.Part AImagine a solution of two liquids in which the molecules interact less favorably than they do in the individual liquids. Will thissolution deviate positively from, deviate negatively from, or ideally follow Raoult's law?An assumption of Raoult's law is that theinteractions between the different components ofthe solution are similar in magnitude to theinteractions of each of the components withthemselves; in other words, the components forman ideal solution. Deviations from this law areobserved when interactions between solute andsolvent are not similar.• View Available Hint(s)O t will deviate positively.O It will deviate negatively.O It will be an ideal solution.

Solution Raoult’s law states that a solvent’s partial force per unit area in an exceedingly answer…

How to apply Raoult's law to real solutions Consider mixing a liquid with a vapor pressure of 100 torr with an equimolar amount of a liquid with a vapor pressure of 200 torr. The resulting solution would be predicted to have a vapor pressure of 150 torr if it behaved ideally. If, however, the interactions between the different components are not similar we can see positive or negative deviations from the calculated vapor pressure. An actual vapor pressure greater than that predicted by Raoult's law is said to be a positive deviation and an actual vapor pressure lower than that predicted by Raoult's law is a negative deviation. Part A Imagine a solution of two liquids in which the molecules interact less favorably than they do in the individual liquids. Will this solution deviate positively from, deviate negatively from, or ideally follow Raoult's law? • View Available Hint(s) It will deviate positively. O t will deviate negatively. O It will be an ideal solution.

How to apply Raoult's law to real solutions Consider mixing a liquid with a vapor pressure of 100 torr with an equimolar amount of a liquid with a vapor pressure of 200 torr. The resulting solution would be predicted to have a vapor pressure of 150 torr if it behaved ideally. If, however, the interactions between the different components are not similar we can see positive or negative deviations from the calculated vapor pressure. An actual vapor pressure greater than that predicted by Raoult's law is said to be a positive deviation and an actual vapor pressure lower than that predicted by Raoult's law is a negative deviation. Part A Imagine a solution of two liquids in which the molecules interact less favorably than they do in the individual liquids. Will this solution deviate positively from, deviate negatively from, or ideally follow Raoult's law? • View Available Hint(s) It will deviate positively. O t will deviate negatively. O It will be an ideal solution.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.88QE

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