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?
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?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text: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)
O It will deviate positively.
O It will deviate negatively.
O It will be an ideal solution.
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Transcribed Image Text: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.
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