Imagine a solution of two liquids that are so similar that their interactions together are the same as in the individual liquids. Will this solution deviate positively from, deviate negatively from, or ideally follow Raoult's law? It will deviate positively. It will deviate negatively. O It will be an ideal solution.

Imagine a solution of two liquids that are so similar that their interactions together are the same as in the individual liquids. Will this solution deviate positively from, deviate negatively from, or ideally follow Raoult's law? It will deviate positively. It will deviate negatively. O It will be an ideal solution.

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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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.