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 ftwo liquids in which the molecules interact less favorably than they do in the individual liquids Will this solution deviate posltively from, deviate negatively from, or idealy follow Raouit's law?

a. It will deviate positively.
b. It will deviate negatively.
c. It will be an ideal solution

Part B
Imagine a solution of two iquids in which the molecules interact more favorably than they do in the individual liquids Will this solution deviate positively from, deviate negatively from, or ideally follow Raoult's law?

a. It will deviate positively. b. It will deviate negatively. c. It will be an ideal solution