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The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?

The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?

Chemistry
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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The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressure
of pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?

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