4. The vapor in equilibrium with a solution of ethanol (eth) and 0.9900 has a pressure of chloroform (chl) at 45°C with Xh 438.59 torr and has Xchl.(g) assumed to be essentially ideally dilute. a. Find the vapor-phase partial pressures. b. Calculate the vapor pressure of pure chloroform at 45°C. = chl (1) 0.9794. The solution can be

4. The vapor in equilibrium with a solution of ethanol (eth) and 0.9900 has a pressure of chloroform (chl) at 45°C with Xh 438.59 torr and has Xchl.(g) assumed to be essentially ideally dilute. a. Find the vapor-phase partial pressures. b. Calculate the vapor pressure of pure chloroform at 45°C. = chl (1) 0.9794. The solution can be

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 82AP

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