At 60°C, the vapor pressure of ethanol is 352.7 mm Hg and that of methanol is 625.0 mm Hg. These two substances form an ideal solution. For a liquid solution that contains 60% mole ethanol, calculate the: a. vapor pressure (mm Hg) of the mixture: ANSWER (in 2 decimal places, no unit required): mm Hg b. mole fraction of methanol in the vapor in equilibrium with the mixture:

At 60°C, the vapor pressure of ethanol is 352.7 mm Hg and that of methanol is 625.0 mm Hg. These two substances form an ideal solution. For a liquid solution that contains 60% mole ethanol, calculate the: a. vapor pressure (mm Hg) of the mixture: ANSWER (in 2 decimal places, no unit required): mm Hg b. mole fraction of methanol in the vapor in equilibrium with the mixture:

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 114CP: Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution...

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