At a given temperature, you have a mixture of ethanol and acetone at 19.5 °C. The vapor pressure of pure ethanol at 19.5 °C is 42.28 mmHg and the vapor pressure of pure acetone at 19.5 °C is 180.5 mmHg. The mole fraction of ethanol in the solution is 0.819. Assuming ideal behavior, calculate the mole fraction of acetone in the vapor above the solution, in mmHg.
At a given temperature, you have a mixture of ethanol and acetone at 19.5 °C. The vapor pressure of pure ethanol at 19.5 °C is 42.28 mmHg and the vapor pressure of pure acetone at 19.5 °C is 180.5 mmHg. The mole fraction of ethanol in the solution is 0.819. Assuming ideal behavior, calculate the mole fraction of acetone in the vapor above the solution, in mmHg.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section13.7: Colligative Properties Of Solutions
Problem 13.10PSP: The vapor pressure of an aqueous solution of urea. CH4N2O, is 291.2 mmHg at a measured temperature....
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