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The pressure of an ideal mixture of o-xylene and m-xylene is 247.5 mmHg at 373 K. The mole fraction of o-xylene in the liquid phase is 0.4 and its vapor pressure at that temperature is 213.1 mmHg. Calculate the number of moles of m-xylene in the vapor phase, knowing that there are 10 moles in this phase, and the vapor pressure of pure m-xylene at that temperature.

The pressure of an ideal mixture of o-xylene and m-xylene is 247.5 mmHg at 373 K. The mole fraction of o-xylene in the liquid phase is 0.4 and its vapor pressure at that temperature is 213.1 mmHg. Calculate the number of moles of m-xylene in the vapor phase, knowing that there are 10 moles in this phase, and the vapor pressure of pure m-xylene at that temperature.

Chemistry: The Molecular Science
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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The pressure of an ideal mixture of o-xylene and m-xylene is 247.5 mmHg at 373 K. The mole fraction of o-xylene in the liquid phase is 0.4 and its vapor pressure at that temperature is 213.1 mmHg. Calculate the number of moles of m-xylene in the vapor phase, knowing that there are 10 moles in this phase, and the vapor pressure of pure m-xylene at that temperature.
Transcribed Image Text:The pressure of an ideal mixture of o-xylene and m-xylene is 247.5 mmHg at 373 K. The mole fraction of o-xylene in the liquid phase is 0.4 and its vapor pressure at that temperature is 213.1 mmHg. Calculate the number of moles of m-xylene in the vapor phase, knowing that there are 10 moles in this phase, and the vapor pressure of pure m-xylene at that temperature.
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