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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
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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