At 300°K, the vapor pressure of pure benzene (C6H6) is 0.1355 atm and the vapor pressure of pure n-hexane (C6H14) is 0.2128 atm. Mixing 50.0 g benzene with 50.0 g of n-hexane gives a solution that is nearly ideal. If this vapor were collected and then recondensed, the mole fraction of benzene in this new solution would be 0.414. If the new solution were allowed to come to equilibrium, what would the mole fraction of benzene in the vapor in equilibrium with the solution be?
At 300°K, the vapor pressure of pure benzene (C6H6) is 0.1355 atm and the vapor pressure of pure n-hexane (C6H14) is 0.2128 atm. Mixing 50.0 g benzene with 50.0 g of n-hexane gives a solution that is nearly ideal. If this vapor were collected and then recondensed, the mole fraction of benzene in this new solution would be 0.414. If the new solution were allowed to come to equilibrium, what would the mole fraction of benzene in the vapor in equilibrium with the solution be?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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At 300°K, the vapor pressure of pure benzene (C6H6) is 0.1355 atm and the vapor pressure of pure n-hexane (C6H14) is 0.2128 atm. Mixing 50.0 g benzene with 50.0 g of n-hexane gives a solution that is nearly ideal. If this vapor were collected and then recondensed, the mole fraction of benzene in this new solution would be 0.414. If the new solution were allowed to come to equilibrium, what would the mole fraction of benzene in the vapor in equilibrium with the solution be?
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