At 300 K, the vapor pressure of pure benzene (C6H6) is0.1355 atm and the vapor pressure of pure n-hexane(C6H14) is 0.2128 atm. Mixing 50.0 g of benzene with50.0 g of n-hexane gives a solution that is nearly ideal.(a) Calculate the mole fraction of benzene in the solution.(b) Calculate the total vapor pressure of the solution at 300 K.(c) Calculate the mole fraction of benzene in the vapor in equilibrium with the solution.
At 300 K, the vapor pressure of pure benzene (C6H6) is0.1355 atm and the vapor pressure of pure n-hexane(C6H14) is 0.2128 atm. Mixing 50.0 g of benzene with50.0 g of n-hexane gives a solution that is nearly ideal.(a) Calculate the mole fraction of benzene in the solution.(b) Calculate the total vapor pressure of the solution at 300 K.(c) Calculate the mole fraction of benzene in the vapor in equilibrium with the solution.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.86QE
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Question
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 of benzene with
50.0 g of n-hexane gives a solution that is nearly ideal.
(a) Calculate the mole fraction of benzene in the solution.
(b) Calculate the total vapor pressure of the solution at
300 K.
(c) Calculate the mole fraction of benzene in the vapor in
equilibrium with the solution.
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