090320_homework9_answer_v2 - Chem340 Homework 9 P8.3) An...

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Chem340 Homework 9 P8.3) An ideal solution is formed by mixing liquids A and B at 298 K. The vapor pressure of pure A is 180. Torr and that of pure B is 82.1 Torr. If the mole fraction of A in the vapor is 0.450, what is the mole fraction of A in the solution? The mol fraction of A in the ideal solution of liquids A and B is given by: ( ) ( ) 0.272 0.450 Torr 180 Torr 82.1 Torr 180 Torr 82.1 0.450 y p p p p y x A A B A B A A = × + × = + = P8.4) A and B form an ideal solution. At a total pressure of 0.900 bar, y A = 0.450 and x A = 0.650. Using this information, calculate the vapor pressure of pure A and of pure B. ( ) ( ) ( ) ( ) * * * * * * * * * * * * * 0.900 bar 0.450 0.623 bar 0.650 0.450 0.650 0.450 0.650 1 0.450 2.27 0.450 1 0.650 1.414 bar total A a B total total B total a A A B A a B A A B A B A B A B P x P y P P y P P x y P x P P P y P P P P P P P = + × = = = = + = + × = = × = P8.5) A and B form an ideal solution at 298 K, with x A = 0.600, P A * = 105 Torr, and P B * = 63.5 Torr. a. Calculate the partial pressures of A and B in the gas phase. b. A portion of the gas phase is removed and condensed in a separate container.
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Calculate the partial pressures of A and B in equilibrium with this liquid sample at 298 K. a) Calculate the partial pressures of A and B in the gas phase. ( ) * * 0.600 105 Torr = 63.0 Torr 1 0.400 63.5 Torr = 25.4 Torr A A A B A B P x P P x P = = × = = × b) A portion of the gas phase is removed and condensed in a separate container. Calculate the partial pressures of A and B in equilibrium with this liquid sample at 298 K. The composition of the initial gas is given by 63.0 Torr 0.713; 0.287 88.4 Torr A A B A B P y y P P = = = = + ( ) * * For the portion removed, the new and values are the previous and values. 0.713 105 Torr = 74.9 Torr 1 0.287 63.5 Torr = 18.2 Torr A B A B A A A B A B x x y y P x P P x P = = × = = × P8.7) Assume that 1-bromobutane and 1-chlorobutane form an ideal solution. At 273 K, P chloro * = 3790 Pa and P bromo * = 1394 Pa. When only a trace of liquid is present at 273 K, y chloro = 0.75. a. Calculate the total pressure above the solution. b. Calculate the mole fraction of 1-chlorobutane in the solution. c. What value would Z chloro have in order for there to be 4.86 mol of liquid and 3.21 mol of gas at a total pressure equal to that in part (a)? [ : This composition is different from that of part (a).] a) Calculate the total pressure above the solution.
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( ) ( ) ( ) * * * * * total 3790 Pa P 3790 Pa 1394 Pa 0.75 3790 Pa 1394 Pa 3790 Pa 1394 Pa 2651 Pa 3790 Pa 0.75 3790 Pa
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090320_homework9_answer_v2 - Chem340 Homework 9 P8.3) An...

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