The molar mass of liquid A = 85.0 g / mole, that of B = 112.0 g / mole. At 100 C, a solution of mass percentage in A equal to 30.0%, considered ideal, has a vapor pressure of equilibrium equal to 110 kPa. The vapor in equilibrium with this solution has a mole fraction of A equal to 0.450. A) Determine the equilibrium vapor pressure of pure A and that of pure B at 100 oC
The molar mass of liquid A = 85.0 g / mole, that of B = 112.0 g / mole. At 100 C, a solution of mass percentage in A equal to 30.0%, considered ideal, has a vapor pressure of equilibrium equal to 110 kPa. The vapor in equilibrium with this solution has a mole fraction of A equal to 0.450. A) Determine the equilibrium vapor pressure of pure A and that of pure B at 100 oC
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
Chapter11: Properties Of Solutions
Section: Chapter Questions
Problem 105AE
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The molar mass of liquid A = 85.0 g / mole, that of B = 112.0 g / mole. At 100 C, a solution of mass percentage in A equal to 30.0%, considered ideal, has a vapor pressure
of equilibrium equal to 110 kPa. The vapor in equilibrium with this solution has a mole fraction of A equal to 0.450.
A) Determine the equilibrium vapor pressure of pure A and that of pure B at 100 oC
b) Determine the mass of A which must be added to 100 g of B to obtain a solution whose
normal boiling point is 100 C.
Please solve part B
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