. In an ideal solution of liquids A and B, the vapor pressure of amixture of 0.60 mol of A and 2.4 mol of B is 0.42 atm at 70°C.1.80 moles of A is added to the solution at 70°C and the vaporpressure of the solution rises to 0.55 atm. Calculate the vaporpressure if some of the vapor in equilibrium with the first solutionwere completely condensed.a. 0.51 atmb. 0.35 atmc. 0.20 atmd. 0.80 atm

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Answered: . In an ideal solution of liquids A and…

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

Section: Chapter Questions

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

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Table sugar granules were dissolved in a glass of water. The solid sugar granules have no measurable vapor pressure, making water as the contributor to the entire vapor pressure of the resulting solution. If sugar was added to the glass of water until the water makes up a mole fraction of 0.75 in the solution, what is the vapor pressure of water in this solution? Given the following: vapor pressure of water at 25°C is 23.8 torr. A. 23.8 torr B. 5.95 torr C. 29.75 torr D. 17.9 torr
135 g of acetone ( C3H6O) and 265 of water are mixed at 20. Find the vapor pressure of this solution. Water vapor pressure = 25 torr at 20C.
A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the molecular mass? A. 98 g/mol B. 125 g/mol C. 168 g/mol D. 178 g/mol E. 207 g/mol F. 150 g/mol
Table sugar granules were dissolved in a glass of water. The solid sugar granules have no measurable vapor pressure, making water as the contributor to the entire vapor pressure of the resulting solution. If sugar was added to the glass of water until the water makes up a mole fraction of 0.75 in the solution, what is the vapor pressure of water in this solution? Given the following: vapor pressure of water at 25°C is 23.8 torr. A. 23.8 tor B. 5.95 torr C. 29.75 torr D. 17.9 torr What is the vapor pressure of the said solution if the vapor pressure of pure benzene is 100 torr at 26.1°C? A. 152.26 mmHg B. 88.00 mmHg C. 22.97 torr D. 78.12 torr A 0.25g of a certain substance is dissolved in 60g of water. The freezing point of the solution is - 0.050 °C. that the substance has a van't Hoff factor of 1 and is non-volatile, what is the molar mass of the substance? (Freezing point depression of water = - 1.86 °C/m) A. 0.00016 g/mol B. 156.25 g/mol C. 186.54 g/mol D. 1.86 g/mol
12. Glycerin, C3H8O3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding glycerin to H₂O at 39.8°C such that the mole fraction of glycerin is 0.0873? The vapor pressure of pure water at 39.8°C is 54.74 torr. a. 50.0 torr b. 60.0 torr c. 4.76 torr d. 70.0 torr e. None of the above Page 6
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A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapor pressure of pure CCI4 is 33.85 torr at 298 K. The Henry's Law constant when the concentration of Br2 is expressed as a mol fraction is 122.36 torr. Calculate the mole fraction of Br2 in the vapor when it's in equilibrium with a solution that has a mole fraction of Br2 equal to 0.050, having the assumption that the vapor still behaves as an ideal gas.
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1. A 4.0mg sample of a certain protein is dissolved in 20.0mL solution. The solution exhibits an osmotic pressure of 1.18orr at 25°C. Calculate the molecular weight of that protein
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