Don't used Ai solution At standard pressure (101.325 kPa), it is found that the boiling point of an ideal binary solutionof A and B is 87 °C. At this temperature, the vapour pressures of pure A and B are 142.58 kPaand 87.09 kPa, respectively. What is the composition of A in the vapour above the solution,presuming it is an ideal gas?

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Answered: At standard pressure (101.325 kPa), it…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 46P

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3. Assume that toluene and hexane form an ideal solution. At 365 K pure toluene has a vapour pressure of 0.582 bar and pure hexane has a vapour pressure of 1.99 bar. Consider a solution with mole fraction of hexane = 0.250. (a) Calculate the partial pressures of toluene and hexane, and the total pressure above the solution. (b) Some of the vapour is removed and allowed to condense in a second container. Calculate the partial pressures of hexane and toluene and the total pressure above this solution.
Benzene and methylbenzene (toluene) form nearly ideal solutions. Consider an equimolar solution of benzene and methylbenzene. At 20 °C the vapour pressures of pure benzene and methylbenzene are 9.9 kPa and 2.9 kPa, respectively. The solution is boiled by reducing the external pressure below the vapour pressure. Calculate (a) the pressure when boiling begins, (b) the composition of each component in the vapour, and (c) the vapour pressure when only a few drops of liquid remain. Assume that the rate of vaporization is low enough for the temperature to remain constant at 20 °C.
A solution is prepared by dissolving 2.33 g of C60 (buckminsterfullerene)in 100.0 g of toluene (methylbenzene). Given that the vapour pressure of pure toluene is 5.00 kPa at 30 °c, what is the vapour pressure of toluene in the solution?
It is found that the boiling point of a binary solution of A and B with xA = 0.479 is 88°C. At this temperature the vapor pressures of pure A and B are 130.1 kPa and 74.9 kPa, respectively. (a) Is this solution ideal? (b) What is the initial composition of the vapor above the solution?
(b) At 80 °C, ethylene dibromide and propylene dibromide mixture forms an ideal solution. Given that the pure vapour pressures of ethylene dibromide and propylene dibromide are 22.9 and 16.9 kPa, respectively. Using the plots of partial vapour pressures of ethylene dibromide and propylene dibromide, and total vapour pressure of the mixture against the mole fraction of ethylene dibromide, determine (i) the composition of the vapour in equilibrium with a solution containing 0.75 mole fraction of ethylene dibromide. (ii) the composition of the liquid phase in equilibrium with ethylene dibromide- propylene dibromide containing 0.5 mole fraction each.
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It is found that the boiling point of a binary solution of A andB with xA = 0.6589 is 88 °C. At this temperature the vapour pressuresof pure A and B are 127.6 kPa and 50.60 kPa, respectively. (i) Is thissolution ideal? (ii) What is the initial composition of the vapour abovethe solution?
An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid phase Xeth = 0.9900 has a total vapour pressure of p = 17795 Torr. The vapour pressure of pure ethanol at this temperature is p*eth = 172.76Torr. (a) Use Raoult's law to calculate the partial pressure of ethanol in the vapour phase. (b) Hence determine the partial pressure of chloroform in the vapour phase . (c) Also calculate the mole fractions of chloroform and ethanol in the vapour phase. (d) Calculate the Henry's law constant for chloroform, Kchl at this temperature.
s) At 20 °C the vapor pressure of benzene is 10 kPa and that of methylbenzene is 2.8 · kPa. If this mixture is an ideal solution, what is the total vapor pressure of an equimolar mixture of the two components? Note that equimolar means that there are the same number of moles of both substances.
3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane (CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25 moles of components, what is the mass of CHCI3 present in that solution.
The enthalpy of fusion of solute B is 4,384.28 kJ/mol and its melting point is 870.49oC. Calculate its ideal solubility (nB) in 8.53 moles of solvent at 143.49oC.
Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0. 0 42 and 0 .161 . (a) Calculate the overall mole fraction of phenol in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases .

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