At 90°C, the vapour pressure of methylbenzene is 54kPa and that of 1,3-dimethylbenzene is 18.0 kPa. What is the molar fraction of methylbenzene in the gas phase above the mixture containing 1 mol of methylbenzene and 2mol of 1,3-dimethylbenzene at this temperature (assume that these solvents form ideal solutions).

At 90°C, the vapour pressure of methylbenzene is 54kPa and that of 1,3-dimethylbenzene is 18.0 kPa. What is the molar fraction of methylbenzene in the gas phase above the mixture containing 1 mol of methylbenzene and 2mol of 1,3-dimethylbenzene at this temperature (assume that these solvents form ideal solutions).

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 12.84QE

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At 90°C, the vapour pressure of methylbenzene is 54 kPa and that of 1,3-dimethylbenzene is 18.0 kPa. What is the molar fraction of methylbenzene in the gas phase above the mixture containing 1 mol of methylbenzene and 2 mol of 1,3- dimethylbenzene at this temperature (assume that these solvents form ideal solutions).
The vapor pressure of pure dichloromethane at 298 K is 57.3 kPa. What is its vaporpressure above its mixture with chloroform with 8:2 molar ratios of dichloromethane to chloroform (consider their mixture an ideal solution).
At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (a) What is the molar fraction of toluene in the liquid mixture when the total vapor pressure is 0.50 atm at 90 °C? In liquid, xtoluene =........... At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (b) What is the molar fraction of toluene in the gas phase when the total vapor pressure is 0.50 atm at 90 °C? In gas, xtoluene = __________ .
A vapour solution with a mole percentage of 10% benzene is cooled gradually. At what temperature does liquid first appear?
At 413K the vapor pressure of pure chlorobenzene is 1.237 bar and that of pure bromobenzene is 0.658 bar. These solvents form ideal solutions. A) What is the mole fraction of chlorobenzene in a mixture of these two that just boils at 413K at 1 bar? b) What is the mole fraction of chlorobenzene in the vapor produced in (a)? c) Supposed this vapor is condensed what is its total vapor pressure at 413K?
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.
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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.
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In this table you can find the composition and total vapour pressure of a benzene-toluene solution at 120 ºC:
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