At 25°C the vapour pressure of pure pentane is 511 torr and that of hexane is 150. torr. What is the mole fraction of pentane in a pentane-hexane solution that has a vapour pressure of 297 torr at 25°C? Submit Answer Tries 0/5 What is the mole fraction of hexane in the vapour that is in equilibrium with this solution? (Assume ideal gas behaviour.) Consider carefully the formula given on p719 in section 17 4 (under "Nonideal Solutions") of Zumdahl "Chemical Principles" 8th ed

At 25°C the vapour pressure of pure pentane is 511 torr and that of hexane is 150. torr. What is the mole fraction of pentane in a pentane-hexane solution that has a vapour pressure of 297 torr at 25°C? Submit Answer Tries 0/5 What is the mole fraction of hexane in the vapour that is in equilibrium with this solution? (Assume ideal gas behaviour.) Consider carefully the formula given on p719 in section 17 4 (under "Nonideal Solutions") of Zumdahl "Chemical Principles" 8th ed

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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The blue line on the diagram illustrates the effect of using fractional distillation to separate a mixture of hexane (C6H14) and heptane (C7H16). If one starts a fractional distillation with a 0.20 mole fraction of hexane, what is the approximate mole fraction of hexane in the vapor phase after two evaporation condensation cycles? Figure B A temperaturecomposition diagram for hexane (C6H14)-heptane (C7H16) mixtures.
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 pressureof 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 oCb) Determine the mass of A which must be added to 100 g of B to obtain a solution whosenormal boiling point is 100 C.
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 pressureof 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 oCb) Determine the mass of A which must be added to 100 g of B to obtain a solution whosenormal boiling point is 100 C. Please solve part B
At 25°C the vapour pressure of pure pentane is 511 torr and that of hexane is 150. torr.What is the mole fraction of pentane in a pentane-hexane solution that has a vapour pressure of 346 torr at 25°C? What is the mole fraction of hexane in the vapour that is in equilibrium with this solution?(Assume ideal gas behaviour.)
At 20 oC, the vapour pressure of pentane is 58kPa and the vapor pressure of hexane is 16 kPa. a) Estimate the pressure at which solution containing 258 g of hexane and 144 g of pentane will boil at 20 oC. b) Estimate the molar ratio of hexane to pentane in the vapor phase above this solution.
A vapour solution with a mole percentage of 10% benzene is cooled gradually. At what temperature does liquid first appear?
Part 1: 6.970 g of a non-volatile solute is dissolved in 230.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 60°C the vapour pressure of the solution is 147.48 torr. The vapour pressure of pure water at 60°C is 149.40 torr. Calculate the molar mass of the solute (g/mol). Part 2: Now suppose, instead, that 6.970 g of a volatile solute is dissolved in 230.0 g of water. This solute also does not react with water nor dissociate in solution. The pure solute displays, at 60°C, a vapour pressure of 14.94 torr. Again, assume an ideal solution. If, at 60°C the vapour pressure of this solution is also 147.48 torr. Calculate the molar mass of this volatile solute.
PART C C PLEASE 1. At 10.4 °C solutions of tetrahydrofuran (THF) and diethyl ether are described as being ideal over the entire range of composition. At this temperature, the vapour pressures of dilute solutions of THF in liquid diethyl ether are as follows: XTHF 0.004 0.009 0.016 PTHF / kPa 6.6 9.4 33.5 (b) At 10.4 °C, the vapour pressure of pure diethyl ether is 300 mmHg and that of THF is 107 mmHg. Calculate the vapour pressure of this solution when 0.06 moles of THF is mixed with 11.1 moles of diethyl ether. Justify the use of any equations used, and state all assumptions. (c) Calculate the mole fraction of THF in the vapour above the solution in part (b) above
At 365 K, pure toluene and hexane have vapor pressures of 5.82 x 10^4 Pa and 1.99 x 10^5 Pa, respectively. a) Calculate the mole fraction of hexane in the liquid mixture that boils at 365 K and a pressure of 760 Torr b) Calculate the mole fraction of hexane in the vapor that is in equilibrium with the liquid of part (a).
A dissolution is prepared dissolving 396 g of sacarose (C12H22O11) in 624 g of water. What is the vapor presurre at 30ºC? The vapor presurre of water at 30ºC is 31.8 torr and sacarose is a non-volatile solute.
The vapor pressure of pure dichloromethane at 298 K is 57.3 kPa. What is its vapor pressure above its mixture with chloroform with 8:2 molar ratios of dichloromethane to chloroform (consider their mixture an ideal solution)
Assuming benzene and toluene form ideal solution, what is the mole fraction of toluene in a solution that has a total vapor pressure of 88.98 torr at 20.0oC and 1.0 bar? The vapor pressures of toluene and benzene at 20.0oC and 1.0 bar are 22.14 torr and 75.01 torr, respctively.