A solution of cyclohexane-toluene mixture was distilling at 88 oC. The analysis of a sample of the distilled liquid and a sample of vapor at that temperature indicate that 60% of the liquid and 77% of the vapor is cyclohexane. Calculate mole fractions of each compound in the solution and in the vapor.

A solution of cyclohexane-toluene mixture was distilling at 88 oC. The analysis of a sample of the distilled liquid and a sample of vapor at that temperature indicate that 60% of the liquid and 77% of the vapor is cyclohexane. Calculate mole fractions of each compound in the solution and in the vapor.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter13: Solutions And Their Behavior

Section13.5: Colloids

Problem 1.3ACP

See similar textbooks

Similar questions

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.
When pure furfural (solvent) is added to a mixture containing 0.2 mass fraction diphenylhexane and 0.8 mass fraction docosane, two separate layers can be obtained. If the composition of the two layers are as shown in the table, how much solvent was added to 500 kg of solution of docosane and diphenylhexane?
Aniline, C6H5NH2, and hexane, C6H14, form partially miscible liquid–liquid mixtures at temperatures below 69.1 °C. When 42.8 g of aniline and 75.2 g of hexane are mixed together at a temperature of 67.5 °C, two separate liquid phases are formed, with mole fractions of aniline of 0.308 and 0.618. (i) Determine the overall mole fraction of aniline in the mixture. (ii) Use the lever rule to determine the relative amounts of the two phases.
There are two separate phases, one of which is 12% phenol and the other is 60% phenol, from a 210 gram phenol-water mixture at a temperature of 60°C with a composition of 35% phenol. Calculate the masses of these phases.
The partial molar volumes of propanone and trichloromethane in a mixture in which the mole fraction of CHCI3 is 0.4693 are 74.166 cm3 mol-1, and 80.235 cm3 mol-1, respectively. What is the volume of a solution of total mass 1.000 kg?
Aniline, C6H5NH2, and hexane, C6H14 , form partially miscible liquid - liquid mixtures at temperatures below 69. 1 °C. When 42.8 g of aniline and 75 .2 g of hexane are mixed together at a temperature of 67.5 °C, two separate liquid phases are formed, with mole fractions of aniline of 0.308 and 0.618.(a) Determine the overall mole fraction of aniline in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases.
In class, we derived the expression:ln XA =(ΔvH/R) ((1/T)-(1/T°))where A represents the solvent (and B would represent the solute, such that XA + XB = 1).Using the approximations given below, derive the expression:∆Tb = XB (RT°2/ΔvH)where ∆Tb is the change in boiling point between the solution and the pure liquid, T − T°.Approximations:ln(1 − X) ≈ −XTT° ≈ T°2Note: this derived expression is often simplified in General Chemistry as ∆Tb = Kbm where Kb is the boiling point elevation constant, and m is the molality.
The weight fraction of methanol in an aqueous solution is 0.64. The mole fraction of methanol (x) satisfies a. X < 0.5 b. 0.5 < XM < 0.64 c. xu = 0.5 d. Xu ~ 0.5
1.Define binary mixture 2. Define density 3. Give an abstract of determination of excess molar volume of binary mixtures of water and methanol by measuring density
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).
There are two separate phases, one with a composition of 12% phenol and the other with a composition of 60% phenol, from a 210 gram phenol-water mixture at 60 °C with a composition of 35% phenol. Calculate the masses of these phases.
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).