Assess the following statements about fractional distillation. Determine which are TRUE/FALSE 1.Multiple vaporization-condensation cycles are needed to purify samples of relatively close boiling points 2. The column efficiency of a fractionating column can be assessed by the HETP 3. A fractionating column is part of the apparatus set-up 4. With every condensation-vaporization cycle, the vapors become enriched in the higher boiling point component

Assess the following statements about fractional distillation. Determine which are TRUE/FALSE 1.Multiple vaporization-condensation cycles are needed to purify samples of relatively close boiling points 2. The column efficiency of a fractionating column can be assessed by the HETP 3. A fractionating column is part of the apparatus set-up 4. With every condensation-vaporization cycle, the vapors become enriched in the higher boiling point component

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 1.1ACP: The blue line on the diagram illustrates the effect of using fractional distillation to separate a...

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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.
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Use an apparatus similar to that shown and assume that the round-bottom flask holds 10 mL and that the Claisen head has an internal volume of about 2 mL in the vertical section. At the end of a distillation, vapor would fill this volume, but it could not be forced through the system. No liquid would remain in the distillation flask. Assuming this holdup volume of 12 mL, use the ideal gas law and assume a boiling point of 100°C (760 mm Hg) to calculate the number of microliters of liquid (d = 0.9 g/mL, MW = 200) that would recondense into the distillation flask on cooling.
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List and describe two methods that can used to improve the separation of a liquid mixture by fractional distillation
1a. Use the given table to construct a temperature-composition diagram for cyclohexane Toluene mixture. Based on the plot, what is the composition of the distillate obtained by Simple distillation 20 mole percent cyclohexene and 80 mole percent toluene? Show your Work on the plot. 1b. Estimate the composition of the distillate of 20 mole percent of cyclohexane if the Distillation column had three theoretical plates.
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The followings methods are useful to induce crystallization EXCEPT adding a small crystal of the desired compound, called a seed crystal, to the solution adding anhydrous potassium carbonate to the solution and cooling it in an ice bath scratching the inner wall of the Erlenmeyer flask with a glass stirring rod reheating the solution to boiling to boil off some of the solvent, and then allow the solution to cool to room temperature again to effect crystallization
Please answer both questions.1. Arrange the following steps based on the order they occur in a distillation process:I. The vapor condenses with the aid of flowing cold water in the condenserII. The liquid is collected in the receiving flask, removing the first 1 mL of the distillateIII. The mixture is heated in the distilling flask while simultaneously monitoring the temperatureIV. The more volatile component evaporates and passes through the three-way connector2. The components of an 80-mL rubbing alcohol sample were separated using distillation and the resulting percent recovery of isopropyl alcohol is 14.70%. Determine the volume, in mL, of isopropyl alcohol present in the sample. a. 11.86 mL b. 11.76 mL c. 11.23 mL d. 12.45 mL
I. FREEZING POINT LOWERING: Some crushed ice was placed in a 400 mL beaker. Some of the ice was allowed to melt before the temperature was taken and recorded to be 0°C as temperature of the ice. A 20 % urea solution is accurately prepared from dissolving 2 grams urea in 8 grams of distilled water. This urea solution is placed in a test tube then submerged in the beaker with crushed ice. The temperature of the urea solution was taken three times(3X) at intervals of 30 seconds and was recorded to be -2°C, -4°C and -8°C respectively. The temperature was taken until the freezing point was reached indicated when 3 consecutive temperature readings were identical to be -8°C. This was recorded to be the freezing point of the solution. DATA AND RESULTS: (Show all pertinent computations on the space provided if applicable. +Answers with no computation will not be considered.) Mass of urea in grams Mass of water in grams Freezing point of ice in degrees Celsius Freezing point of urea solution in…