Temperature (°C) POST-LAB QUESTION: (answers to be typed into your lab report) 1. An efficient fractional distillation of a binary 1:1 mixture of miscible liquids differing in boiling point by 80 °C is carried out in Kearney, NE. What would be the expected temperatures of any plateaus observed with a perfect thermometer in the temperature vs. mL distillate plot? 2. A mixture of toluene and benzene are distilled by distillation. The following is the phase diagram for this distillation, what is the composition of the vapor and the liquid at 95 °C? 115 110 105 100 Vapor 95 90 Liquid 85 80 75 70 65 0 0.2 0.4 0.6 Mole fraction benzene P = 1 atm 0.8 1.0

Temperature (°C) POST-LAB QUESTION: (answers to be typed into your lab report) 1. An efficient fractional distillation of a binary 1:1 mixture of miscible liquids differing in boiling point by 80 °C is carried out in Kearney, NE. What would be the expected temperatures of any plateaus observed with a perfect thermometer in the temperature vs. mL distillate plot? 2. A mixture of toluene and benzene are distilled by distillation. The following is the phase diagram for this distillation, what is the composition of the vapor and the liquid at 95 °C? 115 110 105 100 Vapor 95 90 Liquid 85 80 75 70 65 0 0.2 0.4 0.6 Mole fraction benzene P = 1 atm 0.8 1.0

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.
How many theoretical plates are required to produce a solution with a mole fraction of hexane greater than 0.90? Figure B A temperature-composition diagram for hexane (C6H14)-heptane (C7H16) mixtures.
In the determination of molecular weight through freezing point depression analysis. The volume of cyclohexane is 29.1 mL. Calculate the mass of cyclohexane(d=0.7786g/mL in grams.
Part II. Determination of molecular weight for ethyl alcohol Freezing point, °C DTf Mass of solute, g mass of solvent, kg Calculated molecular weight, g/mol -2.30 0C ΔTf = T0f – Tf 0.0 °C -(-2.30 °C) = 2.30 0C 6.202 g 0.1kg Click or tap here to enter text.
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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Can anyone help? I'm not sure what I'm doing wrong but the graph I keep plotting just seems to end up as straight line.
Pre-lab Assignment 1.) Note from the 'Introduction' that the freezing-point-depression constant, Kfp, for any solvent can be calculated as long as the heat of fusion, AHfus, and freezing point of the solvent is known. Calculate the freezing-point-depression constant (in SI units) for carbon tetrachloride, CC14, given that its heat of fusion is 2.5 kJ/mol and its freezing point is 250.3 K. M solvent & (TF Solvet) AIFUD - molor Mod 1=0,0821 LATM/ molk ~14=153.82glangs Кы = latm (153.82 $7) (0.0821 (ar) (250.5x)² 2 2.5 123/M/G\
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18. You need to dilute 10 M sulfuric acid to 0.5 M sulfuric acid for your experiment. You plan to use 100 mL of your diluted solution. How much of the concentrated solution do you need? Hint use M₁V₁=M₂V₂ 0.5 mL 5 mL C. 50 mL d. 500 mL a. b. (10M)V₁ = (0.5)(100ml) sob (10) = 500 1.05 10
Cryoscopic Determination of Molecular Weight Post-Lab Questions (40 Points) Name Lab Instructor 1. A student performed a freezing point determination and calculated the molar mass of Lab Day Date an unknown like you did in this experiment. The only difference in procedure was that when determining the freezing point of the unknown-naphthalene mixture, they started with a clean empty test tube. If the following errors occurred, how would each affect the calculated molar mass of the solute (too high, too low, or no change)? Explain your answerS. A. The thermometer used actually read 2.0°C too low for all measurements The test tube was put flat on the lab bench and some naphthalene spilled out. The student did not reweigh the test tube, proceeded to determine both the freezing point of pure naphthalene and the freezing point of the unknown-naphthalene mixture. B. The student after weighing out 1.02 g of the unknown accidentally spilled a small amount onto the floor when pouring the…