6. Using the figure below, what is the composition of the vapor from a solution containing 20 grams of toluene and 40 grams of benzene? Show all your work. Composition Diagram For a Binary Mixture of Benzene and Toluene 383.3 378.3 373.3 368.3 363.3 358.3 353.3 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1. mol Fraction of Benzene Temperature (K)

6. Using the figure below, what is the composition of the vapor from a solution containing 20 grams of toluene and 40 grams of benzene? Show all your work. Composition Diagram For a Binary Mixture of Benzene and Toluene 383.3 378.3 373.3 368.3 363.3 358.3 353.3 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1. mol Fraction of Benzene Temperature (K)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 31E: Common commercial acids and bases are aqueous solutions with the following properties: Density...

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The experimental data in the table was collected during a freezing point depression study where BHT (butylated hydroxytoluene) was the solvent. Mass of BHT Mass of unknown Freezing point of pure BHT Freezing point of BHT and unknown solution Kf for BHT 7.709 g7.709 g 1.252 g1.252 g 74.17 ∘C74.17 ∘C 70.91 ∘C70.91 ∘C 6.83 ∘C/?6.83 ∘C/m Use this data to calculate the molar mass of the unknown solute. molar mass =
[Review Topics] [References) An automobile antifreeze solution contains 2.70 kg of ethylene glycol, CH2OHCH2OH, and 1.90 kg of water. Find the mole fraction of ethylene glycol in this solution. What is the mole fraction of water? Mole fraction of ethylene glycol %3D Mole fraction of water =
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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
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D. Freezing Point Calculation Directions: Study the sample problem and do the task given. Sample problem with solution, Task to do Ethylene glycol (C2H6O2) is a molecular compound Calculate the freezing point of a solution that is used in many commercial anti-freezes. An aqueous solution of ethylene glycol is used in. vehicle radiators to prevent the water in the radiator from freezing by lowering its freezing point. Calculate the freezing point of a solution of 400. g of ethylene glycol in 500.g of water. repared by dissolving 27.56 g of glucose (C6H1206) into 125 g of water. Step 1: List the known quantities and plan the problem. Step 1: Kf (H2O) = -1.86 °C/m %3D Known: mass of C2H6O2 = 400. g molar mass of C2H6O2 = 62.08 g/mol mass of H20 = 500. g = 0.500 kg Kf (H20) = -1.86 °C/m *Kf- is the constant freezing point %3D %3D %3D %3DD ni noiulge Unknown: Tf of solution = ? °C *Tf- is the total freezing point This is a three-step problem. First, calculate the moles of ethylene glycol.…