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)
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- 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.Bristol Community College Fall River, Massachusetts Experiment 6: Molar Mass of a Molecular Solid from Freezing Point-Depression Measurement Name: __________________________________ Date: _______________ Approved: ___________ DATA SHEET Mass of lauric acid (in Part II) Mass of benzoic acid (in Part II) Freezing temperature of pure lauric acid (from Part I) data from Video 2 of Part I Freezing temperature of solution (from Part II) data from Video referenced in Part II Freezing point depression, Tf ( = Tf, lauric acid – Tf, solution) Molality (m) of solution ( Eq. 1) Moles of benzoic acid ( Eq. 2) Experimental molar mass of benzoic acid (Eq. 3) Calculate the molar mass of benzoic acid, C6H5COOH. Percent error Summary Questions A student determines…Assuming that pentane and hexane form an ideal solution, A. Calculate the amount of pentane to be added to 65.0 g of hexane to obtain a minimum dG of mixing from mixing those two components. [MM pentane; 72.15, MM hexane; -86.18] B. Calculate the dS of mixing the components of the mixture above.
- The partial molar volumes of acetone and chloroform, in a solution in which the molar fraction of chloroform is 0.4693, are 74.166 cm3mol-1 and 80.235 cm3 mol-1, respectively. What is the volume of 1,000 kg of this solution? Data: M.M. (acetone) = 58.08 gmol-1; M.M. (chloroform) = 119.07 gmol-1.1. What is the mole percent of methanol in your starting solution (composed of 1.5 mL and 6 mL isopropanol)? 2. Using the vapor-liquid equilibrium data graph (NOTE: You have to make this graph using the data provided) and your answer from question 1, answer the following: If your first distillate was 49 mole percent methanol, how many theoretical plates were in your distillation setup? Data Mole % of Methanol Temperature (°C) Vapor Liquid 66.22 95.35 90.10 67.94 89.10 79.00 70.22 80.00 66.05 72.67 68.50 52.20 74.78 57.00 40.80 77.06 42.85 29.30 78.94 29.00 19.50 81.00 13.20 8.10Given that a mixture of nitric acid (bp 86 °C) and water forms a maximum-boiling-point azeotrope that boils at 120.7 °C with a composition of 67.4% nitric acid to 32.6% water. Construct an approximate boiling-point-phase diagram (with % composition on the x-axis and temperature on the y-axis) for this system. Include the boiling points of pure nitric acid, pure water, and the boiling point of the azeotrope on your diagram. Describe the behavior on distillation of a mixture that is 80% water and 20% nitric acid.
- 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.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 with 35% phenol at 60oC. Calculate the masses of these phases.Using the phase diagram for mixtures of cyclohexane and toluene, estimate: A) Boiling point of pure toluene _________ B) Boiling point (Tbp) of solution with molar fraction of toluene 30%.______ C) Molar fraction of toluene (in %) in the gas phase above the solution with molar fraction of toluene 30% at its boiling point Tbp. ____________ D) Approximate molar fraction of solvent which remains in the liquid phase upon heating of mixture with 60% of toluene to 100oC. _______________
- I’ve done this question but I think I’ve done it wrong. Calculate how much 95% Ethel alcohol will be prepared to dissolve 0.3g of sulfanilamide at 78 degrees using the table (pictured below from my textbook) and, based on that volume, calculate how much sulfanilamide will remain dissolved in the mother liquor after the mixture is cooled to 0 degrees. For the volume at 78 I got 1.47mL and for the difference once it cooled to 0 degrees I got 19.96 mL. If I got these wrong could you point me in the right direction as how to solve this? Thank you!3. Refer to the phase diagram depicted below: When 7 moles of A and 3 moles of B are mixed at 50oC which is then cooled to 10oC the sample turns into two liquid phases, phase I has mole fraction xB=0.14 (see diagram below). Find the phase II mole fraction xB, and then calculate the ratio of amount of substance in phase I to that in phase II using Lever rule. Please enter your answer as a number with two decimals. for example, if the ratio you calculated is 2:3, you enter as 0.67The 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 =