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Q: In most distillations, the total volume of liquid obtained (distillate + residue) is not equal to…
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Q: Why is it necessary to pulverize the sample in doing the experiment of melting point?
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A:
Q: Under what conditions can a good separation be achieved with a simple distillation?
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- Uranium tetrafluoride and zirconium tetrafluoride melt at 1035 °C and 912 °C respectively. They form a continuous series of solid solutions with a minimum melting temperature of 765 °C and composition x(ZrF4) = 0.77. At 900 °C, the liquid solution of composition x(ZrF4) = 0.28 is in equilibrium with a solid solution of composition x(ZrF4) = 0.14. At 850 °C the two compositions are 0.87 and 0.90, respectively. Sketch the phase diagram for this system and state what is observed when a liquid of composition x(ZrF4) = 0.40 is cooled slowly from 900 °C to 500 °C.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. _______________1 g of organic matter dissolved 20 times more in ether than water is dissolved in 500 cm3 of water. Organic matter will be extras from the aqueous phase using 20 cm3 of ether each time. How many times should the extraction phase be repeated to extraction at least 90% of organic matter massively?
- A mixture of 20 mL of isoamyl acetate (MW=130.2 g/mol and density= 0.88 g/mL) and 20 mL of methyl benzoate (MW= 136.2 g/mol and density =1.09 g/mL) is distilled. Calculate the mole percent for each component. Use these mole percents and the figure below to answer the following questions.a. What is the initial boiling point of this mixture?b. What is the composition of the vapor in equilibrium with the liquid? Is this composition the same as the composition of the initial condensate from simple distillation?c. Instead of a simple distillation, you decide to use fractional distillation. Assuming two theoretical plates, what is the composition of the first fraction collected?Need solution to all parts urgently The solubility of 1,1,2-trichloroethane in water is 4500 mg/l; the vapor pressure is 30.0 mm Hg. Compute Henry’s constant in units of: a) atm b) dimensionless mole fraction c) atm∙m3/mol d) dimensionless concentrationA solution was prepared by dissolving 35.0 mL of methanol in sufficient water to give a total volume of 115.0mL. Compute for the percent by volume (%v/v) of the said solution. 30.4% 0.23% 23.3% None of the above 0.30%
- The distribution coefficient, KD (C water/C ether), between ether and water for aspirin at room temperature is 0.30. What weight of aspirin would be extracted by a single extraction with 300 mL of water from a solution of with a concentration of 0.67 M? Calculate the weight of aspirin which would be removed by three extractions with 100 mL portions of water. Compare the weight of solute extracted in single extraction process with the triple extraction process. Take note: The volume of the solution is 100mlAssuming 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.Given 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.
- 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.To verify Beer’s Law for solution of KMnO4 or K2Cr2O7 using colorimeter.Sodium chloride (NaCl) was isolated from SiO2 and CaCO3 by dissolving it in distilled water. Unmentioned is that CaCO3 is slightly soluble in water (0.001 g/100 mL). Describe the effect this fact will have on each component of the mixture: will the “isolated“ mass of each be greater than, equal to, or less than that in the sample?
