In the table, rank each substance by its boiling point (1 being the lowest, 4 being the highest) and rank each substance by its vapor pressure (1 being the lowest, 4 being the highest).
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- At 1 atm, a mixture of octane and methylbenzene boils at 135.8 degrees Celsius with a composition of 60% methylbenzene. The boiling points of methylbenzene and octane are 110.6 and 125.6 degrees Celsius, respectively. Draw a boiling point-composition diagram for the octane-methylbenzene mixture system, including all significant labels.A sample consists of butyric acid, acetic acid and ethylene glycol. At a distilling temperature of 162°C, the distillate will significantly consist of: I. Butyric acid (boiling point: 162°C)II. Acetic acid (boiling point: 118°C)III. Ethylene glycol (boiling point: 197°C)A. I and II only B. I onlyC. I,II, and IIID. III onlyThe separation and purification processes given below and the method used against them are given. Which or which of these pairings are correct? I. Brewing of tea - ExtractionII. Purification of water impurities - ChromatographyIII. Separation of olive pomace from olive oil while producing olive oil-DecantationIV.Petroleum fractions obtaining - Ordinary distillationV. Obtaining essential oils and using them in perfume making - Water-steam distillation
- 1.Prepare 250ml of 70% and 90% ethyl alcohol from 95% ethyl alcoholusing the formula: C1V1=C2V2.True or false: Naphthalene is more soluble in dichloromethane than is sodium benzoate.In the lab instructions, it gives you the mass of the ice added to the calorimeter. Why is the mass of the ice important to obtain the molality? Hint: Think about what is present in the solution and how the molality gets computed. Instead of giving you the massed sample, the instructions now tell you to measure out 45g of ice. In your screenshot, show the balance with a beaker with ice massing ~45g. On in-person labs, you would grab an empty beaker, tare the mass of it, remove the beaker from the balance, add the ice, and then place it back on the balance
- Calculate the missing data in the following table. Compound ΔHvap (kJ/mol) ΔSvap [J/(mol·K)] Boiling Point (°C) hexanoic acid 71.1 105.7 hexane 28.9 85.5 69 or 68.73 formic acid 60.7 100.8 1-hexanol 44.5 157.5 The text states that the magnitude of ΔSvap tends to be similar for a wide variety of compounds. Based on the values in the table, do you agree?A student in New York City carried ou1t a boiling point determination for cyclohexane {b.p. 81• C) according to the procedure in this laboratory manual. Will this student's observed boiling point be the same as the value obtained by another student in Denver, Co'lorado.{Nicknamed the "Mile-High City" due to its high elevation)? Will it be lower or higher? Ex plain your conclusion.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.
- What is the molar ratio of 1,1-dichloroethane (11DCE) to 1,2-dichloroethane (12DCE) in the gas phase above the solution containing 10 mol of 1,1-dichloroethane and 10 mol of 1,2-dichloroethane at 20oC. The vapor pressure of 1,1-dichloroethane is 24.0kPa and the vapor pressure of 1,2-dichloroethane is 8.0 kPa at 20oC.Draw a temperature-composition diagram for the acetone-chloroform mixture, wherein the boiling points of acetone and chloroform are 329 K and 334 K, respectively. They supposedly form a high boiling azeotropic mixture at Xacetone = 0.34 with boiling point at 430 K.D. Preparation of 3% (vol/vol) Alcohol Solution1. Compute for the volume of denatured ethanol needed to prepare 25 mL of 3% (vol/vol) solution. Note that the concentration of the denatured alcohol stock solution is 98%.2. Explain in detail how the solution will be prepared in the laboratory.