6.0 mL of cyclohexanol, 8 mL of 85% phosphoric acid, and 10 drops of sulfuric acid are added to a 50-mL round-bottom flask with boiling chips, and the mixture is distilled into an ice-cooled receiver. The distillate is in the form of a colorless bi-phasic mixture. The cyclohexene upper layer is removed from the water layer, and dried over anhydrous calcium chloride. Isolated is cyclohexene as a clear and colorless foul-smelling liquid. Weighing data is given below. Gross mass: 51.24 g Tare mass: 48.04 g Product mass: 3.2g Question: Calculate the theoretical mass of the cyclohexene product, bearing in mind that the cyclohexanol starting material was measured by volume, not by mass (so you must use the density of cyclohexanol to convert milliliters to grams, before calculating the number of moles). Calculate the percent yield of cyclohexene obtained.

6.0 mL of cyclohexanol, 8 mL of 85% phosphoric acid, and 10 drops of sulfuric acid are added to a 50-mL round-bottom flask with boiling chips, and the mixture is distilled into an ice-cooled receiver. The distillate is in the form of a colorless bi-phasic mixture. The cyclohexene upper layer is removed from the water layer, and dried over anhydrous calcium chloride. Isolated is cyclohexene as a clear and colorless foul-smelling liquid. Weighing data is given below. Gross mass: 51.24 g Tare mass: 48.04 g Product mass: 3.2g Question: Calculate the theoretical mass of the cyclohexene product, bearing in mind that the cyclohexanol starting material was measured by volume, not by mass (so you must use the density of cyclohexanol to convert milliliters to grams, before calculating the number of moles). Calculate the percent yield of cyclohexene obtained.

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter7: Extraction

Section: Chapter Questions

Problem 1Q

See similar textbooks

Similar questions

Oral rehydration salts are stated to contain the following components: Sodium Chloride 3.5g Potassium Chloride 1.5g Sodium Citrate 2.9g Anhydrous Glucose 20.0g 8.342 g of oral rehydration salts are dissolved in 500 ml of water. 5 ml of the solution is diluted to 100 ml and then 5 ml is taken from the diluted sample and is diluted to 100 ml. The sodium content of the sample is then determined by flame photometry. The sodium salts used to prepare the mixture were: Trisodium citrate hydrate (C6H5Na3O7, 2H2O) MW 294.1 and sodium chloride (NaCl) NW 58.5. Atomic weight of Na = 23. The content of Na in the diluted sample was determined to be 0.3210 mg/100 ml. Determine the % of stated content of Na in the sample. The stated should be 104.5, how??
Below are the gas chromatography results of two separate distillations of the same 1:1 mixture of ethanol and 1-butanol. One sample was obtained from the first fraction of a simple distillation and one sample was obtained from the first fraction of a fractional distillation. Identify the peaks in the chromatographs. Discuss the conclusions you can make regarding simple distillation compared with fractional distillation. Which method was more successful?
A 25 g of butyric acid was extracted with 400 mL ether from 400 mL water (Kd=3.0 at 25 °C) Using single-step extraction, what is the amount of butyric acid in water layer? What is the total amount of butyric acid extracted using two successive extractions? Calculate the % efficiency of two-step extraction over single
5.0 mL of 1-butanol was mixed with 10 mL of HCl. The reaction was put on an ice bath and 4 mL of concentrated sulfuric acid was added. This mixture was refluxed for 45 min and then the product was co-distilled with water using a simple distillation apparatus. Water and the product are immiscible. 1-butanol has a molar mass of 74.12 g/mol, a density of 0.810 g/mL, and a boiling point of 118 C. The product has a molar mass of 92.57 g/mol, a density of 0.880 g/mL, and a boiling point of 78 C. What is the nucleophile in this reaction? What is the role of H2SO4 in this reaction? Calculate the theoretical yield for this reaction. Give your answer in grams. Select the following statements that can be said about the reaction shown.
11. How much caffeine can be extracted using 50.0ml of DCM if a tea bag contains 15 grams of tea leaves with 0.9% of caffeine? And has undergone solid-liquid extraction with 100ml of distilled water followed by liquid-liquid extraction using DCM. The solubility of caffeine requires 15 ml of water and 2.0ml of DCM for 40.0mg. a 6.1 x 10^-5 b 6.0 x 10^-5 c 7.0 x 10^-5 d 7.1 x 10^-5
You were given a mixture of two miscible solvent A and B that you are tasked to separate. You know that solvent A has a boiling point of 49 oC while solvent B has a boiling point of 174 oC. Which of the listed method would overall be the most efficient? Fractional distillation Recrystallization Solid-liquid extraction Liquid-liquid extraction Simple distillation Acid-Base extraction
20 tablets containing the dibasic drug ethambutol hydrochloride (MW 277.2 g/mol) were powdered. 0.3354 g of tablet powder was dissolved in 10 mL of 2 M sodium hydroxide and was extracted with 5 x 25 mL quantities of chloroform. The combined extracts were evaporated and the residue was dissolved in 100 mL of anhydrous acetic acid. Non-aqueous titration was carried out using 1-naphtholbenzein solution as indicator and 0.1014 M acetous perchloric acid. Volume of acetous perchloric acid required = 14.2 mL, weight of 20 tablets = 3.367 g, state content of ethambutol hydrochloride per tablet = 100 mg. Calculate the % of stated content in the tablets.
0.56 g 1,4‐dimethoxybenzene, 0.9 mL 2‐chloro‐2‐methylpropane, 5 mL nitrobenzene and 0.52 g graphite were combined, and the mixture was refluxed for 1.5 hours. It was then cooled to room temperature and filtered. The filtered graphite was washed with 15 mL hexane. The filtrate was distilled under vacuum to remove any remaining 1,4‐dimethoxybenzene, 2‐chloro‐2‐ methylpropane and nitrobenzene (6.3 g), yielding 0.44 g 1,4‐di‐tert‐butyl‐2,5‐dimethoxybenzene (43.4% yield). What is the Atom economy, E factor, and effective mass yield?
A binary mixture of benzene and toluene containing 57.47 mol% benzene is continuously distilled. The distillate contains 90.40 mol% benzene, while the bottom product contains 86.96 mol% toluene. What molar flow rate of the bottom product will correspond to 183.11 mol/h of the distillate product? Type your answer in mol/h, 2 decimal places.
1a) Hexane, CH3(CH2)4CH3, is found to have a long retention time when separated from a mixture. A column with a C18 (18-carbon chain) stationary phase and a methanol-water modal phase is used for the separation. Explain why hexane has a long retention time. 1b)You wish to chromatographically seperate a mixtureof the follwing compunds. Which of the two compounds will be most difficult to seperatate from one another? Why?
You obtain an Unknown Sample from the Stockroom. You begin testing the solution through the steps outlined in the flowchart of the experiment’s PDF file. You first add HCl and centrifuge your mixture. You observe the formation of a white precipitate in the bottom of the test tube. After pouring off the supernatant liquid, you add hot water to the white precipitate. Upon addition of the hot water, you have some white precipitate still at the bottom of the test tube, and the supernatant liquid is poured off. To this liquid, potassium chromate (K2CrO4) is added. Upon this addition of potassium chromate, you observe no formation of precipitate. Which of the following is a valid conclusion to draw at this point? (Choose one.) Select one: 1. Hg22+ is definitely present. 2. Pb2+ is NOT present. 3. Ag+ is definitely present. 4. Pb2+ is definitely present.
what are key reactions involved in seperation of liquid mixtures by simple and fractional distillation and gas chromatography? chemicals used: 10ml 1:1 mixture of ethyl and butyl acetate techniques: simple and fractional distillation, gas chromatography. target molecules: Ethyl acetate C4H8O2 Butyl acetate C6H12O2