Simple Distillation, Gas Chromatography: Preparation of Synthetic Banana Oil

How was this lab activity similar to other labs that you have done in the past?

According to the group data, which Mrs. Harmon went over to ensure groups received accurate data, the original solution had an inconstant boiling point which reached 2 plateaus (85°C and 100°C) before all the liquid evaporated, a medium odor like alcohol, was flammable, had a density of about 0.91g/100cm3, and did dissolve sugar. The 2 plateaus show that there were two substances in the original mixture, which have 2 different boiling points. These boiling points are the points that the substances can be separated. Based on the two boiling points and the odor, groups predicted the two substances were isopropanol and water. Fraction 1 had a boiling point of about 85°C, a strong odor like alcohol, was flammable, had a density of about 0.84g/100cm3, and did not dissolve sugar.

Since Alka Seltzer is swallowed and reacts with stomach acid, the vinegar is in this experiment is substituting as the stomach acid. The principle of limiting reagents relates to this lab because

Fraction #2 was found mixed with isopropanol alcohol in the sludge. It was not separated from the mixture initially, but before performing the test, it was concentrated on a hot plate.

At the end of distillation it is possible to obtain an ester product with low purity. Low purity occurs as the result of excess water collected with the distillate. Thus, in order to increase purity, distillation should be undertaken with a great deal of

In Part A of the experiment, isoborneol was oxidized. First, 0.5 grams of isoborneol was dissolved in 1.5 mL of glacial acetic acid inside a 25 mL Erlenmeyer flask. Next, 4.0 mL of household bleach was added to the solution with swirling. The solution was swirled for the next 15 minutes and then was tested against starch-iodine paper. If there was a blue color, then that indicated there was an excess of NaOCl. If the test was negative, a small amount of bleach (~0.5 mL) was added and tested again. The mixture was then diluted with 15 mL of water and transferred to a separatory funnel. 15 mL of diethyl ether and 0.5-1.0 mL NaHSO3 was added. The funnel was shaken and the layers were allowed to separate. The aqueous layer was removed. The ether layer was washed (separated) with 10 mL NaHCO3 solution. The aqueous layer was then tested against litmus paper to confirm that it was basic. The ether layer was dried by anhydrous Na2SO4.

The experiment that we carried out was to find the energy given off by the burning of each of the alcohols. We set a beaker of water on a ring stand over an alcohol burner. Then we lit the alcohol burner and burned it for 2 minutes. We also took temperature before we started and after we ended so that we could do the calculations. The other thing we did so that we could do the calculations was mass the alcohol burner before and after so that we could know how much of the alcohol was burned.

Abstract: The purpose of this experiment was to synthesize Isoamyl Acetate, the fruity ester that produces a banana fragrance, by a reversible reaction called esterification. The reaction was prepared by the process of refluxing a solution of acetic acid and 3-methyl-1-butonal. The organic layer of solution was processed through a distillation apparatus where an impure fraction and pure fraction was collected. Infrared (IR) spectroscopy data was collected on both fractions and compared to an IR ran on the starting alcohol (3-methly-1-butonal). The actual yield was 15.3 grams less than the theoretical yield producing a percent yield of 34.8 %. The IR data determined the starting alcohol was present in the final product indicating the sample was impure.

(Mueller). The next step to the process was to add 1mL of Ethanoic acid into Ethanol. Ethanoic acid into Ethanol smelled similar to vinegar and the smell got stronger than Ethanol placed in a beaker. Once the Ethanoic acid and Ethanol were mixed and heated in the presence of Sulfuric acid, an esterification reaction was taking place. The odour was stronger allowing detailed observations of the ester formed.

Objective In this combinatorial experiment, an acid and alcohol were used as reactants in order to produce esters. In order to determine the acid and alcohol used in the reaction, gas chromatography and the smell of the esters formed were used to determine the acid and alcohol. Raw Data Experiment 1 (CA1 with 2 alcohols) and Experiment 2 (CA2 with 2 Alcohols) were performed in this lab. Table 1: Physical Observations of Products Formed in Each Experiment Experiment Number Product Forms Physical Observations 1 2 Smell of cinnamon 2 2 Smell of artificial fruit/candy 3 2 Smell of strawberries 4 2

For the first part of the experiment the fractionating column was set up and a 25-mL sample of toluene and ethyl acetate was prepared and placed into a round beaker. The Bunsen burner was turned on and the mixture was heated to a boil. The vapor from the boiling mixture condensed in the condenser and was collected in a 50-ml graduated cylinder. As the first drop of substance was collected the temperature at that instant was recorded and corresponded with the first 1-mL of substance collected. For volumes 1-mL through 5-mL the amount was estimated as the substance filled the graduated cylinder. The mixture was heated until the graduated cylinder was filled up to 15-mL. For the second part of the experiment simple distillation was used. The process

The entry discussed ways in which to improve percentage yield when synthesizing flavor acetates, Isoamyl acetate (Isopentyl acetate) was used to test these changes. The article had a percentile yield of 80% an 22.31 difference in percentage yield that what was obtained in the lab period, adjusting to these changing could help improving the results. The broader impact is that Isopentyl acetate is a natural occurrence in banana plants and is produced synthetically to mimic banana flavor in foods.

To begin, we added 6 M HCl drop by drop and 1 mL ethanol to our sodium acetate solution. If carbonate was present, effervescing was supposed to occur because carbon dioxide was a produced. Lastly we conducted the acetate test. We added one drop of concentrated sulfuric acid to 1 mL ethanol and combined these to our unknown solution. If acetate was present in the solution, a fruity scent was supposed to occur.

The reflux reaction (equation) is a chemical reaction that occurs in equilibrium. The forward reaction, that is the production of ester, will be favoured until the limiting reagent has been exhausted. In our experiment, butanol is the limiting reagent, therefore, once this reactant has been exhausted the reaction will then proceed in the opposite direction, favouring the production of the reactants. This reverse reaction is an example of a hydrolysis reaction. In this instance, the reverse hydrolysis reaction will only proceed correctly in the presence of water while in acidic conditions.

The procedure was performed as follows: For run 1, 20cm3 of acetone, 10cm3 of sulphuric acid and 145cm3 of water was added to a conical flask. 25cm3 of iodine was then added to this solution which started the reaction and immediately, 20cm3