Butyl Ethanoate

Ethyl ethanoate is made from ethanol and ethanoic acid. In the reaction sulphuric acid is added as a catalyst.

During the halogenation reactions of 1-butanol, 2-butanol, and 2-methyl-2-propanol, there is a formation of water from the OH atom of the alcohol, and the H atom from the HCl solution. The OH bond of the alcohol is then substituted with the Cl atom. Therefore all of the degrees of alcohol undergo halogenation reactions, and form alkyl halides as products. This is because the functional group of alkyl halides is a carbon-halogen bond. A common halogen is chlorine, as used in this experiment.

After synthesizing tert-butyl chloride, the melting point on the compound was found to be 47˚C. According to literature, tert¬-butyl chloride has a melting point of 51˚C, apart from a little bit of deviation, this shows that the correct compound was created. The percent yield obtained for the synthesis of tert-butyl chloride was 47.42%. This could have been due to errors that occurred in the lab. When moving the solution from one test tube or graduated cylinder to another some of the solution may still be left in the tube which lowers the percent yield. Also when working with a simple distillation setup, the vial is not distilled to dryness therefore some of the solution is not collected. Some of the solution can also be trapped on the side

The goal of this experiment was to synthesize aspirin. In this experiment aspirin, also known as acetylsalicylic acid, was synthesized from salicylic acid and acetic anhydride. In the reaction the hydroxyl group on the benzene ring in salicylic acid reacted with acetic anhydride to form an ester functional group. This method of forming acetylsalicylic acid is an esterification reaction. Since this esterification reaction is not spontaneous, sulfuric acid was used as a catalyst to initiate the reaction. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be present in the solution as well as some sulfuric acid, aspirin, and acetic acid. Crystallization, which uses the principle of

In this experiment, the Fischer Esterification of an unknown acid and an unknown alcohol was used to prepare an unknown ester. Sulfuric acid was used as a catalyst in the reaction which then was put under reflux. After cooling, the pH of the solution was raised to approximately 8 using sodium carbonate. Diethyl ether was added, then the aqueous layer was removed and the organic layer was washed with sodium chloride. The aqueous layer was removed again and sodium sulfate was added. The unknown product was then identified using gas chromatography (GC) to obtain the retention time.

At room temperature (25°C), esterification reactions are relatively slow, therefore requiring the rate of the chemical reaction to be increased for the products to be formed efficiently. This is implemented, by using a catalyst, such as concentrated sulphuric acid (H2SO4 (aq)), as well as by heating the mixture: using a heating mantle. As a result, the energy of the reactants can be greater than the activation energy, increasing the rate of reaction. Hence, as the reactants are relatively volatile, so reflux apparatus such as a pear-shaped flask and a Liebig condenser were used, to minimise the amount of reactants lost, as well as allow the reaction to take place at the highest temperature possible. In addition, boiling chips were added prior to reflux, to prevent bumping and a decrease a loss of volatile reactants, during the reflux

Carried out the microscale synthesis of isopentyl acetate by direct esterification of acetic acid and isopentyl alcohol. This was an acid catalyzed Fischer esterification. Both extraction and distillation were employed to obtain a pure product. IR spectroscopy and gas chromatography were used to determine purity of the final product.

GC shows me peaks and to identify them we use polarity. In the experiment, we used a non-polar column. 1-bromobutane is a colorless liquid that is insoluble in water and is a non-polar. Non-polar compounds leave longer retention time and polar compound leaves shorter retention time. My GC shows me peaks with high intensity with a longer retention time at 4.437 because that a higher intensity and a longer retention time we knew that that peak belongs to my 1-bromobutane. 1-butanol was also present in my GC because is more polar leaves a short retention time there before the peak that belongs to 1-butanol is at 3.762 retention time

Jack Kelly Experiment 2: Esterification Organic Chemistry II Lab CH224-53 Dr. Kwan Introduction Experiment 2 involves an esterification reaction, shown in figure 1. Each student was given an unknown, which consisted of an acid and alcohol mixed together. The unknowns all had low molecular weights, causing them to have a strong odor. For this reason, the unknowns were only supposed to be opened under the hood, so that no strong scents were sitting in the lab. Each unknown was heated and mixed with concentrated sulfuric acid, producing an ester and bi-product of water, which can be seen in figure 1 as well.

Butanol used to be produced via fermentation of biomasses (Acetone-Butanol-Ethanol) such as corn, sugar beets and other feedstock. Clostridium acetobutylicum microbes are placed into the sugars from the biomass. These then are converted into various alcohols including ethanol

An ester was synthesized during an organic reaction and identified by IR spectroscopy and boiling point. Acetic acid was added to 4-methyl-2-pentanol, which was catalyzed by sulfuric acid. This produced the desired ester and water. After the ester was isolated a percent yield of 55.1% was calculated from the 0.872 g of ester recovered. This quantitative error was most likely due to product getting stuck in the apparatus. The boiling point of the ester was 143° C, only one degree off from the theoretical boiling point of the ester 1,3-dimethylbutyl, 144 ° C. The values of the

The purpose of this lab was to synthesize the ester isopentyl acetate via an acid catalyzed esterification (Fischer Esterification) of acetic acid with isopentyl alcohol. Emil Fischer and Arthur Speier were the pioneers of this reaction referred to as Fischer Esterification. The reaction is characterized by the combining of an alcohol and an acid (with an acid catalyst) to yield and ester plus water. In order to accomplish the reaction, the reactants were

Distillation is used to separate mixtures that do not work well together. The simple distillation performed during lab is done to obtain a pure liquid, such as recycling waste acetone to retrieve purified acetone (4).

There are a few different steps into separating and purifying the ester from the mixture.

The first objective of this laboratory exercise is to gain an understanding of the techniques used in a “simple” distillation process by reviewing its use as a purification method. The second part of the laboratory is calculating the purity of distillation fractions by measuring and evaluating the physical properties of collected fraction samples. If performed correctly, two substances will be separated. Several pieces of laboratory equipment will be used to carry out the distillation process. Calculating the density and observing the boiling points of each fraction are the methods used to analyze the more pure products.