Literature Review On Esterification Of Methanol

Salicylic acid was esterfied using acetic acid and sulfuric acid acting as a catalyst to produce acetylsalicylic acid and acetic acid. The phenol group that will attack the carbonyl carbon of the acetic anhydride is the –OH group that is directly attached to the benzene since it is more basic than the –OH group attached to the carbonyl 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. Sulfuric acid serves as the acid catalyst since its conjugate base is a strong deprotonating group that is necessary in order for this reaction to be reversible. The need for the strong conjugate base is the reason why other strong acids such as HCl is not used since its conjugate base Cl- is very weak compared to HSO3-. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be present in

Alcohol dehydrations are widely used in many industries to produce alkene. In this experiment 2-methylcyclohexanol was dehydrated to three possible products using phosphoric acid as a catalyst. The main tool for this experiment is the Hickman still. First, Drierite was added to the Hickman still so that any excess water formed during the experiment will be absorbed. It also acted as a boiling stone and addition surface to increase surface area. Next, 0.75 mL of 2-methylcyclohexanol is added to the still and right after 1 mL of phosphoric acid is added. The phosphoric acid (H3PO4) acts as a catalyst in order for the reaction to occur. The mixture is heated up to between 120o Celsius and 160o Celsius. If the temperature goes above 165oC then

The mixture is extracted with sodium bicarbonate because doing so will cause any unreacted acid to react with the sodium bicarbonate to become neutralized. The neutralized acid, being water soluble, would then separate from the ester, which is water insoluble. This causes an increase yield of pure product.

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.

After 10 minutes the reaction liquid was separated from the solid using a vacuum filtration system and toluene. The product was stored and dried until week 2 of the experiment. The product was weighed to be 0.31 g. Percent yield was calculated to be 38.75%. IR spectra data was conducted for the two starting materials and of the product. Melting point determination was performed on the product and proton NMR spectrum was given. The IR spectrum revealed peaks at 1720 cm-1, which indicated the presence of a lactone group, and 1730 cm-1, representing a functional group of a carboxylic acid (C=O), and 3300cm-1, indicating the presence of an alcohol group (O-H). All three peaks correspond with the desired product. A second TLC using the same mobile and stationary phase as the first was performed and revealed Rf Values of 0.17 and 0.43for the product. The first value was unique to the product indicating that the Diels-Alder reaction was successful. The other Rf value of 0.43 matched that of maleic anhydride indicating some

This first section involved several important pieces of information regarding the experiment as a whole, both conceptually what is going on, as well as what is happening experimentally. If we note the amount of acetic acid used, it would be realized that within the actual equation, there is a 1:1 ratio between the acetic acid and isopentyl alcohol needed to do the reaction. But, as noted in the introduction and in the scenario, There is an equilibrium constant of 4.2. This means that the esterification reaction that we are completing is reversible, and if we began with equimolar amounts of acetic acid and isopentyl alcohol, we would only have about two-thirds of our reactants converted to isopentyl acetate once the hour under reflux was completed. Because of this unfortunate equilibrium constant, the

The purpose of this experiment was to synthesize isopentyl acetate via an esterification reaction between acetic acid and isopentyl alcohol, using concentrated sulfuric acid as a catalyst. The product was washed with sodium hydrogen carbonate, as well as with water, then dried with anhydrous sodium sulfate. The product was then distilled using a Hickman still and characterized using infrared spectroscopy. The percent yield of isopentyl acetate was 61.52%. This may have been low due to not all of the condensed product being removed from the Hickman still, some product being lost during transfer of the product from the reaction tube into the Hickman still, or the loss of some product due to evaporation during distillation.

The dehydration of 2-methyl-2-butanol was performed using sulfuric acid and phosphoric acid in order to synthesize alkene products 2-methyl-1-butene and 2-methyl-2-butene. After carrying out steam distillation to isolate the organic alkenes from aqueous components within the reaction mixture, the purity and characterization of the products were then assessed through various analytical methods including Gas Chromatography (GC), Infrared Radiation (IR) Spectroscopy, and Nuclear Magnetic Resonance (NMR) Imaging. Through the characterization of the final products, it was found that little impurities remained in the final reaction solution and according to the GC, no alcohol remained in the vial after the reaction was complete. The actual yield

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

A good yield of isopentyl acetate was obtained during this experiment. Loss of the product was likely through transferring liquid from separatory funnel to the Erlenmeyer flask and residual material left in the distillation flask. Using an organic solvent like benzene or cyclohexane as a transfer agent would improve the yield, since their boiling points were around 80 oC and could be easily separated from the final product through simple distillation. However this

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

In this experiment, a Fischer Esterification reaction was performed with two unknown compounds. The unknown compounds, Acid 2 and Alcohol D, were identified by using the knowledge of the reaction that took place, and the identity of the product that was synthesized. The identification of the product resulted from analysis of IR and NMR spectra.

In recent years, the biotechnological use of xylans and xylanases has grown remarkably (Aristidou and Pentillä 2000; Subramaniyan and Prema 2002; Beg et al., 2001; Techapun et al., 2003). The end-products of xylan degradation of considerable importance in commercial applications are furfural and xylitol (Parajó et al., 1998). Xylan can be converted to β-D-xylopyranosyl and its oligosaccharides via two types of hydrolysis: acid or enzymatic. Acid hydrolysis is often preferred because it is faster, but it is accompanied by the formation of toxic compounds that may hinder subsequent microbial fermentation. Furthermore, in the long run, it can lead to corrosion of the metallic equipment that comes in contact with the acid. Recently, some industrial companies have shown interest in the development of efficient enzymatic processes to be used instead of acid hydrolysis in the treatment of material containing hemicellulose. Commercial xylanases are industrially produced, for example, in Japan, Finland, Germany, Republic of Ireland, Denmark, Canada and the USA. The microorganisms used to obtain these enzymes are Aspergillus niger, Trichoderma sp. and Humicola insolens. Nevertheless, commercial xylanases can also be obtained from bacteria. Xylanase began to be used in the 1980s: initially in the preparation of animal feed and later in the food, textile and paper industries. Currently, xylanase and cellulase, together with pectinases, account for 20% of the world enzyme market.

The purpose of this study is to produce succinic acid from glycerol residue through anaerobic fermentation process. The study of reaction parameters (pH, temperature and mass substrate) was performed by using expert design software in glycerol recovery process. One factor at one time (OFAT) method was performed as preliminary studies for selection of parameters range and subsequently determine its optimum condition using response surface methodology (RSM). The concentration of glycerol and succinic acid were determined using HPLC analysis. The FTIR spectrometry was applied to examine the adsorption of organic element. Statistical optimization (Respond Surface design Methodology) showed that optimal conditions were at pH, 2, temperature 35 0C and substrate 110.36 gram. At this optimum, 159.312 g/L was recovery of glycerol was obtained. Succinic acid was produced via fermentation process by using Escherichia coli type k-12 under 19.67 g/L initial glycerol concentration, 200 rpm rotation speed and at temperature 37 0C. The work resulted 0.66983 g/L succinic acid been produced. The study also investigated succinic acid production from commercial glycerol and its resulted about 0.73337 g/L. Overall, this research showed that the glycerol waste can be used as a carbon sources to produce succinic acid via fermentation process by using Escherichia coli type k-12. From the fermentation process, the succinic acid production does not exist as a major product. From this situation, the

Lipase is the enzyme that also known as triacylglycerol acylhydrolase with EC number 3.1.1.3. It is part of hydrolases family that act on carboxylic ester bond. It had been widely used as biocatalysts in biological process. Most of the lipase was expressed from natural resources such as plant, animal and microorganism. Lipases expressed from microorganism particularly interest due to easy production, capability to adapt in industrial application (Wang et al., 2017), stability in organic solvent, no cofactor required and broad substrate specification (Aravindan et al, 2006). The function of the lipase is to breakdown the triacylglycerol into free fatty acid and glycerol. In addition, it also involved in many synthesis reaction such as esterification, transesterification and aminolysis (Rivera et al., 2017). Due to its ability to breakdown lipid and many biological reactions, lipase is commercially used in large scale production.