Santol Peelings as Potential Source for Ethanol

3. Turned off the laboratory burner and observed the properties of the product in the evaporating dish.

Planning My aim for this experiment is to see the energy produced from different alcohols. This investigation involves burning alcohol in the air. ‘GCSE Chemistry’ by B.Earl and L.D.R Wilford says that "alcohols form, another homologous series, with the general formula Cn H2n+1OH ". The alcohol reacts with the oxygen in the air to form the products water and carbon dioxide.

The experiment began by mixing the initial 1.775g isopentyl alcohol with 2.3 mL acetic acid and about 5 drops sulfuric acid. This reaction mixture was then heated under reflux for an hour after boiling of the reaction mixture began.

(Table 2) Water Sucrose Ethanol NaCl Observed 165 114 72 97 Expected 109 109 109 109 (observed-expected) 56 5 -37

From the data analysed, a clear trend is seen. As the amount of carbon chains (and consequently molar mass) increases, so does the heat of combustion released. The hypothesis was stated as: “because 1-hexanol has more carbon bonds, it will produce the most amount of heat in the shortest period of time. By following the same reasoning, it is suggested that 1-hexanol will be followed by 1-pentanol and 1-butanol, respectively.” The experimental values show there is a linear relationship between the carbon chains and molecular weight, and the heat of combustion

In this experiment, an unknown alcohol underwent a Fischer Esterification reaction by reacting it with acetic acid as well as sulfuric acid catalyst. The unknown product material was purified through distillation and characterized by analyzing an IR spectrum and determining the density of the product. In addition, the boiling point test was performed to test for an ester. Lastly, the starting material, an unknown alcohol, was determined after finding out the product and examining the IR spectrum for the reactant.

Under Peak 0.6 Vs 4.75 Vs Retention Time 345s 385s GC yielded four peaks, one for water, ethanol, 3-methylcyclohexene, and 1-methylcyclohexene. The retention times were 83, 117, 345, and 385 seconds respectively. There is an approximant ratio of 1:7.9 3-methylcyclohexene to 2-methylcyclohexene.

You then take scissors or a knife and cut one hole on the side of the turkey baster or car filler. The car filler/ turkey baster should be facing upwards with the open end of the turkey baster facing up with the handmade hole on the side of it. Then you take apart the spark igniter and reassemble it in the turkey baster or car filler so that the part you spin to create the spark is the only part sticking out of the handmade hole. That is when you use the screwdriver and wrench to take apart and put back together the spark igniter. The cannon is finished when the spark igniter is properly assembled and is able to create a spark. To finish the experiment you then need to add ten to fifteen drops of rubbing alcohol inside of the turkey baster or car filler. When you are in a safe open area where no one is around you can then spin the spark igniter knob really fact to create a spark with the rubbing alcohol and launch the ball out of the cannon. The cannon won’t work properly if there is a dent in the ball. The ball won’t launch if there is a dent because the dent allows oxygen to get into the cannon and the combustion won’t work

The purpose of this assessment was to characterize the pre-blended GPS (Grain Processing Corporation) alcohol, a mixture of 190/200 proof SDA-3A alcohols, produced from corn feedstocks (yellow No. 2 dent. corns) through enzymatic, fermentation, and distillation methods. For this purpose, the chemical and physical properties as show in the Certificate of Analysis (CoA) of the SDA-3AU were considered and their effects were investigated. This was performed by comparing the typical and acceptable limits of the weight percentage of total alcohol and methanol in the SDA-3AU against the current

Procedure: We held our plastic over the flame and observed the way our plastic burned.

For instance, pentan-1-ol, the alcohol utilised to synthesis 1-pentyl ethanoate, is relatively flammable due to the hydroxyl functional group attached to the molecule. Therefore, in order to prevent severe burns, a laboratory coat and safety glasses were worn. The experiment was additionally performed whilst standing up, so that if the aliquot of pentan-1-ol ignited,

Purpose: The purpose of the experiment was to perform the acid-catalyzed Fischer Esterification of acetic acid and isopentyl alcohol to form isopentyl acetate, or banana oil, which is used in flavor industries. The equilibrium of the reaction was changed by adding an excess amount of acetic acid. The reaction was refluxed and product was purified by extraction and distillation. Isopentyl acetate was analyzed by infrared spectroscopy and 1H NMR spectroscopy.

A 10 mL round-bottom flask was weighed both before and after approximately 1.5 mL of the given alcohol, 4-methyl-2-pentanol, was added. 3 mL of glacial acetic acid, one boiling chip, and 2-3 drops of concentrated sulfuric acid were added to the flask in that order. The reflux apparatus was assembled, the

An ice bath was prepared in a large beaker and a small cotton ball was obtained. 0.5 g of acetanilide, 0.9 g of NaBr, 3mL of ethanol and 2.5 mL acetic acid was measured and gathered into 50mL beakers. In a fume hood, the measured amounts of acetanilide, NaBr, ethanol and acetic acid were mixed in a 25mL Erlenmeyer flask with a stir bar. The flask was plugged with the cotton ball and placed in an ice bath on top of a stir plate. The stir feature was turned on a medium speed. 7mL of bleach was obtained and was slowly added to the stirring flask in the ice bath. Once all the bleach was added, stirring continued for another 2 minutes and then the flask was removed from the ice bath and left to warm up to room temperature. 0.8mL of saturated sodium thiosulfate solution and 0.5mL of NaOH solution were collected in small beakers. The two solutions were added to the flask at room temperature. The flask was gently stirred. Vacuum filtration was used to remove the crude product. The product was weighed and a melting point was taken. The crude product was placed into a clean 25mL Erlenmeyer flask. A large beaker with 50/50 ethanol/water

The results that were revealed were thought to be accurate and reliable as many factors were controlled to enable the best quality. The results that a constant rise in the combustion occurred as each alcohol’s carbon chain increased with one exception indicates that the reliability of this experiment has to be examined. With such a high percentage error from these results means they cant be definitive. Also only three trials were conducted on the five different alcohols. If the experiment were to be conducted again I would conduct five trials on each alcohol to get a better average.