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Introduction steam distillation
Discussion for simple distillation
Introduction steam distillation
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Recommended: Introduction steam distillation
Intro
The main objective of this experiment is to separate Eugenol compound from cloves through a process of steam distillation method, and to assess the effectiveness of the method. Steam distillation is a type of distillation process in which organic compounds can be distilled using steam, and does not use vacuum system. In order for the process take place, the very first step is to carefully boil the mixture in a set point, which is slightly below boiling point of water. The vapor, which is the distillute are separated from the cloves and water. It is then transfer to the round bottomed flask as the vapor condense again through the condenser.
Theory
Natural aromatic compounds like eugenol tend to decompose at high sustained temperatures.
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Fundamentally, each compound has its vapor pressure. In this case, the water’s vapor pressure at 100 C is 760 mmHg, which is equal to the atmospheric pressure, and eugenol’s vapor pressure at 100 C is 4 mmHg. Eugenol’s vapor pressure contributes to the vapor pressure of the mixture. Using the Clausius-Clapeyron equation (ln (P1 / P2) = (ΔH / R) (1/T2 - 1/T1)), the temperature at which water boils in the partial vacuum of 4 mmHg was determined, which is less than 99.8 …show more content…
It is comparable with vacuum distillation process in which the purpose is to lower the vapor pressure below the atmospheric pressure in order for the organic materials distills and be purified under their usual boiling point. Steam distillation is very effective in distilling and purifying the eugenol; however, vacuum distillation have more applications, purifying the product even more. In this experiment, where steam distillation is being utilized, the analyte deemed to have impurities after testing it using H NMR. Cloves are made up of eugenol by 17% percent. Theoretically, that is also the maximum amount that can be distilled and be purified; however, that is not the case. With composite errors such as human error and how the distillation process work, it is impossible to get the most pure
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Introduction In this experiment, steam distillation was used to isolate eugenol oil from cloves. The goal of this experiment was to test and analyze the purity level of the eugenol oil that was isolated by applying a TLC test as well as H-NMR spectra. At the end of this experiment, eugenol oil was isolated, but some errors that occurred during the experiment resulted in impurities in the final isolated oil.
Once the mixture had been completely dissolved, the solution was transferred to a separatory funnel. The solution was then extracted twice using 5.0 mL of 1 M
Benzyl bromide, an unknown nucleophile and sodium hydroxide was synthesized to form a benzyl ether product. This product was purified and analyzed to find the unknown in the compound. A condenser and heat reflux was used to prevent reagents from escaping. Then the solid product was vacuum filtered.
The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed.
Performing this experiment, we used the technique called Acid-Base extraction to isolate Eugenol, which is one of the main ingredients of clove oil. Acid-Base extraction is the most efficient method for isolating organic component; it is efficient because it purifies the acid and base mixture based on their chemical identities. We have seen throughout this experiment that acid and base play an important role, when it comes to solubility in water. Our basic knowledge of acid and base is acid is a proton donor and base is a proton acceptor. This ideology helps us to understand why organic compounds are not soluble in water. When compounds tend to be insoluble, we have to use acid and base reaction, to change its solubility. The changes that occurred
After successfully isolating the eugenol and acetyleugenol, all that was left was to weigh each product. Once the lab was completed and the masses of the products were weighed, a 1.8% recovery of acetyleugenol as well as a 4.59% recovery of eugenol were obtained. These values may seem low, but in reality they may not be. This is because the amount of eugenol and acetyleugenol initially contained in the 25 grams of cloves is unknown. However, it is possible there were sources of error that occurred during the lab. A mechanical source of error would be spilling small amounts of solution while transferring it to different containers (beakers/flasks). Other sources of error could include incomplete reaction. This may be due to a lack of mixing
The joints were greased well to prevent vapor loss. 15 mL of the sample used and two boiling chips were placed in the distilling flask. The flask was heated with a hotplate in an oil bath. In separate, numbered, and calibrated test tubes, 0.5 mL of the distillate were collected while the temperature was recorded when each fraction was collected. The distillation was stopped when the temperature reached above 90˚. The set-up was cooled and the remaining liquid in the distilling flask were poured into a graduated cylinder. The volume was recorded. The temperature reading versus the volume of distillate were now plotted. The percent ethanol was computed.
The objective of this experiment was to use a common method of separation distillation. Distillation can be used in purifying or separating liquids, when the liquid if heated the more volatile component, the molecule with the lower boiling point, vaporizes and can be condensed. This type of separation will work efficiently when the feed mixture has a decent range between the boiling points of the components. The relationship between component’s vapor pressure to the composition of the solution is Ptotal==P1+P2, Raoult’s Law. This can be used with Dalton’s Law of partial pressure,
This implies that the vapor pressure of both benzoic acid and camphor are significantly greater than the vapor pressure of tert-butanol. In trial 4 there were less moles of camphor present than in either trial of benzoic acid, yet it had a similar effect on the freezing point of tert-butanol (Figure 3). This supports that camphor has a much higher vapor pressure than both tert-butanol and Benzoic acid. When benzoic acid was added to the solution in trial 3 in greater amount than trial 2, the temperature change was greater, further supporting that benzoic acid has a higher vapor pressure than tert-butanol. This is supported by the data, the experimental groups all reached greater temperatures, and remained liquids at lower temperatures (Figure 3). The accuracy of that recorded data may have been impacted by human error. The actual freezing points of the solutions were difficult to determine accurately due to the equipment used, although the trends overall trends of the experiment were still visible. The method of temperature measurement may have affected the outcome of the experiment. The temperature attachment for the Lab Quest 2 system was held in the test tube by hand, and likely came into contact with the test tube the solution was in. The test tube likely
The purpose of the experiment was to use the method of simple distillation to separate hexane, heptane, and a mixture of the two compounds into three different samples. After separation, gas chromatography determined the proportions of the two volatile compounds in a given sample.
Start by measuring 5.00 mL of commercial bleach in a 100 mL volumetric flask. The bleach was then diluted with distilled water until the contents reached the neck of the flask. Two grams of Potassium Iodide was then weighed out. Then, 25 mL of the diluted bleach solution was transferred into an E. flask by pipet. After that, the Potassium Iodide and 25 mL of deionized water was added to the E. Flash. The content of the flask were then swirled in order to properly dissolve the solid Potassium Iodide. The experiment was then moved to the fume hood, where 2 mL of 3 molar hydrochloric add were added to the E. Flask. The flask was then swirled for 2 minutes in the fume hood to ensure that no chlorine gas was produced by accident. The buret was filled
To investigate the relationship between three different alkanols in terms of their carbon chain length, rate of increased temperature, and heat of combustion, in order to determine which is the most efficient at heating water to a certain temperature whilst reducing time and effects on the environment.
Eugenol was extracted from cloves through the process called steam distillation. A total of 50ml of distillate were collected with temperature monitoring for every 5.0ml of collected liquid. The distillation curve showed that the temperature of volatilization of eugenol is from 98°C to 99°C which is way below its boiling point at 2540C. Chemically active extraction was conducted in order to remove impurities particularly eugenol acetate and caryophyllene. This involves the addition of several solvents particularly hexane, NaOH, HCl, then hexane again in succession.
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.