Distillation Of Limonene Lab Report

The original 1.0 gram of the 50/50 mixture of the benzoic acid and benzil contain 0.5 gram of benzil. Thus, from 0.5 gram of benzil, only 0.266 gram of benzil was collected. The percent recovery of benzil was calculated to be 53.2%. This low percent recovery could be due to filtration errors. Some amount of benzil remained on the filtration paper that contained the MgSO4. In order for determining the purity of the

Experiment 55 consists of devising a separation and purification scheme for a three component mixture. The overall objective is to isolate in pure form two of the three compounds. This was done using extraction, solubility, crystallization and vacuum filtration. The experiment was carried out two times, both of which were successful.

There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated, and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the components of the

Abstract: One mixture of two unknown liquid compounds and one mixture of two unknown solid compounds were separated, isolated, purified, and characterized by boiling point. Two liquid unknowns were separated, isolated, and purified via simple distillation. Then, the process of an acid-base extraction and washing were used to separate two unknown compounds into two crude compounds: an organic acid and a neutral organic compound. Each crude compound was purified by recrystallization, resulting in a carboxylic acid (RCO2H) and a pure organic compound (RZ). The resulting mass of the pure carboxylic acid was 1.688g with a percent recovery of 31.80%, the boiling range was 244-245 °C, and its density was 2.0879g/mL. The resulting mass of the pure organic solid was 2.4902g with a percent recovery of 46.91%, the boiling range was 52.0-53.4°C, and its density was 1.5956 g/mL.

The objective of this extraction experiment was to achieve a comprehensive understanding, as well as master the practice, of the technique of separating various individual components of a compound.

The proof (twice the % alcohol) starts at its maximum and goes down (as the alcohol evaporates). If we start with a high concentration of alcohol, we will get the azeotrope (95% alcohol, 5% water) for a while, then the concentration will decrease.

The first TLC plate showed that the fractions collected during the experiment that appeared to be the purest were fractions 4 and 6. These two fractions and fractions number 5 were combined for the final product. The Rf values for the standard carvone, fraction 4, and fraction 6 were all 0.32 indicating that these compounds were

The purpose of this laboratory experiment was to isolate and characterize clove oil in order to understand how to isolate organic compounds with high boiling points, how to perform and interpret qualitative tests for organic compound functionality, and to continue to learn how to perform and interpret IR spectrometry. Steam distillation was used in order to prevent the organic compound from decomposing at temperatures approaching the compound's boiling point.

Name CHE 173 Sec # January 25, 2005 Experiment 36: Determination of the Structure of a Natural Product in Anise Oil

With the purpose of the experiment being to identify the 30 mL of unknown liquid, the theoretical basis of simple and fractional distillation must be deconstructed and applied to the data obtained describing the liquid in question.

Distillation is a method of separating two volatile chemicals on the basis of their differing boiling points. During this lab, students were given 30 mL of an unknown solution containing two colorless chemicals. Because the chemicals may have had a relatively close boiling point, we had to employ a fractional distillation over a simple distillation. By adding a fractionating column between the boiling flask and the condenser, we were able to separate the liquids more efficiently due to the fact that more volatile liquids tend to push towards the top of the fractionating column, thereby leaving the liquid with the lower boiling point towards the bottom. After obtaining the distillates, we utilized a gas chromatograph in order to analyze the volatile substances in the gas phase and determine their composition percentage of the initial solution. Overall, through this lab we were able to enhance our knowledge on the practical utilization of chemical theories, and thus also demonstrated technical fluency involving the equipment.

Before the start of the experiment, the theoretical yield was to be calculated. First, the limiting reagent was determined from the reagents by comparing the amount of moles. Among the three reagents involved in this experiment - camphor, sodium borohydride, and methanol, camphor was found to be the limiting reagent. The moles of camphor was less than the combined moles of the other two reagents. The theoretical yield, which is the amount of product that could be possibly produced after the completion of a reaction (“Calculating Theoretical and Percent Yield”), was found to be 0.25 g. Once the product was achieved, a percent yield of 97% was determined. As a result, the reduction of camphor to isoborneol was successful.

Eugenol (1-allyl-4-hydroxy-3-methoxybenzene) is a naturally occurring component of clove oil as well as cinnamon, basil and nutmeg oils (Pramod et al., 2010). Eugenol is a member of the allylbenzene class of chemical compounds. It is an allyl chain substituted guaiacol. Guaiacol is naturally occurring organic compound (Saravanakumar Jaganathan, 2012). It appears as a clear to pale yellow oily liquid, general soluble in organic solvents sparingly soluble in water. Eugenol is used as flavor, irritant, sensitizer and can produce local anesthesia. Now a day, eugenol can also be synthesized in laboratory scale and industrial scale by allylation of guaiacol with allyl chloride having the similar kind of functional property (Barceloux DG, 2008). In

The main objective of the lab work done was the extraction of eugenol from cloves, after which a calculation of the the percentage recovery of it is researched, and to the running of an IR in order to analyze the purity of the lab sample. Eugenol is the byproduct of the oil extract from cloves. This produced oil consists of mostly eugenol and acetyleugenol. In medical purposes, the oil could be used as a dental anesthetic. It is also one of the best over the counter cure for a toothache. (Kluger, 2016) Dentists use it as an antiseptic and anti-inflammatory weapon agains dental pain for patients, as well as to kill germs. Because some research shows that eugenol is a good weapon against bacteria and other harmful dental threats, Eugenol is often

For winter and spring baits it is interesting to note that a fair percentage of genuine vanilla flavour is produced from a clove oil called eugenol. Eugenol is a very successful element of many cold water and warm water baits and flavours and can be found in a range of other herbs and spices etc.