Toluene Essays

The Citric Acid Cycle/ Kerbs Cycle/ TCA The Citric acid cycle is important as anaerobic glycolysis can only harvest a fraction of the energy from glucose. In the citric acid cycle there is aerobic respiration of pyruvate from step ten in glycolysis to C02 and H2O. This oxidation of pyruvate can greater a higher yield of ATP. The citric acid cycle occurs in the mitochondria where ten ATP is produced. The main purpose of the citric acid cycle is to harvest electrons from the citric acid cycle and

The two solvents in the unknown were correctly identified as acetone and toluene. The solvent with the lower boiling point was predicted to be acetone, as its boiling point was observed to be around 59 C, which was closest to the 56.5 C, the ideal boiling point of acetone. This result, however, had the possibility of being incorrect, since the boiling point of methanol, 64.7 C, was relatively close enough to the observed 59 C that methanol could have been incorrectly identified due to experimental

The purpose of this experiment was to separate a mixture of 1:1 isopropyl acetate and toluene by a method of fractional distillation by collecting the initial fractions from Hickman still and then redistilling them. Distillation process is a process in which a mixture composed of two liquid substances with different boiling points where the substance more volatile and with less boiling point distillate first. For this experiment, the isopropyl will evaporates first because it has the least boiling

The purpose of this lab was to separate hexane and toluene from a mixture by collecting fractions of both hexane and toluene through simple distillation. Because hexane and toluene have different boiling points they distill at different times and can be separated easily. We found the refractive index by putting our collected fractions in a refractometer. Once we knew the refractive index we could figure out the percentage of both hexane and toluene in the solution. The first fraction was collected

The purpose of this experiment was to use simple and fractional distillation to separate a mixture of hexane and toluene. In this experiment, the mixture of hexane and toluene in a bottom flask was heated with a boiling chip. Heating the mixture cause it to form vapor, and the condensation of vapor was collected as distillate. The temperature was recorded for every .5 mL collected in each set up and was later plotted to compare the difference between each distillation. The main difference between

high-pressure liquid). Data Table Compound: Toluene Mesitylene Structure: Boiling Point (oC): 110.6 164.8 Molecular Weight (g/mol): 92.141 120.1 Density (g/mL): 0.87 0.86 Sample Weights (mg): 49.7 949 Discussion The resulting sample weights displayed in the above data table show that a significantly greater amount of mesitylene was collected compared to toluene. Since a larger amount was taken, the mesitylene sample was likely not as pure as the toluene sample. In order to determine the identity

Instructor: Dr. Beatrix Aukszi LA: Paige Swalley 09/23/2014 Abstract: The purpose of this experiment was to fractionally distill a hexane/toluene mixture and to analyze the fractions. It is hypothesized that the first fraction will contain only hexane, the second a mixture of both, and the third just toluene. In order to separate the toluene and the hexane a Hickman still set-up was used. Once the mixture was distilled into the three fractions an IR machine analyzed the results. The hypothesis

Feras Kaid Chem 2415-43 TA: Rio Assessment 1 Conclusion In this lab, there were 4 different distillations that were performed each with the same end goal to separate the two different organic compounds, cyclohexane and toluene. We used the boiling points of the two compounds to separate them using the following 4 techniques: microscale simple distillation, miniscale simple distillation, miniscale fractional packed distillation, and miniscale fractional unpacked distillation. The three different miniscale

measure for each of the pure liquids (toluene and cyclohexane). After that prepare 9 mixtures of toluene and cyclohexane carrying their volume fractions from 10 to 90 percent in increments of 10 percent using 10.0 mL volumetric flasks. The last step is to read the temperature in the thermometer. Then, determine the the boiling point for toluene and for cyclohexane. Finally, complete the part C: for this part, the composition of vapor and liquid phases of toluene-cyclohexane mixtures. From the done

different types of hydrogens, including primary, secondary, tertiary aromatic, aliphatic, and benzylic hydrogens, were analyzed. The experiment was conducted twice, simultaneously. One set of test tubes containing bromine, dichloromethane, and one of toluene, ethylbenzene, tert-butylbenzene, cyclohexane, methylcyclohexane, or more dichloromethane (control), were exposed to UV light; the other equal set of test tubes were placed in a fume hood with the light off. This set of test tubes was not fully in

This experiment was started to measure the height equivalent of a HETP column to calculate twenty theoretical plates. The company need this information to separate the cyclohexane from the toluene. The separation was accomplished by the use of fractional distillation and gas chromatography. The process yielded one plate for the17.6cm column meaning, that the porcelain beryl saddles as a packing material are ineffective. Although the results were found to be inefficient this may have been due to

conjugated diene and a substituted alkene, also known as a dienophile, was used in the experiment. The purpose was to synthesize a substituted cyclohexene derivate by the reaction between the diene and dienophile, and it reacted in a reflux solution with toluene as the solvent forming an unsaturated six-membered ring. First, approximately 54 mg each of both compounds, tetraphenylcyclopentadienone (TPCPD) and diphenylacetylene (DPA), were placed in a reaction tube to be mixed and heated on a sand bath for

Introduction Toluene, according to the International Union of Pure and Applied Chemistry system (IUPAC) – methylbenzene, is most commonly used to synthesize benzoic acid. The importance of benzoic acid in modern world is due to its uses: the acid and its salts are used as preservatives in food: benzoic acid is globally known as E210 and sodium benzoate as E211. The benzoic acid and its precursors are also used in pharmacy and hygiene products : the shampoo and shower gel that I am using all contain

with ethyl acetate, hexane, toluene, DCM as solvent to separate a mixture. The stock solution is a mixture of benzophenone, biphenyl, and diphenyl methanol. The last trial include the comparison with the standard using the best solvent. It was predicted that toluene and hexane were the best solvent to elute a nonpolar mixture. Since the stationary phase is a silica gel that is polar, the solvent has to be nonpolar in order avoid the like to like interaction. Toluene and hexane were selected for

Aim The purpose of this experiment was to use fractional distillation technique to separate cyclohexane and toluene. Background Information Distillation is a technique which is used for separating two or more volatile products based on differences in their boiling points. Distillation can be used to separate a volatile solvent from a non-volatile product and separate a volatile product from non-volatile impurities. Simple distillation consists of a round-bottom flask, a distilling head, a condenser

chromatography. Furthermore, I hypothesized that cyclohexane and p-xylene distill better than cyclohexane and toluene since cyclohexane and p-xylene have a larger boiling point difference than cyclohexane and toluene. The boiling point of cyclohexane is 80.74C while the boiling point for p-xylene is 138.23C and the boiling point for toluene is 110.6, thus

data and printed gas chromatography data. Discussion The purpose of this experiment was to identify two unknowns and their ratios in a given mixture. The identities of the unknowns were two of either acetone, methanol, hexane, cyclohexane, heptane, toluene, or ethyl benzene. Distillation Distillation is used to remove impurities from a mixture – one component of which must be a liquid. Boiling points are utilized in determining the identity of the unknowns. Types of distillation include

Fractional distillation was performed in this lab to separate a mixture of two miscible liquids with a difference in boiling points of less than 40 C, and to predict their identities. After that, gas chromatography was used to confirm the identities of the two liquids in the unknown solution, and to obtain the ratio of the composition of the solution with respect to these two liquids. Distillation is a separation technique that relies on two substances having different boiling points, so that one

(VOCs) was investigated. Pyrrole reagent will be immobilized onto the PVC film which functioning as a matrix that can hold the reagent in solid manner. This sensor system is then tested to determine volatile organic compounds (VOCs) such as benzene, toluene, ethylbenzene and xylene (BTEX). The analytes and the reagent will react to each other so that the sensing system can be characterized. In these studies, there are some parameters have to be observed; spectral features, reaction response, limit of

(ionic, molecular, macromolecular and metallic) has its own set of properties, by testing these properties and finding them out for each chemical, it was possible to classify them. The properties tested during this experiment were solubility in water, toluene, and ethanol and the electrical resistance for those soluble in water. The melting point was tested for the two unknown chemicals. II. MATERIALS AND PROCEDURES List of chemicals used: Sodium nitrate,