Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Gas chromatography research paper
Gas chromatography conclusion
Gas chromatography research paper
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Gas chromatography research paper
Gas chromatography is a technique by which mixtures of volatile substances can be separated. Mass spectroscopy is a technique that analyses the mass of volatile molecules and their fragments. By using both techniques together, separated compounds are detected by their mass fragments. In this experiment, the CSUDH Chemistry Department Agilent 6890 N Gas Chromatograph, interfaced with an Agilent 5975B XL Mass Selective Detector was used. With this GC-MS machine, a mixture of compounds can be separated and detected by analyzing the mass spectrum data. This process is possible because several compounds have different chemical and physical properties; therefore, some compounds can linger in the column for different times. These properties include: …show more content…
This experiment consists of two parts: calibration and assay. For the calibration working standards of methyl paraben were created from stock solutions. The calibration data is used to determine the concentration of analyte in the sample. Since this experiment is qualitative and quantitative analyses of methyl paraben, in the qualitative analysis methyl paraben and propyl paraben are identified from their molar masses using the mass spectrum. In the quantitative analysis of methyl paraben, both methyl and propyl paraben are identified by using the retention time from the chromatogram. There are two parts for the quantitative analysis. In the first part, propyl paraben is added to a sample of methyl paraben as the internal standard and the relative response factor is calculated from the peak areas and the concentration data. In the second part, serial dilutions from five standard solutions of methyl paraben are performed. The absorbance of each standard solution is measured and a absorbance vs. concentration graph is plotted. The linear equation of the graph is obtained to calculate the concentration of an unknown solution. Both parts of quantitative analysis are paired for the t-test
Fire and thermal properties of PA 66 resin treated with poly-N- aniline- phenyl phosphamide as a flame retardant
The IR spectrum RM-02-CC2 was obtained. The spectrum consisted of a carbonyl peak, an aromatic carbon-carbon double bond peak, and a sp2 hybridized carbon and hydrogen bond peak at 1713, 1598, and 734. These functional groups are all present in 9-flourenone. The carbonyl group specifically was important because fluorenone was the only that contained a carbonyl group. The Identity was further confirmed by the melting point, 79-80˚C. This value is similar to the known value 84˚C2. The melting point observed during the experiment is greater than the known because the sample is slightly impure. This impurity is caused by presence of fluorene on the tip of the columns. As stated before, the tip of the column needs to be manage to ensure pure products. The presence of fluorene would increase the temperature as seen in the melting point results because the melting point of this compound is greater than fluorenone. Overall, both compounds were separated with column chromatography and presented reasonable yields for both products. Column chromatography is a useful technique to separate mixtures with both large and small quantities. Unlike TLC, column chromatography and be used for large amounts of
For this solution, 5 mL of the solution with 2.5 mL of AMV was placed in the cuvette. The cuvette was placed inside of spectrophotometer and the amount of absorbance was recorded. This procedure that involves a solution with a known concentration was repeated for the concentrations:1.0x10-4 M,5.0x10-5 M,2.0x10-5M, and1.0x10-5M.A unknown solution absorbance was measured by putting 5 mL of unknown solution with 2.5 mL AMV in a cuvette. The cuvette was placed in the spectrophotometer and the amount of absorbance was recorded. The procedure that deals with the unknown solution was repeated 2 more times with the same solution and the same amount of solution and AMV.
As shown in figure 2, the percentage of each isomeric alcohol in the mixture had been determined. The hydrogen atom on the carbon atom with the hydroxyl group appear at around 4.0 ppm for borneol and 3.6 ppm for isoborneol. The product ratio has been determined by integrating the peaks. A ratio of 6:1 for the Isoborneol/borneol ratio was expected and is validated by the calculations shown above, with isoborneol percentage at 83.82% and 16.17% of borneol. A CHCl3 group noted at around 7ppm and a CH2Cl2 at around 3.5ppm.
...s the change in the temperature of both of these batches, 6°C for the pure, and 13°C for the crude. In this final sub-section of the Characterization of Aspirin, the values of absorbance were recorded. Initially, 0.0566 grams and 0.0590 grams of pure and crude Aspirin respectively were obtained and each individually placed into beakers (400 milliliter) and had 250.0 milliliters of distilled water added to them. From each beaker, a tiny amount of the just dissolved solutions was transferred to a cuvette, one cuvette for each type of aspirin. Each cuvette was placed into the ultraviolent spectroscopy mechanism which was connected to a computer and absorbance spectrum values were obtained at 298 nm (Figure 5) (0.1987 pure aspirin, and 0.9549 crude aspirin).
For this statistical inference, the question was whether the means were truly different or could they have been samples from the same population. To do draw a conclusion, we must first assume normal distribution. We must also set the null hypothesis to m1 - m2 = 0. And per this assignment we must set the a-level at .05 and the hypothesis alternative to m1 - m2 ¹ 0; thus requiring a two-tailed test.
...bromebutane. Unfortunately, our group was only able to obtain the chromatograph for 2-bromobutane and the rest of the three chromatographs were provided by our T.A. Some possible reasons why the chromatographs for 2-butanol, 1-butanol, and 1-bromobutane were unable to be displayed properly is due to the malfunction of the syringes. If the syringe is not air-tight, the gaseous products can escape before being inserted into the injection port. In addition, the collection tube may have had a minor gas escape from the rubber septum, resulting in less concentrated gaseous products being inserted into the injection port. A possible solution is sealing the collection tube with parafilm. All in all, the provided data chromatographs and the rendered chromatograph by the 2-bromobutane in the lab session did match the expected results for the distribution of gaseous products.
The spots moved 3.8cm, 2.3cm, 2.1cm, 1.8cm, and 2.5 cm, for the methyl benzoate, crude product, mother liquor, recrystallized product, and isomeric mixture, respectively. The Rf values were determined to be.475,.2875,.2625,.225, and.3125, for the methyl benzoate, crude product, mother liquor, recrystallized product, and isomeric mixture, respectively. Electron releasing groups (ERG) activate electrophilic substitution, and make the ortho and para positions negative, and are called ortho para directors. In these reactions, the ortho and para products will be created in a much greater abundance. Electron Withdrawing groups (EWG) make the ortho and para positions positive.
The same procedure was done using 10ml of CV and 20ml of sodium hydroxide, both separately diluted to 50ml and added in a large beaker. The absorbance was recorded. In the last trial, 10ml of CV, 10ml of NaOH were diluted to 50ml. Before adding the two mixtures, 1ml of soap was added to the NaOH solution and then poured into a large beaker, along with the CV. Absorbance was recorded and the materials
One of the best methods for determining mass in chemistry is gravimetric analysis (Lab Handout). It is essentially using the the mass of the product to figure out the original mass that we are looking for. Thus the purpose of our experiment was to compare the final mass in our reaction to the initial mass and determine the change in mass.
Abstract: The goal of this experiment was to determine the amount of hydrogen gas that was produced when one started with a certain amount of mols of hydrogen. In fact, the reactants of the experiment were Magnesium and hydrochloric acid, while the products were Magnesium Chloride and Hydrogen gas. In a flask, the correct amount of hydrochloric acid acid was combined with Magnesium metal, and the resulting gas followed a path through a rubber tubing which connected to a gas measuring tube allowing the amount of H2 gas to be observed and recorded. This collection of data allowed for the ability to recognize the relationship between mols and volume. It was observed that for the most part, as the number of moles increased, so did the volume
By doing this experiment, I can know the physical and chemical properties of these samples. After I get my results about the physical and chemical properties of these samples, I can compare my results with the information given by the past student and identify the 5 unknown samples, finding out which sample is which substance. Hypothesis = ==
After washing it out, and driving off any remaining pet ether with a water bath and reaching a constant mass, the purified product had a mass of 0.272grams. A second TLC was ran to determine if the product was now pure. The plate was found to have two spots for the pure product, benzhydrol and biphenyl with Rf values of 0.67 and 0.15 respectively. It expected to see only one spot if the product was pure, so by TLC it was able to be determined there was not purification of the benzhydrol product. The pure product had a 73.1% yield, but this does not accurately reflect the yield as there were still impurities in the pure
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.