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Gas Chromatography Lab Report

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Gas chromatography is a helpful technique to separate and analyze volatile compounds. In this experiment, ethanol and pentanol are both nonpolar, so they are separated based on their boiling points. Ethanol has a higher boiling point than pentanol, so it elutes first and its peaks can be seen first on all the chromatograms (Figures 1, 2, 4, and 5). It is useful to be able to separate ethanol and determine its percentage, like in this experiment, in the case of alcohol concentration in beer. The purpose of the calibration plot of ethanol solutions made during Week 1 was to obtain a direct correlation between the percent ethanol in a sample and its average ethanol peak area (Figure 3). The R2 value of the graph was 0.9973, indicating that the data obtained during Week 1 was precise and accurate (Figure 3). The linear trendline from the calibration plot, y=0.0687x+0.1683, can be used to determine the unknown percent ethanol in the extraction sample (Figure 3). From the determination of the percent ethanol in the extraction sample, the partition coefficient can be calculated. …show more content…

If K had been less than one, then the aqueous layer would have contained the most ethanol. However, with a K value of 2.1, it was determined that the organic layer contained the most ethanol. From this information, it was concluded that the injections during Week 2 should come from the organic layer. It was only necessary to determine K in Week 1 because the partition coefficient is calculated after the solute has all been extracted, which happened in Week 1. Not all of the ethanol was extracted in Week 2 and the other ingredients in beer could have skewed the partition

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For this experiment, the pure products appear to be in the first and fifth fractions because these fractions had stabilizations of boiling points whereas the other fractions featured comparatively larger boiling point ranges. However, it is important to note that the second fraction had a significantly larger volume than the rest of the fractions did, and only a 4C temperature range reading. This suggests that there could have been some pure product in the second fraction as well, especially because the temperature range was increasing slowly until about 3 mL of distillate had been collected, and then it thermometer readings increased rapidly. The data for this experiment would have been more comprehensive if the after these 3 mL had been collected, a new fraction had been collected with the distillate from the more rapidly increasing temperature range reading had

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Analysis: In order to test the null hypothesis of this lab, it was first necessary to calculate the theoretical concentration of acetic acid in a bottle of vinegar because it can be used to compare with the results of the titration experiments in order to see whether or not the vinegar contains 5% acetic acid by mass. Therefore, the number of moles of acetic acid was calculated through the use of its density, its molar mass, and the total volume of the vinegar. Then its molarity was calculated using its number of moles and the volume of vinegar used in each trial.

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Introduction Your child has received a gastrostomy. A small opening was made through your child’s abdominal wall and into the stomach to insert a gastrostomy button, a device in which will allow your child to receive adequate nutrition. Typical feeding by mouth is sometimes disrupted by problems such as congenital abnormalities of the digestive system, sucking and swallowing disorders, and failure to thrive. A gastrostomy button will ensure that your child receives the proper nutrition needed to grow. Before you leave the hospital, the nurses will train you on how to use a gastrostomy button.

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Despite a slight deterioration in temperature between 12 milliliters and 13 milliliters of distillates collected, Figure 1 roughly resembles the reference fractional distillation plot.1 While the amount of distillates for Fraction 1 and Fraction 2 appears to be similar in the reference plot, Figure 1 displays a larger volume for Distillate 1 as compared to Distillate 3 in terms of relative length of periods at constant temperature. Additionally, the slope for Fraction 2 on the reference plot is very steep, but the slope for Distillate 2 varies from a similar slope to Distillate 1 that later becomes almost as steep as the reference slope. This is due to the fractional column not having enough theoretical plates to handle the separation, so the mixture distilled until all of the lower boiling point component, cyclohexane, was removed. The slope of Figure 1 between 13 milliliters to 16 milliliters of distillates collected is also flatter in comparisons with the

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Fractional Distillation and Gas Chromatography Post Lab Report Discussion: Distillation is a method of purification for volatile liquids that utilizes the boiling points of the liquids. The boiling point of a liquid is the temperature when the equilibrium vapor pressure, the amount of vapor pressure at a temperature that allows a liquid to be at dynamic equilibrium, equals the total pressure present in the system. The two most common types of distillation are simple distillation and fractional distillation. Simple distillation can be used for removing a substance from less volatile substances, where the distillate substance is left as residue after distillation, or can be used to separate two volatile compounds given that the difference between

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Conclusion The GC ethanol analysis method described above has a simple concept, its rapid, and extremely accurate, determining ethanol precisely without interference from other beverage components. With this method, it takes only 7 to 8 min to complete a sample analysis for the determination of ethanol content in a beverage sample. Analyst handling is minimized to prevent deviation in results or possible human error. This method requires a gas chromatograph and a digital integrator, both reasonably expensive and sophisticated pieces of equipment.

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