Cyclohexane Lab Report

The serial 2-fold dilution were done with a volumetric pipette, its pump, and 10 mL volumetric flasks. Eight different solutions were produced, half of which came from Red 40 and the other half, from Blue 1. These different concentrated solutions were placed in a 10 mL volumetric flask, each labelled with either R for Red 40

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.

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 distillations were used to predict the accuracy of the distillation by comparing them to one other. The most accurate of the three distillations is the miniscale fractional packed distillation because this type uses a Vigreux column instead

In this experiment, Analysis of Gaseous Products, a comparison between the elimination reactions created in the presence of an acidic and basic conditions was observed to be further analyzed through gas-liquid chromatography. These conditions were achieved by acid-catalyzed dehydration of a secondary and primary alcohol and based-induced dehydration of a secondary and primary bromide. As a result of these changing eliminations, gas-liquid chromatography makes it possible to separate and isolate volatile organic compounds to analyze the stereochemistry and regiochemistry of these compounds without decomposing them. Overall, gas-liquid chromatography of these compounds in acidic or basic conditions contributed in the identification and analysis

Abstract: 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 from 66°C to 70°C the temperature then dropped and the rose to 98°C and the second fraction was collected from 98°C - 100°C. The first fraction is mostly hexane because toluene has a higher boiling point than hexane and the lower temperature

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 the set-up of these distillations is that fractional distillation apparatus included a fractioning column and copper coils. In addition, the first .5 mL of distillate collected in each distillation was run under a GC. As seen in GC analysis of the distillate collected via fractional distillation in figure 1 , the GC detected acetone, hexane, and toluene with retention rates of .602, .673, and .875 min respectively. This was similar to figure 2 using simple distillation. The retention rates of acetone, hexane, and tuolene were .602, .676, and .882 min respectively. Since hexane had a lower retention time than toluene, this means it eluted quicker. Moreover, the GC analysis provided the

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 was not supported by the employed methods.

The area under each peak allows the calculation of the quantity of the referred component. As expected from gas chromatography analysis, two peaks were seen demonstrating that here are two components in the mixture. Using the fraction #1, the first and biggest peak represents the isopropyl and the smallest represents toluene. This demonstrates that, as expected, the first collection was mainly composed by isopropyl because isopropyl has less boiling point (Table #1). On the contrary, for the last (third) collection GC analysis, the smallest peak represents isopropyl and the highest peak represents toluene. That happened because, since the majority of isopropyl was collected in the first run, the remaining quantity of isopropyl was small while the toluene quantity was higher (see figure 4 or table 3). The experimental calculations also prove that the quantity of isopropyl diminishes from the first fraction to the last (Table

In an 8:2 hexane: ethyl acetate solvent system, the spots moved 0.5cm and 0.6cm. The co-spot and the spot from the standard had the same Rf value of 0.1277. The spot from the experimental oil had an Rf value of 0.106. Although the separation and the identity of the products were definite on the TLC plate; to improve the results, the solvent system could have been changed to 7:3 or 5:5 Hexane: Ethyl Acetate. Adding more Ethyl Acetate to the system should have provided more separation and the spots should have moved up the plate

The distillation was carried out at a reflux ratio of 2 for the duration of this lab. The data collected was used to solve the design problem which uses a binary distillation system with a reflux ratio of 2. At steady state the compositions in the liquid phase of each component in the reboiler, the six trays, and the distillate were measured with gas chromatography. The composition of the components is related to the area under the curve that the gas chromatographer produces. Composition was used to determine tray efficiency by comparing the results with what was to be

The fractions in the fractional distillation such as N-hexane, isohexane, methyl cyclopentane have normal boiling point close to cyclohexane which makes the recovery of cyclohexane uneconomic and difficult.

Based on the graph, DCM was collected from 4 ml to 22 ml, thus 18 ml of DCM was collected. Cyclohexane was collected from 26 ml to 35 ml, thus 9 ml of cyclohexane was collected. Therefore the observed ratio of DCM to cyclohexane was 18:9 or 2:1.

A gas chromatograph (GC) can be utilized to analyze the contents of a sample quantitatively or in certain circumstances also qualitatively. In the case of preparative chromatography, a pure compound can be extracted from a mixture. The principle of gas chromatography can be explained as following: A micro syringe is used to inject a known volume of vaporous or liquid analyte into the head or entrance of a column whereby a stream of an inert gas acts a carrier (mobile phase). The column acts as a separator of individual or chemically similar components. A column is typically packed with a stationary non-volatile matter (stationary phase). The separation occurs due to different interactions of each component with the stationary phase.

Stock solutions of either VAL or SAC 1000 µg/mL were prepared in HPLC-grade methanol. The solutions were stored in refrigerator at

Fractional distillation column is a fractionating column used for separating a mixture into its various