Tori TaylorPartner: Gabrielle TeneyucaCHEM 237:558Shelby OneyExperiment 5: Simple Distillation and Gas ChromatographyResults and DiscussionDuring lab, a simple distillation of heptane and octane was performed. This was done to separate and place the alkanes into three different liquid fractions. Temperature ranges were recorded, and each fraction was injected with a 2 µl sample of heptane to be analyzed with a gas chromatogram. Below are the noted values obtained from the chromatogram: FractionNumberTemperature Collected (C)Retention Time(Minutes)Area % PercentHeptaneArea %PercentOctane1 102.9-110.5 1.082-1.776 71.166 28.8342 110.5-114.0 1.133-1.804 61.963 38.0373 114.0-118.4118.4-119.51.187-1.765 41.036 58.9644 (residualfraction)119.5-122.9 1.214-1.680 20.176 79.824The simple distillation of hexane and octane was performed as well; this section of the lab was conducted by a different lab group and data was shared. Below are the results of Hexane and Octane: FractionNumberArea % PercentHexaneArea %PercentOctane1 95.026 4.9742 93.268 6.7323 43.654 56.3414 (residualfraction)3.286 96.714During the experiment there were a few events that occurred that may have altered our data. The first being, after each fraction was taken the content had to sit while waiting in line to perform a gas chromatogram. This may have altered the results because of the temperature changes. Another event that occurred was, instead of directly poring the leftover mixture into the 4th (residual fraction) vial, it was taken as another fraction just like the previous 3. This more than likely changed what the gas chromatogram was actually supposed to look like due to the fact that most of the heptane was gone so a smaller area percentage should have been shown of the heptane and a larger area percentage should have been shown of the octane. In conclusion, when reviewing the tables above, it is seen that as the area percentage of Heptane/Hexane decreases the area percentage of octane increases. This is because over time the Heptane/Hexane had already evaporated due to its lowermolecular weight over octane. This makes sense due to the fact that the lower the molecular weight of a compound the lower the boiling point should be. All in all, the results were mostly similar throughout the other lab groups. If this experiment was performed again, we could use a taller fractioning tower to get better results. The reason for more accurate results would be due to the more theoretical plates which would allow for more separation of the two organic