Distillation Postlab

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Rutgers University *

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23772

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Chemistry

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Jan 9, 2024

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pdf

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Uploaded by karennshadyy

- Temperature the liquid mixture should have boiled at: 2 mL of Cyclohexane used. Mass (grams) = Volume (mL) * Density (g/mL) Mass = 2 mL x 0.779 g/mL Mass of 2 mL cyclohexane ≈ 1.558 grams Moles of cyclohexane = 1.558 g / 84.08 g/mol ≈ 0.01856 moles 2 mL of Toluene used. Mass (grams) = Volume (mL) * Density (g/mL) Mass = 2 mL x 0.867 g/mL Mass of 2 mL of Toluene ≈ 1.734 grams Moles of toluene = 1.734 g / 92.08 g/mol ≈ 0.01883 moles Total moles = 0.01856 moles cyclohexane + 0.01883 moles toluene = 0.03739 moles Mole ratio of cyclohexane = 0.01856 moles / 0.03739 moles ≈ 0.496 Mole ratio of toluene = 0.01883 moles / 0.03739 moles ≈ 0.504 Mole ratio of cyclohexane to toluene is 0.496 : 0.504. This is a mole ratio of approximately 1:1 which is a mole percent of 50 for both solvents to compare with on the boiling point composition graph on page 90. Theoretically, a mixture of 50:50 cyclohexane to toluene should have boiled at approximately 92 degrees celsius . - Theoretically, the temperature when the first drop of distillate condensed using vapor composition should have been at about 85 degrees celsius. - My graph of the simple and fractional distillation curves for cyclohexane and toluene seemed different than the original graph (Fig. 5.8. Page 90). The original graph had one common point of intersection that my graph didn’t. The simple distillation curve on my graph appeared more linear than the original graph. Some sources of error that could have caused this difference could be: 1. Loose connectors and adapters in the experiment’s set up 2. Airﬂow in the hood could have led to temperature variations 3. Heat lost to the environment if the microscale apparatus had a large surface area 4. Thermometer errors due to calibration or incorrect positioning of thermometer relative to the sidearm. 5. Poor recovery of liquid due to positioning of the sidearm 6. Distillate left adhering to the glass surface of the apparatus - For the mixture used in this experiment, the fractional distillation process would be more eﬃcient in separating the mixture. This is because for this mixture the composition was 50:50 and the boiling point difference was about 30 degrees

celsius. Both of these criteria match the criteria of fractional distillation which includes a substantial composition of more than 10% and a boiling point difference around 20-30 degrees or up to 75 degrees celsius. For simple distillation, on the other hand, the criteria would be a composition of 10% or less and a Boeing point difference of 75 degrees or more. Fraction distillation is more eﬃcient for this mixture. - This experiment led me to learn the techniques of distillation and to compare both simple and fractional distillation of a cyclohexane and toluene mixture. For this experiment, fractional distillation is more eﬃcient due to composition and boiling point differences. I was able to draw a graph of each distillation method and compare the temperatures at which the first drops were observed. This comparison led me to figure out the more effective distillation technique for this experiment.

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