Using Fractional Distillation

According to the group data, which Mrs. Harmon went over to ensure groups received accurate data, the original solution had an inconstant boiling point which reached 2 plateaus (85°C and 100°C) before all the liquid evaporated, a medium odor like alcohol, was flammable, had a density of about 0.91g/100cm3, and did dissolve sugar. The 2 plateaus show that there were two substances in the original mixture, which have 2 different boiling points. These boiling points are the points that the substances can be separated. Based on the two boiling points and the odor, groups predicted the two substances were isopropanol and water. Fraction 1 had a boiling point of about 85°C, a strong odor like alcohol, was flammable, had a density of about 0.84g/100cm3, and did not dissolve sugar.

A glass jar was obtained and filled with 0.5 cm of the solvent consisting of hexane, ethanol, and ethylacetate. The lid was put on so it could become saturated with vapor.

Method: Distillation is based on the fact that the matter can exist in three phases - - solid, liquid and gas. As the temperature of a pure substance is increased, it passes through these phases, making a transition at a specific temperature from solid to liquid (melting point--mp) and then at a higher temperature from liquid to gas (boiling point--bp). Distillation involves evaporating a liquid into a gas phase, then condensing the gas back into a liquid and collecting the liquid in a clean receiver. Substances that have a higher boiling point than the desired material will not distill at the

Answer: The distillation apparatus consists of a round bottom flask connected through an adapter to a condenser, which is connected through another adapter to a second round bottom flask (Yee, n.d., Distillation). There is a thermometer connected through the thermometer adapter at the top (Yee, n.d., Distillation). There is also a vacuum adapter and a heating mantle. The heating mantle is a coil which heats through electrical resistance (Yee, n.d., Distillation). You use cold water and make sure that it goes in through the bottom and out through the top (Yee, n.d., Distillation).

Distillation of the first product began at 83 °C. A Pasteur pipette was used to remove 1-ml of the distillate into a vial. A second vial was filled with distillate until it reached 1-ml. As the second vial is being filled, observe the temperature and remove the apparatus from the heat source if there is an observed drop in temperature.

With the purpose of the experiment being to identify the 30 mL of unknown liquid, the theoretical basis of simple and fractional distillation must be deconstructed and applied to the data obtained describing the liquid in question.

The history of the Lagavulin Distillery is steeped in illegal activity and court room battles. Although officially (and legally) dating back to 1816, illegal distilling on the site can be dated back nearly 80 years earlier to 1742.

C. We can conclude that it allowed us to determine that anaerobic distillate, wine distillate and ethanol and water yielded a precipitate and that the ethanol was present. This shows that during ethanol fermentation of yeast, water and corn syrup distillate did not form precipitate, thus no ethanol present which demonstrated that distilled corn syrup and water do not allow for fermentation to take place while wine distillate and the ethanol and water combination does indeed produce

Distillation is a method of separating two volatile chemicals on the basis of their differing boiling points. During this lab, students were given 30 mL of an unknown solution containing two colorless chemicals. Because the chemicals may have had a relatively close boiling point, we had to employ a fractional distillation over a simple distillation. By adding a fractionating column between the boiling flask and the condenser, we were able to separate the liquids more efficiently due to the fact that more volatile liquids tend to push towards the top of the fractionating column, thereby leaving the liquid with the lower boiling point towards the bottom. After obtaining the distillates, we utilized a gas chromatograph in order to analyze the volatile substances in the gas phase and determine their composition percentage of the initial solution. Overall, through this lab we were able to enhance our knowledge on the practical utilization of chemical theories, and thus also demonstrated technical fluency involving the equipment.

The purpose of this experiment was to separate a two component mixture using fractional distillation. Distillation is a process of vaporization than condensation of a substance, used primarily to separate substances from a mixture when there are different boiling points. Fractional distillation is when the mixture has multiple substances with similar boiling points, and a fractional column is used to create multiple vaporization/condensation cycles. Fractional distillation is important when two or more substances need to be separated, but they have similar boiling points.

The purpose of this experiment is to identify an unknown substance by measuring the density and boiling point. I will be able to conclude which substance is my own from a list of known options stating what its real boiling point and density is.

A 10 mL round-bottom flask was weighed both before and after approximately 1.5 mL of the given alcohol, 4-methyl-2-pentanol, was added. 3 mL of glacial acetic acid, one boiling chip, and 2-3 drops of concentrated sulfuric acid were added to the flask in that order. The reflux apparatus was assembled, the

A mixture of the essential oils, eugenol and acetyleugenol, will be steam distilled from cloves. These compounds are isolated from aqueous distillate by extraction into dichloromethane. The dichloromethane solution is shaken with aqueous sodium hydroxide, which will react with eugenol, to yield the sodium salt of eugenol in the basic aqueous layer, and acetyleugenol in the organic layer. The basic aqueous layer can be acidified to re-extract eugenol from it. And the organic layer can be dried and concentrated to yield acetyleugenol The principle of steam distillation is based

The main objective of the distillation lab was to identify the composition of an unknown binary solution. The only known component is that the boiling point of the two components were at least 40˚C apart in boiling points. Due to the difference in boiling points, fractional distillation would be an easy way to determine the identity of each component of the binary solution. In the experiment, 30mL of the unknown binary solution was ran through the fractional distillation apparatus. As the solution boiled, gas from the unknown solution ran through the column, which had a temperature gradient to allow rapid and repeated distillations, and one of the components were isolated. By recording the temperature and amount of

As it reaches the distilling side arm, the temperature of the vapor is collected. The vapor pressure becomes strong enough that the vapor begins to travel down the condensing tube where it is converted back into liquid. This liquid should be distilled from any contaminants. This is capable because different molecules have different boiling points. For instance waters boiling point is roughly 100oC where as Methanol’s boiling point is 65.4oC therefore the Methanol will boil and evaporator first leaving only water in the boiling flask. Once the temperature of the vapor reaches 100oC no methanol should be left in the boiling flask and the water should now be the only vapor