Fractional Distillation Lab

14 mL of 9 M H2SO4 was added to the separatory funnel and the mixture was shaken. The layers were given a small amount of time to separate. The remaining n-butyl alcohol was extracted by the H2SO4 solution therefore, there was only one organic top layer. The lower aqueous layer was drained and discarded. 14 mL of H2O was added to the separatory funnel. A stopper was placed on the separatory funnel and it was shaken while being vented occasionally. The layers separated and the lower layer which contained the n-butyl bromide was drained into a smaller beaker. The aqueous layer was then discarded after ensuring that the correct layer had been saved by completing the "water drop test" (adding a drop of water to the drained liquid and if the water dissolves, it confirms that it is an aqueous layer). The alkyl halide was then returned to the separatory funnel. 14 mL of saturated aqeous sodium bicarbonate was added a little at a time while the separatory funnel was being swirled. A stopper was placed on the funnel and it was shaken for 1 minute while being vented frequently to relieve any pressure that was being produced. The lower alkyl halide layer was drained into a dry Erlenmeyer flask and 1.0 g of anhydrous calcium chloride was added to dry the solution. A stopper was placed on the Erlenmeyer flask and the contents were swirled until the liquid was clear. For the distillation

Whereas for simple distillation, the compounds need to be around 80C apart in order for proper separation to occur. Thus, cyclohexane and toluene were not able to be properly separated since the boiling point for cyclohexane was 80.74C while the boiling point of toluene was 110.6C—there two boiling points are fairly close to one another. Thus, the mole fraction for cyclohexane and toluene were fairly low when compared to cyclohexane and

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

Objective: The main goal of this lab is to learn how separation of binary liquid mixtures is performed. Especially when the two liquids have boiling points varying by about 30° C. Hexane can be separated from toluene in this experiment because of the difference in their boiling points. Since toluene has a higher boiling point, it will left at the bottom while the hexane starts to boil out and collect in the Hickman still. GC measurements help us in determining how accurate our data is by making a graph of the amount of hexane and toluene in each fraction. Also this lab gives experience with semi-micro

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.

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 boiling range of the 1-pentyl ethanoate distillate was approximately between 149-151°C. This was indicated by the formation of the distillate and when the mixture of the purified 1-pentyl ethanoate started to vigorously

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 the experiment was to produce ethanol through fermentation and determine the maximum concentration of the ethanol product through fractional distillation.

Before the concentration profile of the distillation column could be calculated, the column had be heated to the point of equilibrium. After being heated for forty-five minutes, the binary mixture began boiling, and the equilibrium status of the column was monitored by taking temperature measurements of the mixture from the 8th tray every five minutes. The data collected is located below is Table 1.

The main purpose of this lab was to discover the proof of alcohol in the given unknown solution. The proof of alcohol in a solution is double its volume percent. Therefore if a bottle of grey goose vodka is 80 proof then its liquid solution has a volume of 40% alcohol. To find the proof in this experiment many steps were taken to separate the ethanol from the solution. Since ethanol is c in water it needs to be separated by adding diethyl ether and sodium acetate to cause a chemical reaction. The chemical reaction results in separation of ethanol form water. Since the ethanol and water is chemically separated the ethanol floats on top of the water, which allows them to be easily extracted separately using a separatory

The purpose of this experiment is to identify three unknown compounds and separating the three by distillation. The experiment is broken into two parts in identifying two mixtures, neat liquid and a binary mixture. The binary mixture contains a low boiler and high boiler. Distillation is used in chemistry as a method of separating and purifying organic compounds. The idea of distillation is to heat the compound and to boil the liquid until the impurities has disappeared. The aim of this process is to distilled the liquids at their highest level of boiling points. The starting range of all three unknown’s boiling points is no less than 100 C, this indicates that the compound that is distilling has started to heat up.

The liquid unknown can be purified through the technique of simple distillation. Simple distillation is used to purify a compound that is almost pure already. It takes advantage of the fact that liquids have varying boiling points, and in this lab can be used to evaporate off the organic solvent (which has a very low boiling point) that was still in the organic layer with the neutral component, leaving the neutral component by itself. In simple distillation vapor rises from the distillation flask and comes into contact with a thermometer that records its temperature and gives a starting point for the liquids boiling point range. The vapor passes through a condenser, which turns it back into a liquid and it is collected in the receiving flask. To see a diagram of a simple distillation apparatus set up see the figure below:

Distillation is the process of separating components from a liquid mixture by selective evaporation and condensation, utilizing the different volatility of each substance (Wikipedia, Distillation, 2015). It can result in complete separation or partial separation (which increases the concentration of selected components) (Massachusetts, University of, 2015). The two types that were examined in this lab was simple distillation and fractional distillation. Raoult’s Law also plays an important factor in distillation. It states that the partial vapor pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component multiplied by its mole fraction in the mixture (Perrot, 1994).

Steam Distillation is the process of distilling a mixture wherein one of the immiscible phases is a steam. It is a mild method for separating and purifying volatile liquid or solid organic compounds that are immiscible or insoluble in water. This technique is not applicable to substances that react with water, decompose on prolonged contact with steam or hot water, or have a vapor pressure of less than about 5 torr at 100°C.