Fractional Distillation Lab Report Essay

1. Our percent yield for alcohol was 84.2% which is average. We rushed through our vacuum filtration and probably did not let the solid dry long enough and might have not transferred all of the solid to the vacuum filtration from the beaker.

The experimental average Kf was calculated to be 4.29, which was pretty close to the actual value of 4.30. The identification of Unknown D was Pentane, and the actual compound was Pentane. However, for Unknowns A and C the experimental molar masses were off by 14 g each. The actual molar mass of ethanol is 46.07, where the experimental one was 160.36. That is mostly due to the hydrogen bonding between ethanol molecules, the strong hydrogen bonding interactions are responsible for the high freezing point, which lead to a higher molar mass.

The hypothesis stating if four grapes are placed in distilled water, a salt solution, a sugar solution, and tap water, then the grape placed in distilled water will gain the most mass out of the four grapes was rejected by the data. The grape placed in the distilled water gained the second smallest amount of mass in the experiment, 0.26 grams. The hypothesis stating if four grapes are placed in distilled water, a salt solution, a sugar solution, and tap water, then the grape placed in the salt solution will lose the most mass out of the four grapes was rejected by the data. The grape placed in the salt solution gained a mass of 0.22 grams. The grape placed in the salt solution gained 0.22 grams of mass, the grape placed in distilled gained 0.26 grams of mass, the grape placed in the sugar solution gained 0.55 grams

The purpose of this lab is to separate a mixture and determine the percentages of each of the ingredients. Each substance will have a different boiling point due to its intrinsic properties and from that, we will be able to determine the purity of different products as we evaporate off the next level of product.

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.

Introduction The Purpose of the experiment was broken into two parts both having to do with the purification and separation of different compounds and impurities. In part A was the distillation of cyclohexane and in part B it was about taking a 50:50 mixture of dichloromethane and cyclohexane and separating them through fractional distillation. Experimental Refer to Chemistry 2513 Lab Manual Introductory Organic Chemistry Part 1 Fall 2014. Look for this experiment between pages 21-24 Results Observations:

The memo summarizes the findings from the initial assessment performed on the 190 proof SDA-3AU alcohol for use in Fractionation and downstream processes.

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.

At the end of distillation it is possible to obtain an ester product with low purity. Low purity occurs as the result of excess water collected with the distillate. Thus, in order to increase purity, distillation should be undertaken with a great deal of

Overall, there was much to be learned from this experiment – even including the error that was seen throughout the experiment in our incorrect data points as we attempted to find the percent ethanol in Busch’s, Busch’s Light, and Busch’s nonalcoholic beers – of which we did not get close to in the slightest. The calibration method resulted in a number that made sense for the extraction sample of an original 5% in water solution, 3.46%. The week two experiment resulted in a large amount of error, meaning that the conclusions drawn were not accurate, even though theoretically the standard addition solution should have had more accurate results. The main problem set out to be solved is finding ethanol percent in solutions of which the ethanol

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 volume unit used was because it is equivalent to mL. Once the fermentation control run was completed, the fermentation vial was carefully washed and rinsed for part IV: changed environment fermentation

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

carried out in a batch reactor, where ethyl benzoate was added to a mixture of water, ethanol,