Chem 2203 Sec 026 27/September/2013 Experiment 3B: Fractional Semi-microscale Distillation Separation of Hexane and Toluene. 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 …show more content…
For instance hexanes’ boiling occurs at a lower heat setting so that is why in the first fraction we can view a greater peak of hexanes than toluene. In the third fraction we notice that toluene is found in higher abundances there. This helps when trying to distill out or separate the two compounds. b. Are the GC data consistent with your expectations? The GC data is what is expected, however there were some difference noticed with it than expected. For instance, the first fraction came out with more toluene that was originally expected and the graph showed this. Small unexpected material like this was the only thing not expected with the GC data. 4. Most of you did not have enough time to complete the redistillations of Fraction 1 and Fraction 3, but you are still equipped to anticipate the results. a. For the redistillation of Fraction 1, predict how the gas chromatogram for the initial fraction would have differed from the gas chromatogram of Fraction 1 from Distillation 1. The peaks would be more pronounced and there would be a greater variance in the size of the peaks. Peak 1 would be much higher and steeper and peak 3 or the toluene peak would be found much smaller. b. Similarly, for the redistillation of Fraction 3, predict how the gas chromatogram for the final fraction would have differed from the gas chromatogram of Fraction 3 from Distillation 1. b.i. The difference between
2. Write a statement to explain the molecular composition of the unknown solution based on the results obtained during testing with the Biuret solution and each sample solution.
Perform the following with three 0.05g samples of unknown and the following solvents: methanol, water and toluene
Me and my lab partner, obtained a mixture of a un known proportion from the instructor and then flow the guide line in our lab manual to separate the mixture by applying the separation method motioned in our lab manual pages 33-40 . In this experiment, the separation methods were decantation,
There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated, and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the components of the
6. Restate your predictions that were correct and give the data from your experiment that supports them. Restate your predictions
8.When the reaction is completed, record the volume of gas in the graduated cylinder. Record observations about which reactant was the limiting reactant.
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.
b. As I mentioned above that I spilled some of the benzoic acid therefore the initial mass
3. The spectrophotometer was set at 420nm. Distilled water was also used as the ‘blank’.
1.) Briefly explain the concept of steam distillation. What is the difference between a simple distillation and a steam distillation? When a mixture of two immiscible liquids are distilled it is referred to as codistillation. This process is referred to as steam distillation when one of the liquids is water. This distillation is used to separate organic liquids from natural products and reaction mixtures in which the final product results in high boiling residues such as tars, inorganic salts, and other relatively involatile components. It is useful in isolating volatile oils from various parts of plants and not useful in the final purification of a
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
5. Restate your predictions that were correct and give the data from your experiment that supports them. Restate your predictions
Draw a labelled diagram of a laboratory set-up that can be used for carrying out the process and collecting the gaseous product.