Pentadecane And Dodecane Binary Mixtures

An automatic pipet was used to measure 0.450 mL water and 0.165 mL acetic anhydride and was added to the conical vial. A spin vane was placed into the vial and an air condenser was attached.

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

Data and observations: Substance(s) Trail 1 Trail 2 Trail 3 Penny with soap 3 drops 2 drops 3 drops Penny with water 9 drops 11 drops 8 drops Penny with soap and water together 5 drops 4 drops 5

In the third stage of this experiment, the density of a liquid was determined and compared to known standards. A 100ml beaker was filled to about half-full with room-temperature distilled water. The temperature of the water in ◦C was recorded in order to compare to known standards later. A 50ml beaker was then weighed on a scale in order to determine mass and recorded. A sample of the distilled water with an exact volume of 10ml was then placed in the 50ml beaker using a volumetric pipette. The 50ml beaker with the 10ml of water was then weighed again and the initial mass of the beaker was subtracted from this mass to obtain the mass of the 10ml of water. With the volume and the mass of the water now known, density was calculated using d = m/V and recorded in g/ml. This process was then repeated to check for precision and compared to standard values to check for accuracy. Standard values were obtained from CRC Handbook, 88th Ed.

With time (t) on the x-axis and temperature (Celsius) on the y-axis, the exponential change could be easily observed. At the beginning of the laboratory the masses of the combined polypropylene test tube and 100 mL beaker were recorded by a digital electronic scale. A dry polypropylene test tube was obtained and approximately 2 mL of p-xylene was squirted into it with the use of a pipette. This was added to the beaker and weighed. 10 drops of toluene was then added and weighed again. The polypropylene test tube, which now contained 10 mL of p-xylene and 10 drops toluene was removed from the beaker and placed into a replica 100 mL beaker which was halfway filled with an ice water mixture. The temperature sensor, which was connected to the microlab application was placed inside of the polypropylene test tube and stirred rapidly around the outskirts of the bottom of the polypropylene test tube. The mixture began freezing, giving off an icy slush complex. Once the temperature appeared to have reached the nucleation point and leveled out at its freezing point, the application was stopped. This value was recorded in the laboratory manual. The temperature sensor was rinsed off then wiped, the beaker was re-filled with ice, and the test tube was put into the test tube rack to be thawed. Once thawed, this was discarded into the waste bin

The volume of a small test tube and a thin-stemmed pipet were determined in this section of the lab. Water was poured into a small test tube until the water reached the very top edge of the test tube. The test tube was then emptied into a plastic 25 mL graduated cylinder and volume was measured and recorded into data table 3. A think-stemmed pipet was completely filled with water. Drops were carefully counted and emptied into the empty plastic 25 mL graduated cylinder until the water level reached 1 mL. The number of drops in 1 mL was recorded into data table 3. The thin-stemmed pipet had a total volume of 4 mL and that was also recorded into data table 3.

The purpose of this experiment is to familiarize oneself with the general procedures determining a partition coefficient at the microscale level and learn in weighing milligram quantities of materials on an electronic balance, the use of automatic pipets, the use of transfer pipet, and the use of a vortex mixer. Also, to familiarize oneself with extraction

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.

Answer the following questions after completing the problems in Part III. You will also need to refer to the chart of Saturation Mixing Ratios in Figure 13-1; interpolate from the chart as needed. Assume that condensation begins at 100% relative humidity and that no evaporation takes place as the parcel descends.

The data collected during the experiment allowed an approximation or prediction of the diffusivity trend of both flow rates. It also correlated with the relationship between H2CO3, HCO3- and CO2. To conclude, essential process such as separation and purification of mixtures occur every day in the human body. This experiment allowed an insight about the complex processes organs like the

An experiment meant to measure the density of the white fog is set up using a 500ml round bottom flask with 2 openings and 200ml of a particular liquid. “A pellet of dry ice (9-10g) is dropped into the liquid through one opening, which is immediately sealed. The fog formed

When these droplets settle to the ground, usually they are spread over a wide area, minimizing their effect. (Environmental Impact of Aviation Operations, 2005)

The droplets in a microemulsion are in the range of 1 nm-100 nm in diameter. It is well established that dispersed particles having diameter less than one-fourth (1/4th) the wavelength of visible light, i.e. Less than approximately 120 nm, do not refract light and therefore microemulsion appear transparent to the eye [18]. The concept of microemulsion was introduced as early in the 1943 by hoar & Schulman. They generated clear single phase solution by titrating a milky emulsion with hexanol. Schulman et al. introduced the term microemulsion for this system in

The analyses of mixture were to distinguish and identify homogeneous mixture by using the techniques of decantation and sublimation. By performing these techniques, we examined our solutions such as SiO2 (sand), NH4Cl (ammonium chloride), and NaCl (sodium chloride) and mixed H2O (water) with each solution after being heated. After examining our solutions, we made calculations by finding the percent mass of each solution once the experiment was completed. In our findings, we were able to determine the mass of the determined and the percent recovery of matter. The outcome of the experiment was that we made the correct