The overall basis of this experiment is to take two compounds, in this case toluene and hexane, distill both and observe a constant boiling point in order to later distill a more complex two component mixture which will provide the pure compound. The distillation process begins with heating a liquid to a boiling point, in this experiment that being hexane and toluene separately to start off, the liquid evaporates forming a vapor. A stir bar was provided in order to ensure that an even boiling of the liquid could happen and therefore produce a place where bubbles of vapor can form. We then recorded the temperatures after collecting different amount of Ml hexane distillate, the same steps repeated for toluene as well. The distillate is a purified
It was learned that changing the volume of the same substance will never change the boiling point of the substance. However having two different substances with the same volume will result in two different boiling points. The purpose of this lab was to determine if changing the volume of a substance will change the boiling point. This is useful to know in real life because if someone wanted to boil water to make pasta and did not know how much water to
Felder, M. Richard, Elementary Principles of Chemical Processes, 3rd ed.; Wiley: New Jersey, 2000; p 631.
The boiling point of a substance is “the temperature at which the total vapor pressure of the liquid is equal to the external pressure” (Gilbert & Martin 2011). Boiling point is the point at which the evaporation rate of a given liquid increases as bubbles are formed. The boiling point is usually determined by “reading the thermometer during a simple distillation” (Gilbert & Martin 2011). However for the purposes of this lab, a miniscale method was used to determine the boiling point. This method requires for a liquid to be heated using the apparatus seen in Figure 1. A thermometer is placed just above the liquid at a height where the thermometer is able to measure the vapor temperature of the liquid, not the liquid itself. As the liquid heats, the temperature rises until it reaches an equilibrium where it cannot increase any
The sources stated that water boils at 100°C, so this is what I was expecting when I started to boil the rest of my distilled water. After the water reached a steady boil, my thermometer first reached 102°C. This was a bit off, but I took my thermometer back out and let it reach room temperature again before doing the second trial. The second time my thermometer reached 100°C, which was exactly the right temperature. After repeating the experiment for the last time, I recorded 101°C. This averaged out to be 101°C.
To investigate the relationship between three different alkanols in terms of their carbon chain length, rate of increased temperature, and heat of combustion, in order to determine which is the most efficient at heating water to a certain temperature whilst reducing time and effects on the environment.
The mass of 2mL of the solvent, p-xylene, was measured as well as the mass of 10 drops of toluene, the solute. The temperature of the solution rose to the freezing point after supercooling, then continued to drop as the solution froze, versus stabilizing as the pure p-xylene did. The maximum temperature obtained after supercooling was recorded as the freezing point of the solution. This process was repeated three times, each with a new test tube and the same beaker and scale for measuring the masses, then the Tf was calculated for each trial, as well as the average Kf. For the final portion of the lab, the same procedure as above was followed with the substation of 10 drops of unknown solutes instead of toluene in the p-xylene. Each unknown, A, C, and D, had one trial each. With the experimentally gathered data, the molar masses were then computed and compared to the given compound molar masses to
Michael P. Broadribb, C. (2006). Institution of Chemical Engineers . Retrieved July 26, 2010, from IChemE: http://cms.icheme.org/mainwebsite/resources/document/lpb192pg003.pdf
Then the reaction tube was capped but not tightly. The tube then was placed in a sand bath reflux to heat it until a brown color was formed. Then the tube was taken out of the sand bath and allowed to cool to room temperature. Then the tube was shaken until a formation of a white solid at the bottom of the tube. After formation of the white solid, diphenyl ether (2 mL) was added to the solution and heated until the white solid was completely dissolved in the solution. After heating, the tube was cooled to room temperature. Then toluene (2 mL) was added to the solution. The tube was then placed in an ice bath. Then the solution was filtered via vacuum filtration, and there was a formation of a white solid. Then the product was dried and weighed. The Final product was hexaphenylbenzene (0.094 g, 0.176 mmol,
Explain in detail about the design and operation of packed distillation column, giving its design equations in terms of NTU and HTU.
In order to separate the mixture of fluorene, o-toluic acid, and 1, 4-dibromobenzene, the previously learned techniques of extraction and crystallization are needed to perform the experiment. First, 10.0 mL of diethyl ether would be added to the mixture in a centrifuge tube (1) and shaken until the mixture completely dissolved (2). Diethyl ether is the best solvent for dissolving the mixture, because though it is a polar molecule, its ethyl groups make it a nonpolar solvent. The compounds, fluorene and 1, 4-dibromobenzene, are also nonpolar; therefore, it would be easier for it to be dissolved in this organic solvent.
The Olefins II Unit makes hydrocarbons from naphtha or natural gas using furnaces. After distillation, the p...
In this lab, we found the Heat of Vaporization of liquid nitrogen, supported by the data we obtained. First, we calculated the amount of heat absorbed by the 60.00 g of liquid nitrogen we received. To do so, we had to add the liquid nitrogen to a Styrofoam cup containing hot water at 54.3 °C. We took the temperature of the water and nitrogen until it got to its lowest point, 20.2 °C. The water decreased by 31.5 °C after the liquid nitrogen vaporized. The mass decreased as well. After, we found the amount of heat the cup and water released to be 11,400 J, and the measured heat of vaporization to be 191 J/g or 45.6 cals./g. After, we compared this new heat of vaporization with the theoretical value of 199.9 J/g and attained a low negative percent error of -4.5%.
Gas-Liquid Chromatography utilizes the principle of the difference in solubility of the components of gas mixture (vapourized sample) in the non-volatile liquid phase. Volatile sample to be analyzed is vaporized and blown through heated column by inert gas carrier such as helium. The more sol...
The catalytic process occurs at lower temperature anf offers higher selectivity but requires frequent regeneration of the catalyst. Then, the products are cooled and introduced into a pair of separators which separate the unreacted hydrogen. The unreacted hydrogen is compressed and recycle back to the feed and reactor. The products that leaving the separators are heated before introduced into a distillation column which the toluene is separated from the stream and recycle back to the...
Process da: This low temperature liquid then enters the evaporator where it absorbs heat from the space to be cooled namely the refrigerator and becomes vapour