The identification of the melting point of the organic acid was done to find another characteristic of the acid and to test the purity of the recrystallized pure acid. A 2-4 mm layer of unknown sample was placed into a capillary tube sealed on one end. Then the capillary tube was inserted into the side a Bibby Sterlin device. The plateau was set to 200°C on the melting point apparatus. Once the plateau temperature was reached, the sample was watched carefully. When the sample first began to melt and when it was fully melted was recorded. These numbers were the range of the melting point. A slow melting point of the unknown organic acid and a standard sample was completed next. A new plateau was set about 10°C lower than the observed melting point of the unknown sample. This time once the plateau was reached, the heating was no more than 1°C per minute. This gave a much more accurate read of both melting points. If the standard did not melt in the range listed on the label of the bottle, that meant the machine was not working properly. The standard sample and the unknown organic acid melted in their appropriate ranges.…
9) Put 4mL of stock solution and 1mL of water in a test tube to make the second solution.…
2. To determine the densities of water, an unknown liquid, a rubber stopper, and an unknown rectangular solid.…
The goal of this experiment was to separate Toluene and Hexane by distillation and gas chromatography based on their difference in boiling points. The boiling point of hexane is 69 degrees Celsius and the boiling point of toluene is 110 degrees Celsius. Three fractions were collected for both simple and fractional distillation. The first fraction was hexane since it had the lower boiling point. The second fraction was a mixture of toluene and hexane. The third fraction was toluene since it had the high boiling point of 110 degrees Celsius. Gas chromatography was also preformed on each of the fractions from simple and fractional distillation. In the gas chromatography process, the compounds are carried through a stationary phase, and pushed…
.2400 grams of the unknown compound. This is done in duplicate and purple-tinted precipitates are placed in Gooch crucibles. The precipitates are suction dried using ethyl alcohol then acetone to…
In terms of percent recovery for cyclohexane, it can be concluded that there was a higher yield of cyclohexane collected when the compound underwent simple distillation than when the compound underwent fractional distillation. For toluene, both simple and fractional distillation produced the same quantity, deeming it appropriate to use either technique only in regards to collecting toluene. Simple distillation is considered more effective when the boiling point differences between the two substances are high, which is the primary reason why simple distillation produced a higher yield and thus, a higher percent recovery. Fractional distillation in this case, produced only 74% of the original amount of cyclohexane that was entered into the apparatus…
Analysis via gas chromatography allowed us to determine the relative percentage of hexane and toluene at fractions near the beginning and end of our distillations. Relative percentages have been recorded in the table below, and our calculations are shown on page 5.…
The goal of experiment 1 was to determine the properties and reactions of hydrocarbons. This was achieved by testing solubility and observing the effects of different interactions between solvents and isooctane. Overall procedures involved mixing 9 different solvents with isooctane and observing solubility with the naked eye. It was concluded that 5 of the combinations proved soluble, 2 completely insoluble, and 2 were insoluble at room temperature but soluble if heated. Also tested was the reactivity of cyclohexane and cyclohexene in sulfuric acid which tested to prove reactivity between cyclohexene but not cyclohexane. Finally tested was the reaction between bromine and alkenes, which showed reaction between the more polar alkenes than non polar.…
Toluene is a clear colorless liquid that has an aromatic odor. It ignites in air at 40 degrees Fahrenheit. It is also less dense than water and because so will float atop it. Toluene is non-corrosive.…
Cumene is a compound that less dense than water and insoluble in water as well as moderately toxic if inhaled (Cameo Chemical, n.d). In order to produce phenol and its by-product acetone, cumene undergoes oxidation process to produce cumene hydro peroxide (Sbio, 2003). Cumene hydro peroxide then is split into phenol and acetone by catalytic action using dilute sulphuric acid (Sbio, 2003). Besides, cumene is a stable compound, but may form peroxides in storage if in contact with the air so it is important to test for the presence of peroxides before heating or distilling. The chemical also flammable and incompatible with strong oxidizing agents.…
In conclusion to the distillation lab, I think our data shows that our experiment went well. Our graph resembles the graph in the lab handout (graphs attached to lab notebook sheets). The fractional distillation shows the sharp slope between when the cyclohexane burns off and mostly only toluene remains. The microscale graph seems to be accurate because it shows the large jump where the cyclohexane is burned off. To view the apparatuses used in the experiment look at the attached pictures. To compare the simple and fractional distillation, our GC analysis shows the samples we submitted. The first samples of our simple distillation showed that 76.21 percent of the mixture was composed of cyclohexane and 23.36 percent was toluene. The first few drops of our fractional distillation had cyclohexane composing 70.56 percent of the mixture leaving 29.27 percent for toluene. The other set of data is for the last drops obtained. The simple distillation final drops analysis showed 12.11 percent of cyclohexane and 87.78 percent of toluene in the mixture. These numbers compare to the final drops of the fractional distillation which showed 19.48 percent cyclohexane to 80.38 percent toluene. The fractionating column is used to increase the efficiency of the distillation process which is supposed to give a nearly pure final product. The reason our data might now show this is because the final drops of the fractional distillation weren’t collected before taking it off the heat. This could have allowed some of the cyclohexane to condense and when the drops were finally obtained, some cyclohexane could have gotten in the…
Harry Gilbert, Cuyahoga Falls- With an inert solvent or diluent such as benzene, toluene, trichlorobenzene…
The purpose of this experiment is to understand the process of distilling a solution. Thesolution of 50/50 ethanol-water was used in the experiment. Using fractional distillationapparatus ethanol-water mixture was separated. The fractional use of copper sponge wasused in distillation process which created the heat exchange area between the vapor of ethanol and liquid water. The fractional distillation process yield 9.5 ml of ethanol incollecting flask, thus the hypothesis was accepted.The purpose of this experiment is to understand the process of distilling asolution. Distillation deals with a mixture, a solution composed of two or more elements,that when boiled, will cause each element to vaporized at different temperatures…
The purpose of this lab is to distill crude oil and learn how the chemical properties influence the temperature. The distillation of a substance is based on the boiling points. When the crude oil is brought to a boil, at 275°C, the gasoline and kerosene are distilled, but the lubricant remains part of the crude oil.…
Next, Cyclohexane and Toluene were distilled. The boiling points of cyclohexane and toluene had a difference of 35°C. Cyclohexane had a percent recovery of 10%. Toluene had a percent recovery of 17%. The percent efficiency…