Ethylene Dichloride Chlorination
Perchloroethylene (PCE), along with Trichloroethylene (TCE), are the products of the chlorination of Ethylene Dichloride (EDC). This process involves the reaction of EDC with chlorine, where its products undergo further distillation and purification to produce TCE and PCE fit for consumerism trade. The stoichiometry of the given process reaction indicates which is the greater desired product, i.e. either PCE or TCE. The reaction takes place at a temperature of 400 – 450 degrees Celsius and a pressure of 1 atmosphere.
EDC and chlorine, in their vapour states, are fed into a chlorination reactor. This reactor operates at the conditions mentioned above (temperature: 400 – 450 degrees Celsius; pressure: 1 atmosphere). Chlorinated hydrocarbons that are by products from the reactor are recycled and fed back into the reactor. Chlorinated hydrocarbons and Hydrogen chloride exist in a mixture of the product stream from the chlorination reaction. Hydrogen chloride is then separated from the mixture. The chlorinated hydrocarbon stream is then neutralized and ...
While doing his research Molina learned that these compounds move up to the ozone and stay there. He expected the compounds to be destroy by the solar radiation. However to his surprise he formed that chlorofluorocarbons would simplify into component element when exposed to radiation. This simplify components produce a highly concentration of pure chlorine atoms. From there he already knew that the ozone layer can be destroy with chlorine.
In a small reaction tube, the tetraphenylcyclopentadienone (0.110 g, 0.28 mmol) was added into the dimethyl acetylene dicarboxylate (0.1 mL) and nitrobenzene (1 mL) along with a boiling stick. The color of the mixed solution was purple. The solution was then heated to reflux until it turned into a tan color. After the color change has occurred, ethanol (3 mL) was stirred into the small reaction tube. After that, the small reaction tube was placed in an ice bath until the solid was formed at the bottom of the tube. Then, the solution with the precipitate was filtered through vacuum filtration and washed with ethanol. The precipitate then was dried and weighed. The final product was dimethyl tertraphenylpthalate (0.086 g, 0.172mmol, 61.42%).
Saturated sodium chloride solution, also known as brine solution, is used to wash the distillate mixture. The distillate mixture is the phosphoric acid the co-distilled with the product. The brine solution also removes most of the water from the 4-methylcyclohexane layer. When six drops of 4-methylcyclohexene were added with two
I really don’t have that many bad things to write about. I forgot to shake my sep funnel after my first addition of dichloromethane. I had to redo that step. Also, there is a very slight chance that a little bit of dichloromethane could have been left in my final product. When I was distilling, I thought I had boiled away everything in my flask.
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Through an oxidation-reduction reaction sequence, Borneol is converted to isoborneol. First, borneol is oxidized through a reaction with sodium hypochlorite at 400C to form camphor. When the camphor is then reduced by sodium borohydride, isoborneol is formed. The percent yeild of isoborneol collected was 56.4%, and the melting point range was found to be between 174.2-179.90C. Through analysis of the product through 1H NMR spectroscopy the percent purity is found to be 77.2% pure isoborneol.
The boiling point of the product was conducted with the silicone oil. Lastly, for each chemical test, three test tubes were prepared with 2-methylcyclohexanol, the product, and 1-decene in each test tube, and a drop of the reagent were added to test tubes. The percent yield was calculated to be 74.8% with 12.6g of the product obtained. This result showed that most of 2-methylcyclohexanol was successfully dehydrated and produced the product. The loss of the product could be due to the incomplete reaction or distillation and through washing and extraction of the product. The boiling point range resulted as 112oC to 118oC. This boiling point range revealed that it is acceptable because the literature boiling point range included possible products, which are 1-methylcyclohexene, 3-methylcyclohexene, and methylenecyclohexane, are 110 to 111oC, 104oC, and 102 to 103 oC. For the results of IR spectroscopy, 2-methylcyclocahnol showed peaks at 3300 cm-1 and 2930 cm-1, which indicated the presence of alcohol and alkane functional group. Then, the peak from the product showed the same peak at 2930 cm-1 but the absence of the other peak, which indicated the absence of the alcohol
This excessive yield was resultant of the impurities within the product, where the solvents, particularly the dichloromethane, were not sufficiently removed from the product. In figure 3, the peak at 5.22 ppm with a normalised intensity of 1.00 evidenced the significant proportion of the dichloromethane in the product, and the peak at 0.88 ppm with a normalised intensity of 0.25 indicated some remaining hexane.4 The unreasonable yield was mostly attributed to these.
For part one of the experiment, my team asked the question of which cell fraction of the measured pea seedlings will have a higher ratio of chloroplasts? My group tested for the activity of chloroplasts with three different pairs of cell fractions by two conditions of light and dark in three readings. The first two cell fractions, pellet one and two (P1, P2), are the hard sediments found at the bottom of a tube after it has been centrifuged (which are specimen, like the mitochondria and chloroplast, that are isolated from the rest) (Leicht and McAllister, 2016). The last cell fraction used was the supernatant two (S2), which is just the free liquid surrounding the pellet after the centrifuging of P2 (Leicht and McAllister, 2016). To test for this, DCIP (a chloroplast isolation buffer) was used to
Before using ethylene to produce polyethylene, the compound needs to be purified to almost 100%. In order to reach this level of purity the ethylene needs to be freed of olefins, acetylenes, dienes and water through several processes such as: driers are used to take out the water, a demethanizer is used to remove methane, etc. ...
Process cd : This liquid refrigerant is collected in the liquid storage tank and later on it is expanded to low pressure and temperature by passing it through the throttle valve. At point d we have low temperature liquid refrigerant with small amounts of vapour .
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...
The sample was subjected to steam distillation as illustrated in Figure 1. A total of 50ml of distillate was collected while recording the temperature for every 5.0 ml of distillate. The distillate was transferred into a 250ml Erlenmeyer flask and 3.0 g of NaCl was added. The flask was cooled and the content was transferred into a 250-ml separatory funnel. Then 25.0ml of hexane was added and the mixture was shaken for 5 minutes with occasional venting. The aqueous layer was discarded and the organic layer was left inside. About 25.0ml of 10% NaOH was then added and the mixture was shaken as before. The aqueous layer was collected and then cooled in an ice bath. It was then acidified with enough 6.00 M HCl while the pH is being monitored with red litmus paper. Another 25.0 ml of hexane was added and the mixture was shaken as before. The hexane extract was saved and a small amount of anhydrous sodium sulfate was added. The mixture was then swirled for a couple of minutes then filtered. A small amount of the final extracted was tested separately with 1% FeCl3 and Bayer’s reagent.
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.
Many companies all over the world produce chemicals for their products that are harmful to the environment, human health, and to all living species. Green Chemistry is the use of chemistry for the prevention of chemical pollution to the environment by using chemicals that are benign, or not harmful. The Environmental Protection Agency (EPA) states that the mission of Green Chemistry is, “To promote innovative chemical technologies that reduce or eliminate the use or generation of hazardous substances in the design, manufacture, and use of chemical products.” Green Chemistry contains any aspects and types of chemical processes that reduce the negative effects of certain chemicals, in a way, using chemistry to fight chemistry.