How has the Halogen Bromine, been used to protect swimming pools?
The Halogen Bromine (Atomic number: 35, Atomic weight: 79.9) is the only non-metallic element that’s state is liquid at room temperature . Bromine, produced firstly by Carl Lowig, was not associated with him as even though he was believed to have first created the element his student life took priority giving Antoine-Jérôme Balard another chemist, enough time to discover Bromine for himself and publish a paper in 1826 discussing his findings. It was Balard who was credited with the discovery and thus named the chemical Bromos, “stench” in Greek.
The reddish-brown element (also giving of a very strong odour not dissimilar to that of chlorine) is obtained from sea water and some brine mixtures – that have been left from the production of potassium salts. This process of obtaining bromine starts when Bromine in water is oxidised by chlorine - above the boiling point of Bromine - in order to create Bromine gas or Br2.
2Br + Cl2 → Br2 + 2Cl ( )
This produces a mixture of both Bromine and Chlorine gasses, separating when the mixture cools to a point when Bromine liquefies yet chlorine (still above it’s boiling point) stays as a gas. If extra purification is needed, the Bromine Gas can be mixed with sulphur dioxide. Then, after it is run through a cylinder (with running water falling in the opposite direction) both gasses react with the water to produce hydro bromic acids and sulphuric acids.
SO2+ Br2 + H2O → 2HBr+ H2SO4 ( )
A Primary use of bromine is in the engineering of pharmaceuticals. Brominated substances are key components in many “over-the-counter” but also prescription drugs . These include various sedatives and antihistamines (a form of prote...
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This experiment was divided into two main steps. The first step was the addition of bromine to trans-stilbene. Trans-stilbene was weighted out 2.00g, 0.0111mol and mixed with 40ml of glacial acetic acid in 100ml Erlenmeyer flask on a hot bath. Pyridinium hydrobromide perbromide of 4.00g, 0.0125mol was added carefully into the flask.
Discussion and Conclusions: Interpreting these results have concluded that relative reactivity of these three anilines in order of most reactive to least reactive go; Aniline > Anisole > Acetanilide. Aniline, has an NH2 , the most active substituent , and adds to any ortho/para position available on the ring. This data is confirmed with the product obtained, (2,4,6 tribromoaniline, mp of 108-110 C). As for anisole, it has a strongly activating group attached, OMe an alkoxy group, and it added in two of the three available spots, both ortho. The results conclude: (2,4-Dibromoanisol mp 55-58 C ). Acetanilide has a strong activating group attached, acylamino group, but this group is large and the ortho positions are somewhat hindered so the majority of the product obtained added at the para position, results conclude: (p-bromoacetanilide mp 160-165 C). Since all the substituents attached to the aromatic rings were activators the only products able to be obtained were ortho/para products.
The IR machine was cleaned between uses to reduce contaminated data. The final product was run through the IR spectroscopy to measure the amount of light absorbed and compare it to a graph of pure 1-bromobutane to determine if it is the actual final product obtained. This comparison also shows any impurities in the final product. The graphs were similar but not perfect, implying that an impure product of 1-bromobutane was obtained. To identify the functional group of the molecule, the frequency range of the light absorption patterns was observed. Different functional groups are excited at different unique ranges between 4,000-1,250 cm^-1. The C-H axis could be found in this range. The structure of the molecule is determined by looking at a fingerprint region (1,250-500 cm^-1). The C-Br axis should be visible in this range but the IR machine was not sensitive enough. The fingerprint region is unique to each compound and helps determine things such as stereochemistry. It is important to add sodium sulfate to the product before running it through the IR. This will remove OH from the product so that it will not show up in the spectroscopy. There should be no peaks at OH after the test. My sample for this experiment had to be run through the IR spectroscopy twice because the first time had a significant OH peak. Adding more sodium sulfate to the solution and running the IR again eliminated
Paturau, J.M. 1982. By-products of the cane sugar industry. Second ed. Elsevier scientific Publishing Co., New York. 366 pp.
Despite the significant benefits of pool chlorines in their capacity to kill hazardous bacteria, it is evident that some of the side effects can be disadvantageous. The general smell of chlorine can be overwhelmingly unpleasant, and the agent can irritate the skin and eyes. It is also has the capability to bleach some fabrics, potentially damaging clothing. Most significantly, excessive air pockets of chlorine gas that surround pools can be hazardous for peoples’ health and possibly even be carcinogenic. For these reasons, some industries have started to investigate new alternative methods to chlorine for sterilising pools. According to Smith and Monteath et al. (2006, pp. 1 - 37), ‘some of these are good alternatives, but they do not achieve the cleanliness, oxidation levels or low price that chlorine provides’.
20 Brendan Hill, Victoria the place to be, Molecular Gastronomy research and experience, (June, 18, 2008) date accessed February, 7. 2013
Murphy, Suzanne P., and Lindsay H. Allen. "Nutritional Importance of Animal Source Foods." The Journal of Nutrition 133.11 (2003): 39325-9355. Web.
Enantiomers, a type of isomer, are non-superimposable, mirror images of each other. Diasteriomers, another type of isomer, are non-superimposable, non-mirror images of each other. Dimethyl maleate and dimethyl fumarate are diasteriomers, as they are not mirror images but instead vary in the orientation of the carbomethoxy groups around the double bond. Dimethyl maleate is the cis-isomer because both groups are on the same side and dimethyl fumarate is the trans-isomer because the two groups are on opposite sides. A bromine free radical mechanism was required for this conversion. First, energy from light is required to create two bromine free radicals from Br2. Then one of the free radicals attacks the double bond in dimethyl maleate, breaking it and creating a carbon radical on the other carbon. The bond then rotates and reforms, freeing the bromine radical and creating the trans-isomer, dimethyl fumarate. Bromine in this reaction is acting as a catalyst in this reaction and then cyclohexane is added at the end to neutralize the bromine free radicals. The activation reaction of the radical reaction is lower than the activation energy of the addition reaction, which is why it occurred more quickly. This reaction was successful because the percent yield was 67.1%, which is greater that 65%. It also demonstrated the expected principles, as the reaction did not occur without the presence of both light and bromine. The dimethyl fumarate had a measured boiling point of 100C to 103C, which is extremely close to the expected boiling point of 102C to
Over the years, meat eating has grown dramatically in many countries. Demand for meat production increased at a fearsome speed, which led to producers using pesticides and fertilizers on their crop. Because of our exponential population we could not begin to feed the population of the world without them. Farmers will need to increase the amount the chemicals used on their crops and animals to accelerate production process i...
...ute of Food and Agricultural Sciences." Monroe County Extension Office – Solutions for Your Life - UF Institute of Food and Agricultural Sciences. 2011. Web. 19 Mar. 2011.
This suspension was allowed to stand for 10 minutes, before being filtered, washed (water 2 x 10 mL) and air dried. The crude product was recrystallised from ethanol to yield a yellow solid 3. 26% yield (1.83 g); Elemental analysis for C12H17NO4: C: 54.918%, H: 6.704%, N: 5.122% (Theoretical: C: 60.24%, H: 7.16%, N: 5.85%, Loss:26.75%); Mr 239.2 g mol-1; ν/cm-1: 1259.48 (N-C), 1667.41 (C=C), 1688.41 (C=O), 2976.58 (C-H), 3265.02 (N-H); 1H-NMR (400 MHz, CDCl3), δ/ppm: 1.24 and 1.38 (dt, 3H, C-CH3, C12 and C15), 2.51 and 2.56 (ds, 6H, 2 x =C-CH3, C6 and C7), 4.31 (m, 4H, 2 x -CH2-, C11 and C14), 5.3 (s, 1H, N5-H); 13C-{1H}-NMR (400 MHz, CDCl3), δ/cm-1:11.98 (C6 and C7), 14.43 (C12 and C15), 59.50 and 60.29 (C11 and C14), 133.5 (C3), 117.5 (C1), 131.3 (C2), 138.6 (C4), 165.47 (C8 and C9) .
of sucrose, 88.5 lb. of allyl chloride, 46.2 lb. of sodium hydroxide and 23.1 lb. of water by Griffin, Willard, Sinnamon, Edwards and Redfield, Ind. Eng. Chem., 43, 2629 (1951) [5].
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The process need toluene and hydrogen as a main reactor. Then, toluene and hydrogen are converted in a reactor packed with catalyst to produce benzene and methane. This reaction is exothermic and the operating conditions are 500 0C to 660 0C, and 20 to 60 bar of pressure. This process begins with mixing fresh toluene with a stream of recycle unreacted toluene, and the mixing is achieved in a storage tank. Then, the toluene is pumped to combine it with a stream of mixed hydrogen and fresh hydrogen gas. The mixture of toluene and hydrogen is preheated before it is introduce to the heater or furnace. In the furnace, the stream is heated to 600 0C, then introduced into the reactor. Basically, the main reactions occurs in the reactor.
Keener, K., Hoban, T. and Balasubramanian, R. 2014. Biotechnology and its applications. [online] Available at: http://www.ces.ncsu.edu/depts/foodsci/ext/pubs/bioapp.html [Accessed: 11 Apr 2014].