how do you synthesize 5-amino-2-nitrobenzotrifluoride from toluene?
491215
-Fluorinate toluene with F2 (highly controlled) or FCl or F5Cl, or DAST or one of these other nice fluorinators - gives the trifluoride on the methyl carbon\n-Nitrate it with nitric acid/sulfuric acid - CF3 is withdrawing so nitro goes on the 3-position\n-Reduce the nitro with Sn/HCl or H2/Pd\n-Nitrate again - the amino protonates and directs to the 5-position\n-Titrate the water to basic pH and extract with solvent like ether.  Concentrate and purify - probably crystallizes nicely.
788534
N2 + 3H2 -> 2NH3\n\nN2 has a gfm of 28g/mol and H2 has a gfm of 2g/mol.  (you do the math to find the moles I will make a rough guess) you've got about .5 mols of N2 and about 1 mole of H2, so H2 is your limiting reagent.  your ratio of H2 to NH3 is 2molNH3/3moleH2 and you multiply that by the one mole of H2.\n\nNH3's gfm is 17g/mol so .667molNH3 x 17g/molNH3 ~ 12g\n\n*edit* make sure you do the math over because I was guessing and estimating where you should not *edit*
316857
Part 2: Synthesis of Benzil \n\nStarting with the a-hydroxyketone benzoin (prepared in Part 1), you will prepare an oxidation product, benzil, which is an a-diketone. \n\n \n\nThis oxidation can easily be done with a variety of mild oxidizing agents, including Fehling's solution (an alkaline cupric tartrate complex) or copper(II) sulfate in pyridine.  In addition, benzoin could be oxidized by sodium dichromate, but the yield of benzil is lower because some of the benzoin is converted back into benzaldehyde following cleavage of the bond between the two oxidized carbon atoms, which is activated by the phenyl rings, producing benzoic acid as the final product.  In this experiment, due to ease of use and consistent results, we will use nitric acid as the oxidizing agent. \n\nCaution: Concentrated nitric acid is highly corrosive and causes severe burns if spilled onto your skin. Nitrogen dioxide (NO2) fumes are highly toxic and can damage the lungs due to inflammation. Do not breathe NO2 fumes, and perform this part of the experiment in the hood. \n\nProcedure \n\nHeat a mixture of 4.0 g of benzoin (prepared in Part 1; save enough for analysis, but proportion reagents as needed) into a round-bottom flask with 14.0 mL of concentrated nitric acid.  Add a stirring bar and attach a condenser to the top of the flask. Set up a reflux in the hood to vent NO2 produced during the reaction. With stirring, heat the reaction mixture. Begin timing the reaction when NO2 (red-brownish colored gas) are visible above the reaction mixture and gas bubbles are present on the stir bar. Reflux for at least 30 minutes, or until no more NO2 gas is apparent. Do not stop the reaction until the reaction is complete. Stop the reaction by removing the heating mantle, and letting the reaction mixture cool for about 5 minutes.  Add about 75 mL of cold water to the reaction mixture, cool to room temperature, and swirl for a minute or two to coagulate the precipitated product: collect and wash the yellow solid using vacuum filtration.  Continue drawing air through the crystals on the funnel by suction for about 5 minutes to assist in drying the crystals..  The crude product (dry weight 3.7-3.9 grams) need not be dried but can be crystallized at once from ethanol.  Dissolve the product in 10 mL of hot ethanol, add water dropwise to the cloud point (mixture goes from clear to cloudy, or solids being formed), and set aside to crystallize.  Record the yield, crystalline form, color, and melting point of the purified, and recrystallized, benzil.   \n\nTest for the presense of unoxidized benzoin: Dissolve about 0.5 mg of crude or purified benzil in 0.5 mL of 95% ethanol or methanol and add one drop of 10% NaOH.  If benzoin is present the solution soon acquires a purplish color owing to a complex of benzil with a product of autoxidation of benzoin.  If no color develops in 2-3 min, and indication that the sample is free from benzoin, add a small amount of benzoin, observe the color that develops, and not that if the test tube is stoppered and shaken vigorously the color momentarily disappears; when the soluton is then let stand, the color reappears. \n\nCleaning up: The aqueous filtrate (containing HNO3) should be neutralized with sodium carbonate, diluted with water, and flushed down the drain.  Ethanol used in crystallization should be placed in the organic solvents container.
932873
Go to "protein" on wikipedia ( put, protein, in address bar ) then scroll down to "synthesis", for the process. It is too  long a story for my typing skills. The wiki article is not too technical.
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I know of at least 4 ways.  I think that the distillation or membrane separation are the most practical.\n\n(1)Distillation\nOxygen and nitrogen have different boiling points.\noxygen: 90 K\nnitrogen: 77 K\nIf you cool the mixture to a temperature between the boiling points of each you will be in a two-phase region.  There will be a gas phase rich in nitrogen (because it has a lower boiling point) and a liquid phase rich in oxygen.  A distillation column can be used to separate the phases and collect them in a continuous, pretty efficient process.  I think you have to do something special about the argon in air when you do this (like have more than one separation step, more than one distillation column).\n\n(2)Adsorption\nOxygen and nitrogen gases may adsorb to (stick to) the surfaces of certain compounds (like metal surfaces).  If you make a series of tubes lined with a substance that preferentially adsorbs (for example) oxygen, you will get a gas output that has less oxygen in it.  In a well-designed case, the adsorption is reversible.  Increasing the temperature of the substance will causes the oxygen to leave the solid surface and once again become a gas, giving you a relatively pure oxygen stream.  If the purity is not good enough, you can collect the streams and repeat the process (use a longer tube).  I don't know of an example of an adsorption material off-hand.\n\n(3)Stripping\nStripping is the process of passing a gas through a liquid and may involve chemically removing one of the components of the gas.  If you bubbled air through a liquid that had a chemical in it that reacted with oxygen to form a compound then the gas that reaches the top will be nitrogen-rich.  For example, your blood contains hemoglobin, so that when it is in contact with the air in your lungs the oxygen sticks to the hemoglobin, forming a chemical complex.  This is a lot more effective than limiting yourself to an oxygen supply based on whatever gases can dissolve in your blood. \n\n(4)Membrane Separation\nOxygen and nitrogen have different permeability in membranes.  They can diffuse through solids, but at different rates.  I think oxygen typically has high permeability.  If you pressurize the gas mixture and pass the gases through a bundle of tubes (high surface area is key) then some gas will pass through the tubes axially and some will diffuse through the walls radially.  The stream that passed through the tubes will be richer in nitrogen, since it is less permeable.  The stream that diffused through the walls of the tube will be richer in oxygen, becuase it is more permeable.  Repeat the process to get the desired purity.\n\nAn artificial lung can be made by passing blood through a long set of tubes that have oxygen on the outside of the tubes.  The oxygen diffuses into the blood through the permeable tubes.
239315
im pretty sure that would be a very volatile compound but im not sure what the combination or final chemical compound would create but I think the best place to find ammonia nitrate is in ceratin types of fertilizers
405453
If you do the above reaction, you can get the following compounds: (chloromethyl)benzene, (dichloromethyl)benzene, and (trichloromethyl)benzene.
644051
See if this article has a diagram\n\nhttp://jchemed.chem.wisc.edu/Journal/Issues/1999/Apr/abs542.html
1075365
Dinitrogen oxide is somewhat soluble in water and it will simultaneously also get oxidized to give NO2 as brown fumes. NO2 will further dissolve in water to give nitric and nitrous acid. \n\nN2O (g) --------> NO2(g)  (in water)\nNO2(g) + H2O(l) ------> HNO3(aq) + HNO2(aq)\n\nIndustrially, CuSO4 is made by first heating scrap Cu with sulphur:\n\nCu(s) + S(s) -----> CuS(s)\n\nThe sulphide is then oxidized by heating it in excess air:\n\nCuS(s) + O2(g) ---------> CuSO4(s)\n\nIn the lab, you can heat some dilute H2SO4 in a beaker and then add excess of copper(II) oxide a little at a time and stir. You'll get a blue solution of CuSO4 and a black precipitate of the excess CuO which didn't react with the acid. By filteration, you'll separate the precipitate and get CuSO4 solution as a filterate which you can heat gently and then cool to obtain crystals.
160185
try this website, I just did a search and this came up:\n\nhttp://nuclearweaponarchive.org/Nwfaq/Nfaq5.html
6121
Hey cable_ray,\n     One of the most easiest way to get the recipie you require or any other synthesis can be found on the following website. It is the organic synthesis website, maintained by cambridgesoft.com. It is a free service they provide. You can use it. Just put in the name of the ether you want to produce eg. dimethyl ether, diethyl ether, etc. I am an MSc by research student. So you can also mail me. I will surely reply. my mail add is jchemie@gmail.com
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Key points to look for include:\n\nInfrared\n-NO2 bonds: 1515-1560, 1345-1385\nAlkenes: C-H: 3020-3080 (moderate), 675-1000\n         C=C: 1640-1680(variable) \nIf wet: Large OH hump in the 3500 area... should obliterate most other peaks in the area.\n\nI am not as up to scratch with NMR.\n\nThis is a common compound and an IR and NMR spectra should be easily found on the internet. I recommend chaecking them carefully as jus tlooking for the peaks above will probably not be highly useful.\n\nEven better than the internet is a resource book, any laboratory or university library should have such resource books.\n\nPersonally I recommend that if you are doing much organic chemistry to get 'Organic CHemistry' by Morrison R.T. and Boyd R.N., published by Prentice Hall.\nThis book has an excellent guide for spectra.
1150323
Methcathinone can be synthesized by oxidation of (pseudo)ephedrine with (di)chromate salts, or via Jones reagent.Here is the synthesis via Jones reagent:\nOxidizing the Alcohol to a Ketone\n1.068 grams (just over 1 gram) CrO3 are added to 0.92ml H2SO4, and distilled water is added to bring the total volume to 4ml. 2 grams of pseudoephedrine are dissolved in 20ml acetone, and cooled in an ice bath. The Jones reagant is slowly added to the pseudoephedrine, dropwise and with stirring. The mixture becomes a reddish brown.Since we used just about the exact number of molecules required, and under very mild conditions, the reaction will proceed slowly, but very smoothly. Just let the ice melt and the stirred solution warm over night.\nExtracting the Ketone\nAbout 12-18 hours later the reaction is complete, the color is now a very dark green. We now have to neutarlize and extract our ketone. Add about 20mL of water, and chill in an ice bath. Dropwise and with stirring add about 1 gram of lye (Sodium Hydroxide - NaOH) in a solution with as little water as possible (highly concentrated). Check the pH regularly, and stop at pH=12. The now basic solution is shaken with 50ml of toluene. Allow to stand and two layers will form. The ketone will move into the toluene layer. Let the mix settle and remove the acetone/toluene/ketone and put it aside. Add another 50mL portion of toluene to the aqueous (water-based) portion, shake, filter (which breaks the emulsion and removes some chromium salts), and remove and put aside the toluene. Ensure that pH is still 12, and repeat again with another 50mL portion of toluene.Combine the three toluene extractions and evaporate them with a hair dryer. The result is the impure ketone of pseudoephedrine, also know as methcathinione or ephedrone.We used very gentle oxidation, neutralization, extraction, and evaporation conditions. Shortcuts can be used (no ice, evaporate with some heat, etc.), but good lab practice is never to stress the substrate needlessly. So we were careful.The raw "dirty" methcathinone weighs about 1.7 grams.It is purified by adding just enough tolene to redissolve it. Some particles will not dissolve, and are left in the drying dish. The toluene is filtered to remove any additional particles, poured back into the separation funnel and shaken with an equal amount of distilled water. This removes any small amount of water solubles. The toluene is put into a clean dish and dried once again. The impurities are more soluble in acetone than the ephedrone, so a very small amout of acetone is added, and sloshed around. Pour this off into the waste (original green mix). What's left is a little over 1 gram (about 60% yield) of relatively pure, slightly off-white methcathinone.\nBetter chemists can expect a much higher yield. This is a general procedure. The example given -Pseudoephedrine or Ephedrine to Methcatinone - is for illustrative purposes only. Oxidizing cold pills is illegal, and makes a lousy drug anyway
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I was able to find the following citation in a database called AGRICOLA, created by the National Agricultural Library:\n\nTitle:  Total nitrogen determination in plant material by means of the indophenol-blue method.\nAuthor:  Novozamsky, I.\nOther Author(s): Eck, R. van.\nSchouwenburg, J.C. van.\nWalinga, I.\nSource Info: Netherlands journal of agricultural science. Neth J Agric Sci 1974, 22 (1)\np. 3-5.\n\nIf you happen to live near Beltsville, MD you can go to the National Agricultural Library, request the journal and copy said article.\n\nIf you do not, you can make a request through your local library.  If you are not in the U.S., they will send a copy of the article to some libraries in another country.  If you are in the U.S., you can make the request through your public library.\n\nYou can also see whether there is a library closer to you that has this journal by looking through something called Worldcat.  If the link works correctly, you search for this journal and then enter your zip code to see libraries in your area that may have it.\nhttp://www.worldcatlibraries.org/wcpa/top3mset/54df6814ac864cc4.html\n\nIf the link does not work, your local library should be able to get this information for you.
138623
Go to http://rutchem.rutgers.edu/Courses_f04/Chem161/Lecture19k.pdf#search='lewis%20structure%20for%20nitrous%20oxide' and scroll down until you see it
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If you havent had University training on organic chemestry, and don't have the lab equipment (about $5000 atleast) its gonna be pretty impossible. LSD is a very hard Compond to synthasize.\n\nThe closest thing to LSD u can make yourself is probly an LSA Extraction (LSA is similar but not as potent as LSD) From either Hawaiian baby woodrose seeds or Morning glory seeds. \n\nThese extractions are rather simple requireing only A high proof alcohol (bacardi 151, everclear) and Naptha (Zippo lighter fluid will work)\n\nHow to do this can be found probly on a google search or http://www.erowid.org/plants/hbw/\n\ngood luck, and if you read anyhting that tells you how to make LSD and looks asthough u would be able to do it, it wont be LSD but either lsa or somthing that will kill you.
1037670
I think you'll need to go to a university library or get a subscription to some online chemistry journals. Emil White, D. Mead Johnson Professor of Chemistry and faculty member in the Krieger School of Arts and Sciences at John's Hopkins was the first to synthesize it. Here's one promising reference:\nWhite, E.H., F. McCapra, G.F. Field, and W.D. McElroy, J.Am.Chem.Soc., 83,2402 (1961).\n\nHere's some leads:\nhttp://www.modares.ac.ir/sci/saman_h/Pages/Firefly.htm\nhttp://cas.bellarmine.edu/chem117a/lab/luminol.htm\nhttp://www.jbc.org/cgi/reprint/233/6/1528\nhttp://phot.allenpress.com/photonline/?request=get-document&doi=10.1562%2F0031-8655(2002)076%3C0153:TTMFPP%3E2.0.CO%3B2\nhttp://www3.interscience.wiley.com/cgi-bin/jhome/10009400\nhttp://www3.interscience.wiley.com/cgi-bin/jhome/4087