can anyone help me with this topic? other then ammonolyisis of phenol and hydrogenation of benzene, i could not find any other methods for production of aniline? pls provide the url if any is found thanks
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Search http://www.scirus.com
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You can produce benzyl alcohol from benzaldehyde by the crossed Cannizzaro reaction (see link below), but there is a theoretic maximum yield of 50% only.
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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
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just mix petrolium and flour together in a bottle - make it thick into a sauce\n\nthat is instant NAPALM !!!!!!!!!!!!!!!!!!!!!!!
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In most of the cases the catalyst is insoluble and you can filter them out.\nFor hydrogentaion., Pd/H2 is one of the useful techniques.... but this catalyst will not be soluble.. its a black powder.. after hydrogenation, you can filter it off.\n \nI remembercatalysts like Raney Nickel or Raney Cobalt also will not soluble.. you need to filter them off on Celite porus plug.\n\nHope this info will help you
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Can you give more info?  There seems to be much info on making fuels by this method, but nothing on quenching.
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no there isn't but it will last about 1-2 hours. ammonium nitrate and water it the reaction.
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If you are dealing with a reaction involving ammonium carbonate in solution, and are then measuring the temperature rise, you need the heat capacity of water, not ammonium carbonate!\n\nPlease post the whole problem if that is not enough to get you started.
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Gee, I know you're a student but you are dull and lazy.\n\nHaven't you heard of google??  \n\nStep 1 - I went to www.google.com\nStep 2 - I used the following search  "electroclorination +equation"\n\nhttp://www.google.com/search?hl=en&lr=&q=electrochlorination+%2Bequation\n\nStep 3 - I followed the first link (listed below) on the google.com search results.\n\nAnd you've waited how many days for this answer?  It took me less than one minute to find.
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Habers process is a reversible reaction where ammonia is formed from the reaction of nitrogen and hydrogen using a iron catalyst.\n\nOptimal temperature is 400K and 100 atm pressure. This provides a the optimal yield within time restrictions.\n\nSearch Habers Process on google, yahoo, etc..to find out more information
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There are many ways to generate hydrogen outside electrolysis. Steam reforming, methane reforming, propane reforming, etc... Coastal countries may appear to have an advantage but you cannot have a fair comparison of supply and demand.  Consider the following:\n1. Many, many, many countries have access to coastal water, thus competition would be extremely fierce\n2. Countries will be more than self-sufficient and may "sell" excess product at a very low cost.\n3. Rivers, streams, rainwater etc... is available to more countries in the world than petroleum to many. \n \nI would not worry about it, depleting the sea is way way way way off, and besides, using H2 as fuel means that emission is....water. And no, the roads are not going to be slippery from algae (sorry, but I have heard a statement like that in the past)\n\nEver considered that we may come up with the technology to recover and re-use the water emission? Thus less filling up at your local Shell H2 station? \n\nI hope I was able to answer it for you in a objective manner
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The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
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http://www.chem.uni-potsdam.de/~thomas/1hbuch/english/index.html\n\nhere is a website that seems short and simple\ngood luck
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Concept: An element and a compound can react to form another element and another compound. \n\nMaterials: 200 mL of 0.1M copper(II) chloride (CuC12), 5 cm. square piece of aluminum foil (Al), 400-mL beaker, safety goggles. \n\nProcedure: 1. Place the beaker of copper(II) chloride in front of the class. 2. Crumple the aluminum foil and throw it in the beaker. 3. Soon the solution starts to bubble as hydrogen gas is produced. 4. A red brown precipitate of copper falls to the bottom of the beaker, and the aluminum foil dissolves completely. 5. Aluminum would react spontaneously with water without its protective oxide coating. The aluminum-copper(II) chloride reaction removes this protection. Caution: Copper(II) chloride is an irritant. \n3CuCl2 + 2Al --> 2AlCl3 + 3Cu\n\nInput = 3CuCl2 + 2Al \nOutput = 2AlCl3 + 3Cu
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If you have them in solution?  Aqueous or organic solvent?\n\nThe phenol group is acidic.  Assuming that the other portions of the molecule do not counteract the acidity, you can extract them from an organic matrix with basified water like bicarbonate solution.  If you want to get them back into an organic solvent, you have to acidify the aqueous system they are in and they'll start acting like regular organic molecules.\n\nThis is only one way.  There's lots and lots but you've given us very little to go on.
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Silver tarnishing.\nBurning natural gas for cooking.\nCharcoal grill (burning charcoal).\nBleaching an ink or grass stain from clothing.\nCopper pipes turning "green."\nCooking (think of boiling an egg).\nExploding gasoline vapor in an automobile engine.\nLighting a cigarette lighter (propane burning).\nA burning candle (paraffin or wax).\nPaper or leaves decomposing.\nElectricity production from the chemicals in a battery.\nBread dough rising.\nFermentation of wine or beer.\nToast burning.\nMaking caramel.\nMixing Jello.\nTreating hard water to remove minerals.\nAcid rain dissolving limestone.\nOzone production by an electrical spark or lightening.\nOxygenation of exhaust gases by a catalytic converter on a car.\nBaking a cake.\nMaking pickles.\njust to name a few.
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2.\nBy decreasing the temperature and increasing the pressure. As ussually done in Haber;s process\nAnother way is to keep on removing the ammmonia gas to make reaction go forward\nRead th Le Chatelier's principle for more detail.\n\n13.\n2 HCl + Na2CO3  -----> 2 NaCl + H2CO3\nH2Co3 can exist as water and carbon dioxide.\n\n14.\nBecause acid-base reaction is spontaneous.\n\n11.\nBecause of the formation of copper(II) carbonate which will settle down as precipitate.