what is the application of nitro chloro benzene?
408997
Nitrochlorobenzenes are used in making needles, prisms and leaflets. They're also used in the manufacture of nitroanilines and nitrophenols by treatment with ammonia or dilute alkalis.\nNitroanilines are important dye-stuffs intermediates and used as first components in the preparation of azodyes.\nNitrophenols are used in dyestuffs and photographic processes.
342187
There are many you could choose.  These may not be the most efficient, but I'm just going with initial thoughts here.\n\n1.  Aniline -> benzamide\nDiazotise the aniline and trap out with CO2 to form benzoic acid, then make an amide.  Probably easiest way is to make the acid chloride with (COCl)2 and then treat with NH3.\n\n2. Bromobenzene -> 1-phenylethanol\nForm phenylmagnesium bromide by treating bromobenzene with magnesium in diethyl ether, and react with ethanal.\n\n3. Butanal -> 1-chloropropane\nMany ways to do this, none of them nice.\n\nReduce butanal to butanol, de-hydrate, perform a reductive oxonolysis to give 1-propanol and then do a chloro-dehydroxylation with SOCl2 or something like that.\n\nAlterantively you could oxidise and do a Barton-Crich de-carboxylation and trap out the radical with NCS, although this method may not be too successful.\n\nHope these quick ideas help.
40972
I believe Theisen AG of Germany produces Chlorine gas (CL2)
488906
The most obvious one is chloroform, CHCl3.\nIt is created by reacting methane with chlorine free radicals.  I think its a UV light thats used to create the radical, but im not certain.\n\nIt can be used as an anaesthetic, administered orally. Whenever you see someone on a film pass out when a hankie is helt to their mouth its meant to have chloroform on it. More recently it has been used more as a solvent by chemistry labs. Although its main use is in the  production of freon, the thing in fridges that help to keep them cold.
46852
I don't understand what you are trying to test or why you are doing the test. But  gasoline is a mixture of hydrocarbons ranging from five to twelve carbon atoms . Most of those hydrocarbons do not resemble benzene in structure. Gasoline has benzene as a minor component. \n\nA better substitute would likely be toluene or xylene since these are both very similar to benzene in structure and only differ by one functional group on the ring of carbon atoms.
561728
Grignard Synthesis of Benzoic Acid\n\n\nPreparation:  McMurry, sections 10.8 and 20.6.\n\nConversion of an organic halide into a Grignard reagent completely transforms the reactive character of the organic compound. Carbon bears partial positive charge when bonded to halogen but partial negative charge when the carbon is bonded to magnesium. The Grignard reagent is a very reactive nucleophile and base. \n\nIn this experiment you will make the Grignard reagent phenyl magnesium bromide; this reagent will then be treated with carbon dioxide to form benzoic acid. The sequence (Equation I) is explained in McMurry Sect 20.6.\n\n\nAs in any work, this experiment may not succeed the first time; be prepared to repeat it from the beginning. On the second try, you should be able to work much more efficiently and with more understanding. \n\n\nProcedure: Obtain a 150 mm piece of magnesium ribbon. Hold one end with forceps and with the other hand remove the residue on the ribbon by scraping it with a spatula, scissors or pliers to obtain a shiny surface. Cut at least 0.12 g of the shiny ribbon into 2-3 mm pieces (do not handle the pieces) and place on a folded piece of paper to obtain the mass on the balance. Transfer the magnesium pieces to the 5 mL conical vial, add the dry spin vane, add one small crystal of iodine and add 300 µL (0.3 mL) of anhydrous ether. Be prepared to add more ether as necessary to maintain the liquid level at a minimum of 300 µL.\n\nAssemble the rest of the apparatus as in Mayo, et al., Fig 3.24. Clamp the apparatus firmly to a stand.\n\nIn the hood, prepare a solution of 510 µL of bromobenzene in 700 µL of anhydrous ether in the 3 mL vial using the delivery pipettes provided. Cap this vial with a polyethylene top. \n\n(*Note:  Be certain the dry ice is ready before you initiate the reaction below.)\n\nDraw half of the bromobenzene solution into the syringe and insert the needle through the polyethylene cap in the Claisen head as in the figure. While stirring the mixture below, add 6-8 drops of the bromobenzene solution. Evidence of reaction is the formation of tiny bubbles. When the reaction has started, add the remainder of the bromobenzene solution slowly over 3-5 min. The temperature should be maintained at about 40 oC to allow gentle refluxing (Mayo, et al., p. 29) of the ether. To the 3 mL vial add an extra 300 µL of ether, then transfer this to the reaction via the syringe. Adjust the total volume to 3 mL with the addition of more anhydrous ether. Reflux the mixture for 10 minutes, then allow the gray-brown solution of the Grignard reagent to cool to room temperature. What do you observe?\n\nThe Dry Ice (at least 1.0 g) is added in small chunks to the Grignard solution. Note the reaction as this is added. To convert the C6H5C(=O)-OMgBr, to benzoic acid (last step, Equation I), use a pipet to VERY SLOWLY add 1 mL of 6 N HCl and again observe the result. Test the aqueous layer with pH paper; it should be acidic. Remove the ether by gently heating the vial for 5 minutes on the steam bath. Cap the vial, mark it and set it in your drawer until the next laboratory period. \n\nPreparation for the 2nd laboratory period:  The benzoic acid has been synthesized, but it must be purified. Water soluble magnesium salts are removed by extracting away the water layer; but, a number of organic side products remain with the benzoic acid.  These are side products of the Grignard reaction; small amounts of benzene are formed (Equation II), unreacted bromobenzene remains, and biphenyl, H5C6-C6H5, is formed from the reaction (Equation III). \n\nThe benzoic acid can be isolated from this mixture by taking advantage of its property as an acid. Only it can dissolve in aqueous NaOH (Equation IV) while the side products remain in the ether. After the ether-soluble side products have been removed, strong acid is again added to reverse this reaction in order to restore the benzoic acid.\n\nRecrystallization of the crude product in
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
782364
You get napalm.\n\nIf you google "gasoline and styrofoam", the first thing that pops up is a short explanation from totse.com which has a TON of other articles about things like this.
450615
Any of the heavy metals, or benzene products would be excellent topics. If you attempt to present a case on a chemical that's too obscure you'll have a difficult time finding enough research/clinical trials to support your claim. Peruse the EPA website to get some other ideas.
596395
Benzene + benzoyl chloride + AlCl3 is one\n\nYou can also do \n\n2 calcium benzoate + LOADS OF HEAT --> benzophenone + CaO + CO2
242072
Mol of benzene is 6.50 g/(78 g/mol) = 0.083 mol. Consequently, a solution of 6.50g of benzene is 160g of CHCl3 is 0.083 mol/0.160 kg or 0.520 molal. The freezing point lowering is thus ΔT = Kfpm, or ΔT = (4.60 °C/m)(0.520 m) = 2.43 °C, and the freezing point is -63.5 °C - 2.43 °C = -65.9 °C.\n\nI'm sure this helps,\nUltimeaciax
575847
Any amine hydrochloride, ammonium chloride, or even hydrochloric acid can be used.  You may need to actually call a company to get more specific information, if they will even tell you.  If you look at MSDSs, you can gleam some information.  \n\nhttp://www.efdsolder.com/lit_msds.htm\n\nYou will see that nonionic organics can be used.  Because they would be bought in bulk, there are no commercial names other than the chemical name.
233314
Any of various halocarbon compounds consisting of carbon, hydrogen, chlorine, and fluorine, once used widely as aerosol propellants and refrigerants. Chlorofluorocarbons are believed to cause depletion of the atmospheric ozone layer.
483391
I'd sure be cautious with any Methylene Chloride!  It is highly volatile and it is a carcinogen.  Nasty stuff!  I would first try a strong detergent and steam.  Steam will loosen a lot of compounds that you wouldn't expect to respond to heat and water alone.\n\nJohnny
1137161
No. It is not flammable but can be a powerful oxidizer.\nNitrous oxide (N2O), also known as laughing gas and is used in dentistry for its anesthetic ability.  However you are more interested in its use as an oxidizer in engines.  The nitrous oxide releases oxygen (O) as it breaks down in the hot combustion chamber provides additional oxygen for combustion which in turn allows more fuel to be burned. More fuel combustion means more power produced. \n\nThis method of boosting power is destructive to reciprocating engines so running your car on N2O may not be such a good idea.\n\nFor more info you can check the site below.
741099
I got your message.  I a little unsure about what you need to know.  I thought you said that you bought this chemical before.  What did you use it for and/or what do you need it for?  If you want more info. on the chemical itself go to your search bar and type in "strychnine hcl powder" and the listed sites will give you all the information that you need.
1141478
I don't know about chloroform but acetone works well