chlorosulfonation of acetanilide
133216
Search http://www.scirus.com/srsapp/
645855
1)\nSodium Sulfate (Na2SO4) will break into ions in solution,\nNa2SO4 (s) --H2O--> 2 Na+1 (aq) + SO4-1 (aq)\nFor every 1 mole of Na2SO4 dissolved, 3 moles of ions are formed.  If the concentration of Na2SO4 is 1.15 mol/Liter, then the ion concentration must be 3 times as much, 3.45 mol/Liter.\n\n2)\nTlCl3 is an ionic compound which when dissolved in water will break into ions since Chloride compounds are generally soluble,\nTlCl3 (s) --H2O--> Tl+3 (aq) + 3Cl- (aq)\n\nC2H5OH, otherwise known as ethanol, will easily dissolve (easily mincible) in water, but will not break into ions (as it is not an ionic compound).\n\nFe2(CO3)3 (although it is an ionic compound) in considered insoluble in water.  Carbonates in generally are considered insoluble unless they are bonded with a group 1 element or the Ammonium ion.\n\n3)\n.356 mol/Liter HCl means that for every 1 Liter of solution, there are .356 moles of HCl dissolved in it.\nMolarity  = moles / Liter --> moles  = Molarity * Liters\nSo if you originally had a 6.5 M solution with a volume of .0572 Liters, you originally had .3718 moles of HCl.\n\n.356 M = .3718 moles HCl / x Liters\nx Liters = .3718 moles / .1.044 Liters.\n\nSo if then old volume was 57.2 mL and the new volume should be 1044 mL, then 986.8 mL shoudl be added to solution.
456842
One needs toluene and concentrated nitric and sulfuric acids, plus "fuming" sulfuric acid (H2SO4 + SO3). As the reaction proceeds, the first nitro groups usually go on either in the position next to the -CH3 (2-, ortho) or diametrically opposite (4-, para). All three mostly end up in the 2-, 4-, and 6-positions. The operator nitrates in three stages, with the temperature raised gradually during the three stages from 35degC to 110degC. However, there is also formation of small amounts of the 2,3,4- and 2,4,5-trinitro compounds. These unsymmetrical isomers make the product dangerously shock-sensitive to handle. The crude product is therefore stirred with 15% aqueous sodium sulfite solution at 100degC. This treatment converts the two impurities to sulfonic acids, which are water soluble and poured away from the oily product in the water.
374337
Cl2 + 2 KI → I2 + 2 KCl
459512
2Al + 3*(CuO) -> Al2O3 + 3*Cu\n\nI2 + 2*(Na2S2O3) -> 2*(NaI) + Na2S4O6\n\nI2 + 5*(Cl2) -> 2*(ICl5)
209188
C4H9OH + 6O2 --> 4CO2 + 5H2O
457360
CuS + H2SO4 ===> H2S + CuSO4
441596
This is a addition-elimination reaction (http://www.chem.ucalgary.ca/courses/351/Carey/Ch23/ch23-3-3.html). can be accelerated by lewis acids.
353554
NaOH + NaH2PO4 ===> Na2HPO4 + H2O\n\nH2S + 2KOH ===> K2S + 2H2O\n\n(NH4)2SO4 + 2KOH ===> 2NH3 + K2SO4 + 2H2O\n\nSO2 + Ca(OH)2 ===> CaSO3 + H2O\n\nIn the above equation, further oxidation in air could occur by\n\n2CaSO3 + O2 ===> 2CaSO4
443242
Here is a good guide\n\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Stoichiometry/Limiting-Reagent.html
468915
Theoretically this would yield H2SO4, sulphuric acid (c).\n\nIn praxis, SO3 doesn't dissolve well in water and is prone to dissociate into SO2 and 1/2 O2, which then may form sulphurous acid H2SO3 which in turn will re-oxidize to H2SO4.
487564
Al2S3 + 6H2O -> 2Al(OH)3 + 3H2S\n\nP4O10 + 6H2O -> 4H3PO4\n\n\nShould be right.
498999
C6H6O + 7O2 yields 3H2O + 6CO2
482242
Cu2S + 12HNO3 -> Cu(NO3)2 + CuSO4 + 10NO2 + 6H2O\n\nThere you go.
167487
H2 + Cl2 -> 2HCl\n2Ag + H2S -> Ag2S + H2 \nCH4 + 2O2 -> CO2 + 2H2O\n2HgO -> 2Hg + O2\n3Fe + 4H2O -> Fe3O4 + 4H2
432273
1. sodium hypochlorite\n2. hydrogen chloride\n3. concentrated sulphuric acid\n4. oxidising it, for example with potassium manganate(VII).\n\nIf you've done the other 96, well done!
254995
My father manufactured the active ingredient in agent orange,(C-5,6), at Hooker Chemical's Montague Michigan plant for the duration of the Vietnam War. The process was so volatile and so toxic that it had to be manufactured on a seven story wall-less superstructure in the middle of a 160 acre field. All of the production was then loaded on railway tankcars for shippment to Dow Chemical of Midland Mi.for addition of solvents and packaging for shipment to the military. At the close of the war, the superstructure was dismantled, and it, and all associated equipment, tools etc. were buried in a huge clay lined disposal pit on the site. The site remains a Toxic hot spot to this day and all of the surrounding neighborhood has water piped into them as the groundwater is highly contaminated. From '82-'93 my father ran a chlorine plant's maintainence department on the persian gulf, about 25 kliks from Kuwait City in Saudi. In 1997 he fell ill with the small cell cancer that has become consistent, though unrecognized by our government, as due to exposure to AO or its components. I know this as I was a service officer for the Am Legion Post here in my  town, and have seen the wreckage that this stuff left in its wake. I am an Non Combatant, US Navy, Vietnam Era vet, ( Commonly refferred to as a "rear echelon puke" ), who salutes and thanks you for your service. Hope you are well, and look forward to your Photo posts as you are quite knowledgeable on the subject. God Bless, Jed