budullewraagh

governmental restrictions

you could add loads of hydrogen to this layer, resulting in ethane and hydrogen chloride. but then youd have acidic water. at least you'd be left a fossil fuel:\

i love organic chemistry. i dont find that to be scary, jdurg, i find that to be absolutely wonderful

i think the point is to make the haloform; the carbonic acid is just a byproduct...

do you need to actually perform the experiment or do you need to explain it?

i dont see how enflurane can be what you call it. 2-chloro-1,12-trifluoroethyl difluoromethyl ether. you can't have a 12th carbon if you have a methyl ethyl ether, which happens to have only 3 carbon...

no, i said "-OCOO-" (see above) which covers the structure of a carbonate (note the - before the first O and after the last O).

we could get maybe enough to last a day. that's it.

wow sorry i wrote that incorrectly: -OCOO- with sodium cations it would be the dibasic salt of carbonic acid

chloroform isnt used so much anymore because it can kill. it is produced by a haloform reaction, a form of nucleophilic substitution: R-COCH3+3MOCl-->R-COCCl3+3MOH R-COCCl3+3MOH-->R-COO-+M++CHCl3 also, R-COCH3+3X2+4MOH-->R-COO-+M++CHX3+3X-+3H2O i've been studying for my orgo I class btw, this reminds me. for home production of chloroform with minimal other waste products: since you need a methyl ketone, why not use acetone? it is a doubly methylated ketone: H3CCOCH3 thus, if one were to use 6MOCl, would one not achieve twice the chloroform and no R product? H3CCOCH3+6NaOCl-->Cl3CCOCCl3+6NaOH-->2Na+ -OOCOO- +2CHCl3

yes, if the anion is HSO4- or SO4-2 ionization is a reaction...

well the fact of the matter is that, for all intents and purposes, there is really nothing there

yes, you could collect and dissolve your nitric anhydride, but again, it's bloody scary. if you HAVE to do this, use PTFE tubing; just about anything else will be oxidized h2so4 at high concs will fume the anhydride, SO3, a white gas. it makes you choke. i had a fun experience with that once.

akcapr, if you do that reaction cold with not very conc sulfuric acid, you could conceivably avoid the nitric anhydride problem. still, it's tricky and you will be left with a very impure product. raivo, nitric anhydride is just as bad as i described

ive never been exposed to that much. it would, im sure. i got pretty buzzed during that ap bio lab.

you probably wouldnt...

i happen to really like the smell and the effects of diethyl ether

no, diethyl ether is the kind you're thinking of, akcapr

it's FeSO4 complexed with NH3

it's scary and it will cause permanent respiratory failure. if you survive the initial pulmonary edema, 10 years from now you'll feel it coming back; you'll feel asthmatic, you'll be susceptible to bronchitis and pneumonia, etc. need i say more?

so N2+O2-->2NO, which oxidizes immediately to NO2/N2O4 with the majority as N2O4. out of curiosity, do you know what the SO2 comes from? surely not S(s) or H2S...

what salt are we considering? if it's sulfate/bisulfate, there will be less ionization by the sulfuric acid. btw, H2SO4 almost always ionizes to H+ and HSO4-. very little of that HSO4- ionizes further to H+ and SO4-2.

sometimes it is. ex: Al+Fe2O3-->Al2O3+Fe sometimes it isnt ex: 2LiCl+RbF-->RbCl+LiF akcapr, im almost positive you had a fairly acidic solution. in the future use glass and by all means, measure your reactants!

ok, did you measure the amounts of ammonia and sulfuric acid before? if you have a 1:1 ratio, you have the bisulfate. if you have a 2:1 ratio you have the sulfate. what sort of ammonia and sulfuric did you use? store brand? did you titrate? i think your solution had a displacement reaction with the pan. try again and use indicators. test for ammonia gas being released.

wait, where do the oxides of nitrogen come from? i know there is the dioxide of sulfur...