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Carboxyl amines
The formation of the amines would actually be the result of an acid base reaction. The ammonium pero ... |
20-5-2002 at 19:43
by: madscientist |
Carboxyl amines
I have been intrigued for a while with the idea of carboxylic amines. They would be produced by the ... |
20-5-2002 at 19:42
by: madscientist |
Nitroxamide
I am thinking that nitroxamide, NH2OCCONHNO2 would make a decent energetic material. I postulate tha ... |
20-5-2002 at 19:39
by: madscientist |
Nitrated sugars
Nitrated sucrose is very annoying to dry; it takes days to get the water content down to a reasonabl ... |
20-5-2002 at 19:32
by: madscientist |
Nitrated sugars
I prepared a small amount of nitrated sucrose recently. The procedure that I followed was:
1) Pla ... |
20-5-2002 at 19:30
by: madscientist |
Preparation of sulfur
You could react the CaS with H2O2, much simpler.
8CaS + 8H2O2 --> 8Ca(OH)2 + S8 |
20-5-2002 at 19:12
by: madscientist |
Extracting magnesium metal from its salts
Sorry, but the answer is no to both questions. Somehow this slipped my mind though: you can also use ... |
20-5-2002 at 19:08
by: madscientist |
Extracting magnesium metal from its salts
I can't think of a less dangerous gas to use. The only alternative to carbon monoxide that occurs to ... |
20-5-2002 at 19:07
by: madscientist |
Extracting magnesium metal from its salts
CO2 cannot be used instead of CO; the CO2 will oxidize the magnesium metal.
Mg + CO2 + heat --> M ... |
20-5-2002 at 19:06
by: madscientist |
Extracting magnesium metal from its salts
Check to see if the lead electrodes are corroded. If they are not corroded, then the reason for the ... |
20-5-2002 at 19:05
by: madscientist |
Extracting magnesium metal from its salts
No chlorine gas was given off at all? Perhaps the lead is reacting with the chlorine forming PbCl2; ... |
20-5-2002 at 19:04
by: madscientist |
Nitrating with NH4NO3 and HCl
Nope. Here's why: hexamine is a basic organic compound, it forms salts with acids. Hexamine is (CH2) ... |
20-5-2002 at 18:49
by: madscientist |
Perchloric acid preparation
I really can't think of a simple solution to the inert-gas problem. Most of the time, the gas is goi ... |
20-5-2002 at 18:47
by: madscientist |
Perchloric acid preparation
Oh, by the way, you can produce chlorates by heating an aqueous solution of hypochlorites.
3NaOCl ... |
20-5-2002 at 18:46
by: madscientist |
Perchloric acid preparation
Intriguing, thanks for that link!
I still think this reaction would occur:
2ClO2 + H2O --> HCl ... |
20-5-2002 at 18:46
by: madscientist |
Perchloric acid preparation
Yes, there are much easier ways. Hydrochloric acid will react with various strong oxidizers to liber ... |
20-5-2002 at 18:45
by: madscientist |
Perchloric acid preparation
Unfortunately, production of chlorine oxides is far more complex than that. It is possible to easily ... |
20-5-2002 at 18:43
by: madscientist |
Ammonium permanganate preparation
Ammonium permanganate, contrary to popular belief, is actually a relatively stable compound (althoug ... |
20-5-2002 at 18:32
by: madscientist |
Acetic anhydride preparation
I haven't worried about my experiment, considering that what acetaldehyde I have is either collected ... |
20-5-2002 at 18:09
by: madscientist |
Acetic anhydride preparation
es, I remember a thread that I started at The Forum a while back, "Holy Grail Oxidizer"? That includ ... |
20-5-2002 at 18:08
by: madscientist |
Acetic anhydride preparation
Thanks for reminding me of that... I believe that is the ketene process. |
20-5-2002 at 18:04
by: madscientist |
Acetic anhydride preparation
I'm theorizing that concentrated acetic acid could be dehydrated to acetic anhydride by mixing with ... |
20-5-2002 at 18:03
by: madscientist |
Hydrofluoric acid
Hrm, strange... all I can think of for explanations are:
1) The glass might not contain enough si ... |
20-5-2002 at 17:36
by: madscientist |
Reducing organic peroxides.
How about reducing organic peroxides with phosphites or sulfites? If that doesn't work, is there any ... |
20-5-2002 at 17:25
by: madscientist |
Reducing organic peroxides.
[quote]-CH2-NO2 <-> -CH2-O-N=O
-CH2-O-N=O + O --> -CH2-O-NO2[/quote]
Just how would one carry ou ... |
20-5-2002 at 17:25
by: madscientist |
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