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YT2095
International Hazard
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JEANBERGIAN I rest my case 
\"In a world full of wonders mankind has managed to invent boredom\" - Death
Twinkies don\'t have a shelf life. They have a half-life! -Caine (a friend of mine)
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YT2095
International Hazard
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to Elucidate...
| Quote: | Originally posted by JEANBERGIAN
If I had a cooling sistem up to the job, this would be my pet.Do you know yow many B.Units need to do ,say, 4
ounces? At 70 / 80F ?
Urea is cheap and simple to get. |
reads Alc or Drug induced .
\"In a world full of wonders mankind has managed to invent boredom\" - Death
Twinkies don\'t have a shelf life. They have a half-life! -Caine (a friend of mine)
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12AX7
Post Harlot
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I think the most salient point from almost all those explosions is that excess AN, in the exploding heap, was thrown significantly far and did not
itself detonate. A pretty shitty explosive if a sizable fraction (like, more than half) doesn't explode!
Tim
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S.C. Wack
bibliomaster
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from here
Ammonium nitrate, in solid or molten
form or in solution, is a stable compound
and generally is difficult to explode.
Ammonium nitrate may explode, however,
when exposed to strong shock or to high
temperature under confinement. In a large
quantity of ammonium nitrate, localized areas
of high temperature may be sufficiently confined
by the total quantity to initiate an explosion. The
explosion of a small quantity of ammonium
nitrate in a confined space (e.g., a pipe) may
initiate the explosion of larger quantities (e.g.,
in an associated vessel).
Contaminants may increase the explosion
hazard of ammonium nitrate. Organic materials
generally will make ammonium nitrate
explosions more energetic. Ammonium nitrate
may be sensitized by certain inorganic
contaminants, including chlorides and some
metals, such as chromium, copper, cobalt, and
nickel. As ammonium nitrate solution becomes
more acidic, its stability decreases, and it may
be more likely to explode.
Low density areas, such as bubbles, in molten
ammonium nitrate or solutions, also may
increase the possibility of an explosion and
enhance the propagation of an explosion.
Ammonium nitrate by itself does not burn, but
in contact with other combustible materials, it
increases the fire hazard. It can support and
intensify a fire even in the absence of air. Fires
involving ammonium nitrate can release toxic
nitrogen oxides and ammonia. A fire involving
ammonium nitrate in an enclosed space could
lead to an explosion. Closed containers may
rupture violently when heated.
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Engager
Hazard to Others
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Any soluble salt of ammonia + NaHCO3/Na2CO3, just mix solutions and boil them. That will result in ammonia gas and corresponding salt of sodium, for
example:
Na2CO3 + 2NH4Cl = (boiling) => 2NaCl + 2NH3 + H2O + CO2
Ammonia is dried by passing colunms with KOH and is liquified/freezed in U shape tubing cooled by dry CO2 (dry ice) / acetonе mixture (-90C
temperature could be reached).
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HenningBasse
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can someone help me out with this??
http://www.sciencemadness.org/talk/viewthread.php?tid=7695
is just about making ammonia from urea
thx in advance
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MagicJigPipe
International Hazard
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The bottom line is NH4NO3 is difficult to detonate even with a blasting cap and a booster charge ON PURPOSE. I'm thinking these incidents only happen
with HUGE quantities of NH4NO3 and I believe it presents virtually zero risk to the home experimenter.
"There must be no barriers to freedom of inquiry ... There is no place for dogma in science. The scientist is free, and must be free to ask any
question, to doubt any assertion, to seek for any evidence, to correct any errors. ... We know that the only way to avoid error is to detect it and
that the only way to detect it is to be free to inquire. And we know that as long as men are free to ask what they must, free to say what they think,
free to think what they will, freedom can never be lost, and science can never regress." -J. Robert Oppenheimer
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not_important
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| Quote: | Originally posted by Engager
Any soluble salt of ammonia + NaHCO3/Na2CO3, just mix solutions and boil them. That will result in ammonia gas and corresponding salt of sodium, for
example:
Na2CO3 + 2NH4Cl = (boiling) => 2NaCl + 2NH3 + H2O + CO2
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However using a carbonate leads to the formation of ammonium carbonates and carbamates in the takeoff tubing. For some applications this is not a
problem, a solution of the gases can be considered a solution of ammonium carbonate, as is used in some inorganic analysis. But if the goal is strong
aqueous ammonia, or liquid ammonia, you had best use a hydroxide rather than a carbonate.
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