DFliyerz
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Interacting Compounds with Ozone
I'm aware that ozone is an extremely powerful oxidizer, and possible to create, which begs the question; how would one go about combining a compound
with ozone? Simply put the two reactants in a sealed container together?
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mayko
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Very carefully; ozonides are unstable explosives comparable to organic peroxides.
More: ozonolysis
al-khemie is not a terrorist organization
"Chemicals, chemicals... I need chemicals!" - George Hayduke
"Wubbalubba dub-dub!" - Rick Sanchez
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franklyn
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It's best just to follow a written process. Saturated ( no double bonds present ) Chlorocarbons or Fluorocarbons
( Freons ) are used for a solvent in some proceedures. This is mainly for safety when separating the product. O3 will oxidize almost anything but
organic ozonide products are dangerously sensitive. The bigger problem is working at the cryogenic temperarues required in many cases. At room
temperature, the gathered amount will degrade very quickly, providing it has not spontaneously exploded.
http://ww2.valdosta.edu/~tmanning/research/ozone
Attachment: Inorganic Ozonides.pdf (138kB)
This file has been downloaded 481 times
Attachment: Inorganic Ozonides J.chem.ed.pdf (538kB)
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Attachment: Safer ozonolysis reactions- A compilation of laboratory experience.pdf (192kB)
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Attachment: Ozone+Amine=Nitro.pdf (455kB)
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Attachment: Ozonation of Naphthalene in Water.pdf (337kB)
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franklyn
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My interest in these compounds is as explosives , but there is a rich ever widening general application of
ozonolysis as an oxidant reagent.
http://www.ozonolysis.com/ozonolysis/web.nsf/wp/Attachment%2...
- Ozonolysis of Bicyclic Bridged 1,2-Dioxines
http://digital.library.adelaide.edu.au/dspace/bitstream/2440...
Synthesis of five- and six-membered cyclic organic peroxides
www.beilstein-journals.org/bjoc/content/pdf/1860-5397-10-6.p...
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Shob dhillon
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I'm interested in seeing if I can make percarboxylic acids from reacting Ozone with the corresponding carboxylic acid but
I don't know what reaction conditions and setup are required, but I think that bubbling Ozone into chilled 99.7% pure acetic acid might generate the
peroxyacetic acid in some percentage. I know that peroxy acids can be produced by adding concentrated (~70%) Hydrogen peroxide to either the acid
anhydride or carboxylic acid, but the hazards and very scarcity of that stuff make it impossible for my amateur use.
http://www.prepchem.com/synthesis-peracetic-acid/
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Tsjerk
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I think ozone won't form the peroxy acid, but oxidize the acid or form the probably very explosive ozonide variant of the peroxy acid.
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Rhodanide
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Be careful...
And don't condense it! It's been reported to "Decompose explosively upon rapid heating to boiling point".
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Tsjerk
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Always cool with a boiling point of -112!
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Rhodanide
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I wouldn't go as far to say that LO3 is "Chill", though... 
...
Ok, that was disgraceful, I'll leave.
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PHILOU Zrealone
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You have to be prepared for a severe blast:
-Peracids in high concentration are very sensitive explosive (to friction, shock and heat)...especially those with a closer to 0 oxygen balance like
performic acid (HCO3H performs very wel with its perfect OB of zero) and like
peracetic acid.
-Ozon is explosive on its own.
-Condensed phase ozon and fuel must be like LOX (liquid oxygen) explosives but worst.
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
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Melgar
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Ozone is especially selective for C=C double bonds, and will typically replace each side's double bond to a C with a double bond to an O, splitting
the molecule in a reaction termed "ozonolysis". Normally, this has to be done at very low temperatures, and even then can result in explosions.
However, if you want to perform a much safer version of the ozonolysis reaction, you can use the reaction described here with terminal alkenes
(alkenes that terminate in a double-bonded carbon):
http://www.sciencemadness.org/talk/files.php?pid=201968&...
IIRC, ozonides are only formed when ozone adds across double bonds, otherwise you just get typical partial oxidation products for that compound.
[Edited on 1/12/17 by Melgar]
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