SpiffyVision
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HexaChloroEthane Synthesis?
I've been looking into the possible synthesis of Hexachloroethane for pyrotechnical use (smoke). There is not a lot of information available on
the topic, I've searched E&W, rec.pyro, and this place, no luck at all. I was wondering if some could possibly point me in the correct
direction, or perhaps a suggestion on its manufacture.
Thanks in advance.
All your base are belong to who?
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Pyrovus
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My suggestion would be to use the Kolbe reaction. Starting from a sodium or potassium or whatever salt of trichloroacetic acid, electrolysis would
yeild hexachloroethane at the anode as follows:
CCl3COO- -> CCl3COO. +e-
This radical decomposes:
CCl3COO -> CCl3. +CO2
The two carbon trichloride radicals then combine to form hexachloroethane:
2CCl3 -> C2Cl6
Trichloroacetic acid can be formed by reacting acetic acid with chlorine. There's a detailed synthesis for chloroacetic acid, which can also be
used for trichloroacetic acid at http://www.roguesci.org/megalomania/synth/synthesis2.html#ch...
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Polverone
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From Ullman's Encyclopedia of Industrial Chemistry:
| Quote: | Limited industrial uses of hexachloroethane do not justify large-scale production processes.
A primary source for hexachloroethane is from the production of tetrachloroethylene and carbon tetrachloride by chlorinolysis of hydrocarbons and
chlorinated hydrocarbon residues (see page 79 Tetrachloroethylene by Chlorination of Hydrocarbons and Chlorinated Hydrocarbons ). It can be separated
from the residues by distillation and fractionated crystallization.
For the intentional production of hexachloroethane, tetrachloroethylene is chlorinated batchwise in presence of iron chloride. The hexachloroethane
crystallizes from the mother liquor and is isolated. The mother liquor is recycled and again chlorinated [322].
The photochemical chlorination of tetrachloroethylene is performed similarily [323]. |
This is within the reach of a determined amateur, since tetrachloroethylene (aka perchloroethylene) is a fairly common solvent, but gaseous chlorine
isn't much fun to work with.
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chemoleo
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are there other things you can do with C2Cl6 other than burning it? I mean, it isn't a solvent (MP 187 deg C) or anything... so what could it be
used for?
Never Stop to Begin, and Never Begin to Stop...
Tolerance is good. But not with the intolerant! (Wilhelm Busch)
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AngelEyes
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might make a good thermite (of sorts) mix with Aluminium....I read somewhere that CCl<sub>4</sub> also goes up well with Al...
but I guess that is still burning it.
[Edited on 22-1-2004 by AngelEyes]
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Theoretic
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Maybe addition of hydrogen chloride to cyanogen (addition across the triple bind) will help... 
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BromicAcid
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| Quote: |
I mean, it isn't a solvent (MP 187 deg C) or anything...
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At its melting point it rapidly sublimes. It might do good under reduced pressure but I've yet to test this.
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guaguanco
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| Quote: | Originally posted by Theoretic
Maybe addition of hydrogen chloride to cyanogen (addition across the triple bind) will help... |
Or not.
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