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redox
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Quote: Originally posted by smaerd  | Now I'm a pretty dumb dude but wikipedia shows something interesting on the AlBr3 page.
(DRY) 2Al + 3Br2 ==> Al2Br6
(DRY) 2Al2Br6 + 3CCl4 =heat=> 4AlCl3 + 3CBr4
Now the actual feasibility of preparing CCl4 from chloroform/dichloromethane and Cl2 gas I'm not really aware. This is the only way around the furnace
I could find.
Drying Br2 is a pretty unnerving task without a fume-hood/blast shield.
Will this actually work? I don't know... Also there is like 10 AlCl3 threads, this is getting out of hand... Wish I could find a supplier that didn't
only sell it by the kg(and overseas).
[Edited on 9-8-2011 by smaerd] |
When I get back from vacation in a couple weeks, I will attempt this, as I have both CCl4 and AlBr3. 
My quite small but growing Youtube Channel: http://www.youtube.com/user/RealChemLabs
Newest video: Synthesis of Chloroform
The difference between chemists and chemical engineers: Chemists use test tubes, chemical engineers use buckets. |
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Mildronate
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But why you need it? You can use alBr instead of AlCl3?
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Bitburger
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It's pretty easy to make AlBr3, but once you made it under reflux with toluene as a solvent you should see that clouds will form immediately when
exposed to air. It's caused by the reaction of this substance with water in the air, I think that AlBr3.6H2O might be formed in the first phase.
I choose toluene because both bromine and AlBr3 are soluble in it. However, the mixture have a brown colour.
I can do two things: a one pot reaction without isolating AlBr3
OR
Try to isolate AlBr3 by destillation.
I prefer the first one.
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AlBr3 forms yellow-white hygroscopic monoclinic crystalls
mp.97.5°C
bp.255°C
Ref; Handbook of Chemistry and physics 2010-2011
Good to be wrong
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MeSynth
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I just found a listing on ebay for this chemical.
http://www.ebay.com/itm/Aluminium-chloride-anhydrous-100g-98...
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