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Crypto
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CuCl2 + Al in solvents other than water
Aluminium reacts with an aqueous solution of CuCl2 to form hydrated AlCl3. What if copper chloride was dissolved in methanol or acetone. Would react
in a similar manner?
[Edited on 23-12-2013 by Crypto]
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TheChemiKid
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This would still react, but the aluminum chloride formed would be less hydrated (If the copper chloride was anhydrous, the aluminum chloride would be
anhydrous. If the copper chloride was hydrated, the aluminum chloride would be that hydrated.)
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bismuthate
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But the reaction of the to usualy involves water (thus the evolution of hydrogen) I believe. So wouldn't reacting the in an anhydrous enviorment
change the reaction its self?
[Edited on 23-12-2013 by bismuthate]
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TheChemiKid
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I think the reaction would go as follows:
3CuCl2.2H2O + 2Al => AlCl3.6H2O + 2AlCl3 + 3Cu
AlCl3.6H2O + 2AlCl3 <=> 2AlCl3.3H2O
Or with anhydrous CuCl:
3CuCl2 + 2Al => 2AlCl3 + 3Cu
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bismuthate
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I dont actualy know how the reaction reaction proceeds but that couldn't be it because it doesn't evolve H2
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Crypto
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Does it really evolve hydrogen? That's a displacement reaction and water serves only as a solvent.
[Edited on 23-12-2013 by Crypto]
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bismuthate
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It does. It's more complex than it seems.
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TheChemiKid
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IIRC, Hydrogen is not evolved, only water.
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bismuthate
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Well the gas is flammable so I would think it's H2.
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TheChemiKid
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Are you sure the gas is flammable? If it is, I am intrigued.
I think that if hydrogen was produced, it would be by the reaction of aluminum and water. Maybe the high temperatures would get to the point when a
sizable amount of hydrogen could actually be produced.
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bismuthate
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That was the conclusion I came to but then I wondered where the Al(OH)3 went. My theory is that it reacts with CuCl to form Cu(OH)2 which then
decomposes to CuO. Although I've only seen a video of it being lit on fire (I can't seem to find it) so I'll need to test it myself.
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TheChemiKid
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Ok, I'll do the same when I am back from vacation.
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bismuthate
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well I just got back from the lab and the results are in. The bubbles formed by the reaction where flammable yet the vapors where not, thus leading me
to believe that both H2 and H2O are formed. If my theory is correct I'd better make a new copper sample using Zn. Speaking of which when Zn reacts
with CuSO4 does that release H2 because the reaction doesn't produce enough heat to boil water? If so I wonder how.
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WGTR
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I think you might be interested in this reference.
It should lead to a page 55 of The Chemical News and Journal of Physical Science, Volume 76.
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Galinstan
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The reaction is between the (CuCl4)2- which removes the aluminium oxide coating and a simple displacement reaction occurs, the hydrogen gas that is
evolved is simply due to the aluminium reacting with the water forming aluminium hydroxide and hydrogen.
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bismuthate
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Tis what I concluded, but now I wonder why gas is evolved (I presume H2) in the reaction between CuSO4 and Zn?
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TheChemiKid
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I think zinc can also react with water at high temperatures to form zinc hydroxide and hydrogen.
I can't remember where I saw this, but I know that when zinc is hot enough, it will react with water. I think the reaction probably just reaches the
temperature that can have the zinc react with water.
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bismuthate
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I don't believe that that is what's happening (the reaction doesn't get very not at all). Heres a better example; why is gass released when AgNO3
reacts with Cu?
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Crypto
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| Quote: |
The reaction is between the (CuCl4)2- which removes the aluminium oxide coating and a simple displacement reaction occurs, the hydrogen gas that is
evolved is simply due to the aluminium reacting with the water forming aluminium hydroxide and hydrogen. |
So would doing the reaction in methanol lead to the formation of aluminium methoxide? What about reacting it in acetone?
[Edited on 23-12-2013 by Crypto]
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TheChemiKid
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Hmm... Maybe, I don't know whether that would work. I don't know what will happen with acetone, I will check that out.
EDIT: Alkali, Alkaline-Earth, and some other reactive metals (Including Zinc) will react with acetone to form Pinacol Alcohols upon neutralization.
[Edited on 12-23-2013 by TheChemiKid]
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WGTR
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I've done some basic reductions with combinations of zinc and copper. The reactions are very interesting, and very old:
The Copper-Zinc Couple
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TheChemiKid
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Can you please give me some examples?
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Random
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This could actually mean that anhydrous CuCl2 in very small amount could remove protective layer of Al and make it react with anhydrous ethanol to
produce Aluminum ethoxide.
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TheChemiKid
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How could this be separated from the aluminum chloride?
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WGTR
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Is the link in this post not working?
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