Theoretic
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High-t (useful) ion exchange
Would this work:
6NaCl+Al2O3=>2AlCl3+3Na20
You see, the products would be useful(AlCl3 could be hydrolysed to give HCl vapour).
If it works, it should be very exothermic(the only driving factor would be the formation of volatile AlCl3) due to the difference in lattice energies
of the reactants and the products.
[Edited on 23-7-2003 by Theoretic]
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BASF
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I recall that Al2O3 has a V E R Y high melting point, and i think adding other chlorides like CaCl2(eutectic mixture, as applied in the down-cell for
melt electrolysis) to lower the melting point would not help much.
Al2O3 is the compound in the heat-resistant tiles of the space shuttle for reentrance in the atmosphere.
But i have to admit the basic idea behind is very attractive...
Possibly another combination of salts would be successful?
HLR
[Edited on 23-7-2003 by BASF]
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Theoretic
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Al2O3 needn't melt, it could be a semi-solid-state reaction - NaCl melts at 800C.
Or maybe not even that temperature is needed - I know of several completely solid-state ion-exchange reactions.
Cyanide preparation (many methods) is also a solid-state reaction.
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BASF
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Cool. Maybe you have a link about that?
But what exactly is semi-solid-state reaction? - Does it mean only one of the reactants has to be liquid?
[Edited on 29-7-2003 by BASF]
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Theoretic
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Yes, that's one reactant solid and one liquid (Edit: or gas). A link? No, I coined the term myself -  .
[Edited on 31-7-2003 by Theoretic]
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Iv4
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I'll give this a shot
How pure will the allamunium oxide have to be?I got some salt that I'm quite sure is not iodized(had hell finding it too).
I'm hoping to make the alamunium oxide by heating/cooling repeatedly.
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Theoretic
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You don't need especially pure Al2O3. I think anything with a content of Al2O3 will do (as long as you don't mind the purity of the
products). So don't bother with the non-iodized salt, I think.
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kryss
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Your reaction is the reverse of a neutalisation rxn , reactants strongly favoured over products.
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