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Author: Subject: CuSO4 ---------> SO3
my nootloss
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[*] posted on 23-5-2005 at 14:11
CuSO4 ---------> SO3


Would any one know how to get CuSO4 to H2SO4?


thanks

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Hey guys sorry about this post I was not in my right mind, I want SO3, not H2SO4. See I am going to put the SO3 in H2O and then make H2SO4. Sorry about the other posts but I have not found any that have SO3 with copper2 sulfate

[Edited on 24-5-2005 by my nootloss]

[Edited on 24-5-2005 by my nootloss]
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tom haggen
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[*] posted on 23-5-2005 at 14:36


Oh oh i know i know

CuSO4 + 2HCl --> H2SO4 + CuCl2

Check it out my gen chem is paying off I can finally answer posts.




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evilgecko
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[*] posted on 23-5-2005 at 14:54


Or you can use the electrolysis method of CuSO4. I believe you can use carbon electrodes.

CuSO4 + H20 -> H2SO4 + CuO
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The_Davster
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[*] posted on 23-5-2005 at 15:05


There has already been a huge thread on this you do know there is a little button to push when you want to find info on a topic that has been discussed before, the SEARCH button
https://sciencemadness.org/talk/viewthread.php?tid=1739
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ChemPhile
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[*] posted on 23-5-2005 at 18:47


CuSO4+H2S-->CuS(沉淀)+H2SO4
anyone know Chinese
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BromicAcid
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[*] posted on 23-5-2005 at 18:53


Maybe it just means solid? It would work but if the concentration got too high it would drive the equilibrium in the other direction, there are other methods too that form insoluble salts, of course if you wanted to avoid doing this in soluiton maybe you could get away with the method the Rhodium page used to make anhydrous formic acid from lead formate, passing H<sub>2</sub>S through lead formate in a verticle tube, the prepared formic acid dripping down. Of course I am very weary of working with H<sub>2</sub>S, expecially after my last experience with it, and it is one of the few chemicals I recomend against using in nearly all cases.

Yes, the thread Rogue Chemist links to is also relevent for copper sulfate and there are several other threads around here on sulfates converting to sulfuric acid, I know at least on describing the pyrolysis of copper sulfate and the subsequent absorption in water of the SO<sub>3</sub> formed.




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12AX7
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[*] posted on 24-5-2005 at 01:23


That being the original method to make concentrated acid.

Iron sulfate has the lowest decomposition temperature, I think. You could do it in glass.

Tim
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MadHatter
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[*] posted on 24-5-2005 at 02:20
Iron Sulphate


Iron(III) Sulphate decomposes at 480 C.
Iron(II) Sulphate decomposes > 300 C.
According to the CRC.




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