D S2 A - 7-1-2010 at 08:59
I was wondering about a method to produce sulphur trioxide without demanding great deals of heat. Reading A Comprehensive Treatise on Inorganic
and Theoretical Chemistry 8 I found something very interresting about it. Let's see what is in page 102.
According to J. B. Senderens, the reaction with sulphur when boiled with cuprous and cupric oxides, or with silver
oxide, can be symbolized: 4Ag2O + 4S ~> 3Ag2S + Ag2SO4; and 3Ag2SO4 + 4S ~> 3Ag2S + 4 SO3.
The silver may be recovered for further use. Although, the book seems to not claim the temperature that the sulphur trioxide releases, but it still
looks a nice procedure for small batches of sulphur trioxide.
So, any ideas? How to make it work?
Best regards, Dúlio.
[Edited on 7-1-2010 by D S2 A]
[Edited on 7-1-2010 by D S2 A]
DJF90 - 7-1-2010 at 09:12
Does it give any reference information other than "according to J. B. Senderens..."? If it does, paste it here and I'll get the relevant paper, which
should hopefully have the experimental details.
D S2 A - 7-1-2010 at 09:20
The came from here: [ http://library.sciencemadness.org/library/books/Mellor_ACTIT... ]. That is the best I can show you now, DJF90.
Best regards, Dúlio.
[Edited on 7-1-2010 by D S2 A]
[Edited on 7-1-2010 by D S2 A]
Sulphur trioxide from lead!
D S2 A - 7-1-2010 at 09:54
In the same book, I also find that reaction: Pb + 6SO2 ~> PbS + S + 2SO3.
Sulphur dioxide is pretty easy to make and lead is easily available. How could someone produce sulphur trioxide by that way? I suppose it would demand
a certain amount of heat...
Any ideas?
Best regards, Dúlio.
hissingnoise - 7-1-2010 at 10:21
Dúlio, all the usual methods of preparing oleum have been attempted by members on this forum with the possible exception of electrolysis of
concentrated H2SO4.
If the electrolytic method does indeed work it would be relatively painless by comparison with sulphate decomposition methods.
D S2 A - 7-1-2010 at 10:24
I am new here, therefore I am not very familiar with the site yet. Would mind send me the links of the best procedures discussed here, hissingnoise?
Picric-A - 7-1-2010 at 11:43
Try here :
http://www.sciencemadness.org/talk/viewthread.php?tid=727
D S2 A - 7-1-2010 at 11:49
Useful link, Picric-A.
Best regards, Dúlio.
Taoiseach - 8-1-2010 at 02:00
You should look into antimony sulphate as well, there's a reference somewhere according to which it decomposes into SO3 at a moderate temperature. The
tricky part will be to completely dry it as it hydrolyzes easily, just like most antimony salts.
Unlike silver, antimony can be bought on Ebay for decent prices and in kg quantities.
[Edited on 8-1-2010 by Taoiseach]
D S2 A - 8-1-2010 at 07:04
Thank you for the hint, Taoiseach. Unfortunately antimony is not easy available here. I know silver nitrate is expensive but its silver mais be
recovered. I also suppose that silver would work better due its high atomic radius and relatively low energetic demands on reactions.
So am I right?
Best regards, Dúlio.