Post 463311 (https://www.thevespiary.org/talk/index.php?topic=6383.msg46331100#msg46331100)
(Vitus_Verdegast: "More suggestions...", Chemistry Discourse).Post 480352 (https://www.thevespiary.org/talk/index.php?topic=5437.msg48035200#msg48035200)
(Chewbacca: "decomp products", Chemicals & Equipment). However, it seems to be the preferred method to get highly pure disulfates in a controllable way and high yield. I think the first report of that method can be found in Chem. - Ztg., 45.1921;1113-1114, which was a pain in the ass to get from the library and finally the wrong publisher and volume (always fun to get stuff from pre-WWII).Post 462958 (https://www.thevespiary.org/talk/index.php?topic=11772.msg46295800#msg46295800)
(Rhodium: "Na-Acetate + Na-Pyrosulfate -> Acetic Anhydride", Novel Discourse)) should be retried with pyrosulfates prepared this way.Post 246368 (https://www.thevespiary.org/talk/index.php?topic=9447.msg24636800#msg24636800)
(Antoncho: "Re: Nitroalkane Preparation FAQ", Methods Discourse) oleum can be produced by bubbling sulfur trioxide into sulfuric acid.Post 418829 (missing)
(lugh: "Industry", Chemicals & Equipment)Post 58152 (missing)
(terbium: "SO3 from P2O5", Chemistry Discourse) - a bit counter productivePost 259376 (https://www.thevespiary.org/talk/index.php?topic=11885.msg25937600#msg25937600)
(lugh: "Re: Methylene Sulfate", Novel Discourse) - decomposition of ferrous sulphatePatent BP904971 (http://l2.espacenet.com/dips/viewer?PN=BP904971&CY=gb&LG=en&DB=EPD)
Patent DE40696 (http://l2.espacenet.com/dips/viewer?PN=DE40696&CY=gb&LG=en&DB=EPD)
Post 418829 (missing)
(lugh: "Industry", Chemicals & Equipment), or the chamber process, described inPost 428197 (https://www.thevespiary.org/talk/index.php?topic=5131.msg42819700#msg42819700)
(lugh: "Sulfuric Acid by the Chamber Process", Chemicals & Equipment) is to oxidize sulfur dioxide with ozone, producing sulfur trioxide ;) An alternative to burning sulfur for the preparation of sulfur dioxide is to heat sulfur with sulfuric acid, as mentioned inPost 507414 (https://www.thevespiary.org/talk/index.php?topic=5131.msg50741400#msg50741400)
(lugh: "Alternative Route to Sulfur Dioxide", Chemicals & Equipment)Post 441606 (https://www.thevespiary.org/talk/index.php?topic=6651.msg44160600#msg44160600)
(lugh: "Industrial Method", Chemistry Discourse) ;) The article on sulfur trioxide/sulfuric acid from Thorpe's Dictionary of Applied Chemistry:(https://www.thevespiary.org/rhodium/Rhodium/hive/hiveboard/picproxie_imgs/djvu.gif)
Patent US3885024 (http://l2.espacenet.com/dips/viewer?PN=US3885024&CY=gb&LG=en&DB=EPD)
The alchemists' method is starting from FeSO4 hydrate which in our days is very cheap and is sold in every agricultural chemicals shop. In my country it is called "green stone". Green FeSO4.xH2O is allowed to stay for several days/weeks on air when it is oxydized to the pale-yellow Fe(OH)SO4. Scatter it on a newspaper, place in a not very dry place and wait. The so obtained Fe(OH)SO4 is pyrolized at 700 deg.C and it decomposes in Fe2O3 and oleum H2S2O7. The problem is that you'll need a ceramic, or better porcelaine, alambic.
My problem here is that I cant get this balanced even when correcting the Fe(OH)SO4 to the correct Fe(OH)2SO4 what is the real product of oxidation of ferrous sulfate in moist air.
From the Wikipedia:
".... in a technique similar to the original alchemical processes. Pyrite (iron disulfide, FeS2) was heated in air to yield ferrous sulfate, FeSO4, which was oxidzied by further heating in air to form ferric sulfate, Fe2(SO4)3, which when heated to 480°C decomposed to ferric oxide (Fe2O3) and sulfur trioxide, which could be passed through water to yield sulfuric acid in any concentration."
(emphasis added by me)
Looks much better to me - more balanced so to say....
ORG ;)
(https://www.thevespiary.org/rhodium/Rhodium/hive/hiveboard/picproxie_imgs/djvu.gif)