making SO2 is hard even with sulfur candles and sodium meta bi sulfate plus acid. sulfur and H2SO4 is easy to get hold of . i think the reaction is
endothermic so no runaway reaction Hot concentrated sulfuric acid is needed
S +2H2SO4 -----> 2H2O +3SO2
note- i need SO2 to react with MnO2 to make MnSO4 iwas thinking heating MnO2 with sulfur in a H2SO4 slurry
3MnO2 + S +2H2SO4 ------> 2H2O +3MnSO4
.Bedlasky - 23-3-2020 at 08:47
MnO2 reacts with SO2 to form MnS2O6, not MnSO4.
Why is making SO2 by mixing metabisulfite and acid hard? It's very simple and cheap way.rockyit98 - 23-3-2020 at 11:28
[Edited on 23-3-2020 by Bedlasky]CharlieA - 23-3-2020 at 15:48
I'm ignorant of Mn chemistry. However I have several questions which I don't think that some of the posters seem to know.
1. How about balanced equations for each of the 2 reactions? You can write a balanced equation are any reaction, real or imagined, if you follow the
law of conservation of mass.
2. Has anyone heard of structural formulas? isomers? Just a random thought that may not be relevant here.
3. While MnO2 + SO2 = MnSO4 is mathematically correct, it does not say anything about the structures of the compounds involved. There may be 2 or more
structural isomers of MnSO4, and thus 2 or more different chemical substances (I don't know the answer to this).
3. Not all chemical reactions are combination reactions, i.e, A + B = AB. Also if A and/or B is polyatomic, there may well be 2 or more isomers of AB.
Forgive the rants of an old man, but many questions posed in this forum reflect little knowledge of chemistry. I'm not talking of legitimate questions
seeking an answer (after the appropriate literature search, of course), but of questions that purport to be a fact, with no supporting theoretical
reason.
At any rate, it's time for my dinner!
P.S. I guess I'm already going stir-crazy being cooped up while hoping to outlast this COVID-19 crisis. I hope all of our members can avoid this flu
crisis.
[Edited on 3-23-2020 by CharlieA]Boffis - 24-3-2020 at 03:47
At low temperature manganese dithionate MnS2O6 is the main product but if this reaction is carried out in hot solution manganese sulphate is the main
product.Abromination - 24-3-2020 at 12:19
Literally all you do is drip the acid onto metabisulfite, how the hell is that hard?Sigmatropic - 24-3-2020 at 13:15
It needs a p and e addition funnel. Now I don't consider that hard but a starter might?
Same for a sulfur candle, requires a gas washing bottle and a vacuum pump, not particularly unobtainium but not exactly starter equipment either.
So I can see why OP wants a chug-plug-heat kind of reaction/set-up. That being said, sometimes it's just better to get ahold of that p-e addition
funnel. Heptylene - 24-3-2020 at 14:29
Doesn't sodium metabisulfite decompose when heated? (To sodium sulfite and sulfur dioxide) Wikipedia quotes a 150 °C decomposition temperature, but I
haven't tried myself.
Granted a powder isn't the best in a gas generator, it will tend to become airborne, but maybe an interesting alternative for those who don't have
sulfuric acid on hand.Bedlasky - 24-3-2020 at 14:44
PET bottle, hose, sodim metabisulfite, acid - simple SO2 generator. You can heat it on hot water bath to release more SO2 from acid.rockyit98 - 25-3-2020 at 00:01
Sulfur dioxide react with manganese(IV) oxide is 2SO2 + MnO2 → MnS2O6
possible in a neutral to some what basic conditions but we are talking about hot concentrated acidic medium. there is no way of manganese(II)
dithionate formation.
Source: https://chemiday.com/en/reaction/3-1-0-998 https://en.wikipedia.org/wiki/Dithionate says " Strong oxidants oxidise them to sulfates and strong reducing agents reduce them to sulfites and
dithionites.[3] Aqueous solutions of dithionates are quite stable and can be boiled without decomposition"
[Edited on 25-3-2020 by rockyit98]pneumatician - 25-3-2020 at 09:55
