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Author: Subject: Sulphur dioxide from sulphuric acid
idrbur
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[*] posted on 17-4-2017 at 06:33
Sulphur dioxide from sulphuric acid


Hey guys, i want to make Na2S2O5 for many experiments by bubbling SO2 from a solution of sodium carbonate but making SO2 by burning sulfur needs little setup and i can't make it from Na2S2O5 because as you know this ia what i want to make. So is there any method of making it directly from H2SO4 or making Na2S2O5 directly or indirectly from H2SO4.
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Alice
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[*] posted on 17-4-2017 at 07:03


Sulfur dioxide can be generated by treatment of sodium sulfite or sodium bisulfite with sulfuric acid.
Hope this helps.
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Amos
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[*] posted on 17-4-2017 at 07:05


Are you positive that there's no place where you live that you can simply buy sodium sulfite, bisulfite, or metabisulfite? Metabisulfites are one of the most commonly accessible amateur chemicals.
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idrbur
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[*] posted on 17-4-2017 at 08:50


Bro! I live in a small town in india and here finding even a most common chemical is like finding water in desert. So i have to make most of the chemicals on my own.:(
And thanks for replies.

[Edited on 17-4-2017 by idrbur]
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Sulaiman
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[*] posted on 17-4-2017 at 09:39


can you get Sodium thiosulfate ?
('hypo' in photographic circles).

not very efficient,
1 mole sulphuric acid + 1 mole sodium thiosulphate = 1 mole sulphur dioxide




CAUTION : Hobby Chemist, not Professional or even Amateur
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Aqua-regia
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[*] posted on 17-4-2017 at 10:59


If you have a plenty of sulfuric acid, and no else, boil this with common copper wire. You can get lot of SO2
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ave369
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[*] posted on 20-4-2017 at 09:47


Yes, heating sulfuric acid with copper should do the trick. It should be concentrated.



Smells like ammonia....
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pneumatician
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[*] posted on 22-4-2017 at 16:34


you use this?

http://www.ebay.com/itm/282442114323?_trksid=p2060353.m1438....

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bluamine
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[*] posted on 23-4-2017 at 02:35


If I still have a good memory, you can react it with tin to produce SnSO4, which decomposes at a relatively low temperature to give Sno2 with SO2
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AJKOER
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[*] posted on 24-4-2017 at 14:27


An interesting path mentioned in Atomistry.com on SO2 is the action of H2 on H2SO4 at room temperature with time. To quote:

"Sulphuric acid is reduced to sulphur dioxide and water by prolonged contact with hydrogen at ordinary temperatures. The reaction is fairly rapid at 250° C."

Link: http://sulphur.atomistry.com/sulphur_dioxide.html .

No heating, or any need for conc H2SO4, but an iron impurity in the sulfuric acid, I suspect, may help.

My speculation is that the reaction could proceed via a hydrogen atom radical and solvated electron pathway which could be sourced, for example, by photolysis in the presence of iron dust (see discussion at: http://onlinelibrary.wiley.com/doi/10.1029/2004JD005519/abst... ). Fine iron in air/water vapor could be a source of FeO, Fe2O3, FeOOH with the latter known to be photo active producing solvated electrons and hydroxyl radicals with H2O. Note, in the presence of H2SO4 and solvated electrons:

H+ + e-(aq) ---) .H (see, for example, https://www.google.com/url?sa=t&source=web&rct=j&... )

With hydrogen gas and any formed hydroxyl radical:

H2 + .OH ---) .H + H2O

Also, per Atomistry it is reported that "finely divided iron decomposes acid of density 1.75 at 200° C., yielding the gas", but the action of light may remove the need for heating Fe/H2SO4 or H2/H2SO4 to produce SO2 gas.
------------------------------------------------------

One possible embodiment would be add a small amount of fine iron to H2SO4 in a collapsed large clear plastic bag resulting in situ H2 formation filling the bag and allowing also some surface iron contact. Place in sunlight. Caution: calculated the volume of H2 generated so make sure the vessel does not rupture splattering acid. Safety gear a must!

[Edited on 24-4-2017 by AJKOER]

[Edited on 25-4-2017 by AJKOER]
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