guy
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Iron pyrite
Is there anything i can do w/ iron pyrite?
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The_Davster
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Fools gold eh? Try selling it to people who dont know the difference between it and gold and Use the money you make to buy chemicals. But if you are wondering what to do chemically with it you could dissolve it in an acid of
your choice and from there make whatever iron compound you fancy.
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chemoleo
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Hmm when I tried it FeS2 did not dissolve in HCl. No gas (H2S) evolution either, it remained unchanged.
For making Fe compounds, I would use normal iron nails for that  - easier and
cheaper
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Geomancer
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Hmm. I was just reading that one could generate H<sub>2</sub>S with dilute HCl+iron pyrite. Then again, that was in "The Complete
Book of Ecstacy" (on Rhodium's site), which may not be an authoritative source. Chapter 3, under HI.
Industrially, iron pyrite is used as a sulphur source, for the production of sulphuric acid, both by roasting for SO<sub>2</sub> to
feed the contact and lead chamber processes, and by converting to ferric? sulphate, for the clay pot process.
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guy
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i put it in H2O2 and bubbles formed. they were odorless. Acids don't seem to work.
After putting it in H2O2, the liquid reacted w/ NaHCO3 to form CO2
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guy
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Maybe the reaction is
FeS2 + H2O2 --> Fe(OH)2 + H2SO4
then the acid reacted w/ the iron hydroxide to form the bubbles.
That explains why it took a while for the bubbles to form.
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The_Davster
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The FeS2 could have acted as a catalyst for H2O2 decomposition, like MnO2, to form oxygen bubbles. You should try to collect the gas produced and do
the glowing splint test.
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guy
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http://www.mines.edu/fs_home/jhoran/ch126/app.htm
This website shows the oxidation of FeS2 with Hydrogen peroxide
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The_Davster
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Wow, personally, I'm surprised that sulfuric acid is produced. I guess I was partially wrong.
2 H2O2 --> O2 + 2H2O
4 FeS2(s) + 15 O2(aq) + 14 H2O(l) --> 4 Fe(OH)3(s) + 8 SO42-(aq) + 16 H+(aq)
I assume that the first reaction is still catalysed by the FeS2 as I mentioned before, but then the products from the first reaction react with the
FeS2 to make the sulfuric and iron hydroxide. The reaction 4 FeS2(s) + 30 H2O2(aq) --> 4 Fe(OH)3(s) + 8 SO42-(aq) + 16 H+(aq) + 16 H2O(l) is
actually to overall reaction-it did not show both reaction steps which is why I did not understand why it happened.
hmm...this gives me an idea. Moisten some powdered pyrite with water and let sit untill all the "gold" color has dissappeared, periodically
re-moistening to keep the pyrite at the constituency of a putty. When gold color has dissappeared squeeze out the liquid which should be some H2SO4
of decent concentration. I suppose this could be done with H2O2 but with the concentrations of it available to most of us, heavily diluted with
water, the final sulfuric concentration would be pretty low. Also keeping it in a putty like state increases the surface contact with the air,
supplying the oxygen necessary for the reaction.
This is begginning to sound like a good method for sulfuric, only reactants are water and fools gold, accessible to everyone.-Can anyone find any
problems with this method?
Well, I'm off to dig up my mineral set I got as a child and begin some testing.
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Saerynide
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How come the ferric hydroxide wont react with the sulfuric acid to make ferric sulfate?
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vulture
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I was about to ask the same thing.
Also, oxidation of PbS with H2O2 yields PbSO4...
One shouldn't accept or resort to the mutilation of science to appease the mentally impaired.
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unionised
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FeS2 + "o"--> FeSO4 + ??
Pyrites has an excess of sulphur compared to ferrous sulphide.
Even allowing for Fe(III) suplphate as the product would still be sulphur left over and this might be oxidised to H2SO4.
(Of course, it might just get oxidised to sulphur and sit there grinning at you).
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The_Davster
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I'm so stupid
I can't believe that I did not notice that if an acid and base are produced that they would react.
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Polverone
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According to one of the old chemistry books I have lying around, powdered iron pyrite + charcoal may be heated to produce CS2. Fun!
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Theoretic
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If the solution of sulfuric acid is dilute, iron hydroxide will not dissolve, and any present will hydrolyse. The ferric cation is very acidic,
remember. Fe2+ is much less acidic, but will be quickly oxidized by air to Fe3+.
The excess sulfur will be oxidized to sulfuric acid.
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guy
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You could heat up FeS2 to make Fe2O3 and SO2.
How much heat is required though?
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guy
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Na2CO3 + FeS2 --> ?
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axehandle
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You could heat up FeS2 to make Fe2O3 and SO2.
How much heat is required though?
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From what I can remember of my H2SO4 production studies, it's a self-sustaining reaction once it's begun and the pyrite is in a pile.
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