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rikkitikkitavi
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hence the name "vitriol oil" ?
Interesting , that thing about FeSO4 becomes usefull. I once found an old, non opened plastic can with FeSO4 (used as a biocide) wich
to much surprise wasnt full of light green crystals (FeSO4) but a brown mush of what must have been Fe(OH)SO4 then. Fe2+ easily oxidizes to Fe3+
/rickard
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axehandle
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Pumice seems hard to get. Does anyone think perlite would work as a substitute? Or even those little clay balls used in the bottom of flower pots
("lekakulor" in Swedish, can't remember the English name)?
[Edited on 2004-2-18 by axehandle]
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Mr. Wizard
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Is Vermiculite the pumice substitute you were thinking about? It is made by heating a volcanic rock which then expands into little worms (vermi?).
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axehandle
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No, perlite originally has a density close to water and is technically a glass. It is made into a very porous material by soaking it in water, then
heating it. The steam expands the material to about 10 times its original volume.
Edit: It's white, btw. Can be bought for next to nothing in any gardening store, is very porous, can absorb lots of water (and catalyst...?).
Edit2: Also, it's used in refractory comps because of its porosity and resistance to heat (in the 2000C range!). + I have about 100 liters of it
in a huge plastic bag. Weighs about 3kg.
[Edited on 2004-2-18 by axehandle]
[Edited on 2004-2-18 by axehandle]
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axehandle
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On my eternal quest for H2SO4, I'm now manufacturing large volumes of Fe(OH)SO4 using FeSO4, a glass pipe, a stainless but stained steel bowl, an
aquarium pump and hot water... the reaction is very fast, I couldn't believe it. We're talking 100g of FeSO4 converted to Fe(OH)SO4 in 15
seconds here. This is the <b>good</b> part.
| Quote: |
That's true, that pure FeSO4, when heated, give a mix of SO2 and SO3.
But: [Hofmann/Rüdorff: Anorganische Chemie]
Centuries ago, they let FeSO4 ("iron vitriol" with moisture oxidize by
air to an Iron(III)-hydroxide-sulfate Fe(OH)SO4.
This, when heated, gives that "fuming sulfuric acid":
2 Fe(OH)SO4 ===(heat)===> Fe2O3 + H2S2O7 (thus H2SO4 + SO3).
You really can get it by blowing air through an FeSO4-solution, this Fe(OH)SO4 is unsoluble, you can it filter and dry.
How easily to oxidize an FeSO4-solution is, you can see when you dilute pure FeSO4 in hot water and in few minutes in contact with air it will change
its color ang get cloudily because of Fe(III)- building.
Just I don't know that decomposition temperature but I can remember it was very low. (Even must not glow...)
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Does anyone have access to a textbook that would cite the temperature required? I don't want the <b>flat filled with SO2</b> thing to
happen again.... If it really is very low (e.g. lower than the boiling point of H2SO4), then it could be made on the stove.
Otherwise I'll have to build an improvised Liebig cooler.....
And I'll have to buy a propane Bunsen burner..... My furnace doesn't allow for much control, it's basically two settings: Off, and full
blast, respectively.
Edit: Slowly drying the Fe(OH)SO4 on the stove. The brown sludge bears a striking resemblance to what I produced the last time I had a stomach
illness.
[Edited on 2004-2-19 by axehandle]
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Friedrich Wöhler
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| Quote: | | Does anyone have access to a textbook that would cite the temperature required? |
Let me search at the weekend.
| Quote: | | The brown sludge bears a striking resemblance to what I produced the last time I had a stomach illness. |
 Don't confound them, the last one is not suitable to produce sulfuric
acid!
Kein Schwanz ist so hart wie das Leben.
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axehandle
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Thank you.
| Quote: |
Don't confound them, the last one is not suitable to produce sulfuric acid! |
I'm not so sure about that.
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