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clearly_not_atara
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I no longer think that will work.
However I'm still sort of interested in ways to reduce/absorb the heat of hydration of SO3. Instead of dealing with strange chemicals the following
rxn seems interesting:
CaSO4*2H2O (plaster/gypsum) + 2 SO3 >> CaSO4 + 2H2SO4
with significantly less heat released than the reaction with water, but still a lot. How to perform this though?
The difficulty is not in producing SO3, which happens by simply heating bisulfate, but in capturing it without destroying it or killing the
experimenter.
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Radium212
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Nice! Finally a way for people with little equipment to produce sulphuric acid at home. Thank you.
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TheIdeanator
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Codyslab did a video on this recently and got me thinking about improvements. It would seem to me that the dissolution rate of SO3 is limited by the
surface area. Why not add in one of those piezoelectric humidifier elements to get some good spray going.
“I will show you fear in a handful of dust.”
― T.S. Eliot
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j_sum1
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Thread Closed
6-1-2019 at 00:53 |
j_sum1
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Thread Opened
6-1-2019 at 01:12 |
j_sum1
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Thread Pruned
30-1-2019 at 06:22 |
Refinery
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Calcium sulfate with sodium silicate at significant temperature should result with SO3 production that can be absorbed to 98% sulfuric acid to yield
oleum and that can be then diluted?
Other sulfates are also viable with lower decomp temp like copper, but the source price is too high. CaSO4 is extremely cheap, hence resulting product
can just be discarded.
I suggested the same method with nitrates. Bulk Ca, Mg and Cu nitrates can be pyrolyzed for NO2 to produce HNO3, and I figure that they could be
reconstituted with two step metathesis process from another source of nitrate?
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RogueRose
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What would the product be of the calcium sulfate and sodium silicate and what temp do you think you would need, I suspect pretty high, like melting
steel high?
[Edited on 5-6-2020 by RogueRose]
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woelen
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Thread Untopped
15-8-2020 at 13:22 |
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