Hermes_Trismegistus - 19-10-2004 at 17:55
Barium Carbonate is a common chemical used in pottery. It decomposes at ~1300, releasing Carbon Dixide and leaving Barium Oxide. When Barium Oxide is
heated strongly in air it forms Barium Peroxide. When Barium Peroxide is dissolved into sulfuric acid, it forms insoluble Barium Sulfate and a strong
Hydrogen Peroxide solution.
If the Barium Sulfate was heated strongly would Sulfur Trioxide gas evolve leaving Barium Oxide?
Are there any other ways to relieve the Barium Sulfate of its burdensome Sulfate? (it wants a divorce)
P.S.
(please....no responses about alloying the barium with ununnium and shooting it into the sun with a rocket ship propelled by walnut flavoured
jellybeans and used condoms..)
[Edited on 20-10-2004 by Hermes_Trismegistus]
BromicAcid - 19-10-2004 at 18:22
I don't think heating barium sulfate to yield sulfur trioxide is possible. My handbook of chemistry and physics gives a melting point for barium
sulfate of 1580 C, nothing mentioned of decomposition, and even if it did liberated SO3 later, the temp would be too high and disproportionate it
between sulfur dioxide, sulfur, and oxygen.
Heating barium sulfate with carbon yields a mixture of barium oxide and sulfide, sulfur dioxide gas and carbon monoxide exit. A mixture of barium
sulfate with aluminum powder should yield barium metal, barium sulfate, barium oxide, and barium peroxide. Of course they would be difficult to
separate.
Acidic azide solutions are strong reducing agents, maybe you could give one of those a try 
Ium - 19-10-2004 at 19:02
With a 1580C melting point and an even higher temperature of decomposition there is an obvious hurdle to overcome if you wish to decompose with heat.
You may want to try reduction with aluminium. Is it possible? In the free metal it could be separated from the Al oxide via mechanical separation
while melted (Ba mp is around 725C).
Industrial reduction follows the below series of overall reactions.
BaSO4 + 2C = BaS + 2CO2
BaS + CO2 + H2O = BaCO3 + H2S
BaSO4 + SiO2 + C = BaSiO3 + SO2 + CO
Both reactions produce an acid soluble product which can be further manipulated.
The temperatures involved however are around 1000C. Still, it allows for a lower temperature than roasting the sulfate independently.
One novel idea if you have lots of time on your hands. Microbial reduction
!
http://water.usgs.gov/nrp/proj.bib/microbiology/barite.html
S.C. Wack - 19-10-2004 at 19:04
Heating the sulfate with Na2CO3 will give you BaCO3 in high yield.
That's the fuckin' ticket!!!
Hermes_Trismegistus - 19-10-2004 at 19:24
(clap hands)
Edit: Thank you all very much.
[Edited on 20-10-2004 by Hermes_Trismegistus]
Blind Angel - 21-10-2004 at 18:13
Na<sub>2</sub>CO<sub>3</sub> + BaSO<sub>4</sub> =x joule=> Na<sub>2</sub>SO<sub>4</sub>
+ BaCO<sub>3</sub>
=> BaCO3 is suppose to precipitate, filter, heat BaCO3 to release CO and make BaO<sub>2</sub> (just simple Q, what goes up to
1300°C?).
Here's the idea, passing H<sub>2</sub>SO<sub>4</sub> on BaO<sub>2</sub> on a mesh so the
BaSO<sub>4</sub> is automaticly filtered, dripping conc. H<sub>2</sub>O<sub>2</sub>. Then why not reusing the
Na<sub>2</sub>SO<sub>4</sub> (previously dehydrated) to clear up some more water in the Peroxide? (is
Na<sub>2</sub>SO<sub>4</sub> soluble in Peroxide?)
=> Go get your "My First V2 Rocket" at your local x-Mart 