khanoomkochooloo
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catalases for:H2O2->O2+H2O
hi everyone;
i want to know a little about the catalases used in getting O2 out of H2O2
i know about the enzymes but i m atually interested about KMnO4 or H2So4
how much shall i be using from each ?
pppppplllllllllzzzz help me !
[Edited on 6-8-2005 by khanoomkochooloo]
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Mr. Wizard
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KMnO4 works real well. Blood causes it to break down into O2, as witnessed when you clean a cut with peroxide. The experimental H2O2 rockets use a
silver screen to break down the peroxide, but it is the concentrated stuff. I haven't tried it with the diluted variety.
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Tsjerk
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MnO2
MnO2 is one of the most used catalyts for this purpose. And it's fairly easy obtained.
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khanoomkochooloo
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which ones better?
which ones better choped chicken liver or sth like mno2 or kmno4?
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Fleaker
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You can also use a halide salt (potassium iodide, sodium bromide, etc.)
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my nootloss
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Steps to getting O2
1 Go to the 99-cent store
2 Buy the cheep (D cell) batteries (will cost you 99 cents for about 4)
3 Get some h2o2 (cost = 99 cents)
4 Get the batteries open, take the black stuff out (MnO2)
5 poor on the h2o2, and there you go.
price = 1.98+tax+gas+time
Oh a word of advice, keep the zinc and carbon. Oh and the batteries are mostly called “heavy duty”
H2O2+MnO2= MnO2+O+H2O
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ordenblitz
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Activated carbon (filter charcoal) works very well also. It's cheap and easier to get at than digging in batteries.
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BromicAcid
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Practical catalyst for H2O2 decomposition.
http://sciencemadness.org/talk/viewthread.php?tid=2197
There is also at least one thread elsewhere on this that I remember because I referenced the erlier thread I just linked to, maybe they were merged.
Please use the search engine, or better yet use google with the operator site:sciencemadness.org to get good results. 
You mention using H<sub>2</sub>SO<sub>4</sub> as your decomposition catalyst, peroxide/sulfuric acid mixtures are not readily
decomposed unless somewhat concentrated and then some heat may need to be applied. They are kind of dangerous in contact with organic matter if
concentrated as well. Peroxide is more stable in acidic enviorments, you'd be better off adding to NaOH instead. As for permanganate, that is a
known peroxide decomposition catalyst, too powerful from the description some members give of the reaction.
[Edited on 8/9/2005 by BromicAcid]
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The_Davster
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Permanganate works, in a controlled fashion, if used as crystals(or at least in my test tube sized experiment it did), however, if you use a
permanganate solution you better watch out .
[Edited on 9-8-2005 by rogue chemist]
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my nootloss
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"Activated carbon (filter charcoal) works very well also. It's cheap and easier to get at than digging in batteries."
Batteries are a 3 in 1 deal
1 carbon rod
2 zinc
3 mno2
All that for about 99 cents, you cant beat that.
4(1+2+3) = 99 cents
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praseodym
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Well, why not use MnO2? It is the most commonly used for decomposition of MnO2.
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khanoomkochooloo
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| Quote: | Originally posted by my nootloss
Steps to getting O2
1 Go to the 99-cent store
2 Buy the cheep (D cell) batteries (will cost you 99 cents for about 4)
3 Get some h2o2 (cost = 99 cents)
4 Get the batteries open, take the black stuff out (MnO2)
5 poor on the h2o2, and there you go.
price = 1.98+tax+gas+time
Oh a word of advice, keep the zinc and carbon. Oh and the batteries are mostly called “heavy duty”
H2O2+MnO2= MnO2+O+H2O |
 thnx!
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Tsjerk
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"All that for about 99 cents, you cant beat that."
Sure I can beat that, believe me. MnO2, zinc or carbon don't cost that much, the amount that comes out of a battery isn't that much, just a
couple of grams.
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mericad193724
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Sodium Bromide huh.....I just tried it and IT DOES NOT WORK!!!! It was 99% Sodium Bromide from the pool store and it did not catalyze the
decomposition!!! So...what about Potassium Iodide...has anyone actually tried it. Or Iron Sulfate. Can someone tell me from experience if these work?
thanks
Maricad
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The_Davster
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KI definatly does work. It is used in the 'elephant toothpaste' type of demo. I have preformed it before.
Never tried with FeSO4
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neutrino
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Potassium permanganate is not a catalyst here. Rather, it is a reactant:
MnO<sub>4</sub><sup>-</sup> + H<sup>+</sup> + H<sub>2</sub>O<sub>2</sub> -->
MnO<sub>2</sub> + H<sub>2</sub>O + O<sub>2</sub>
[Edited on 27-6-2006 by neutrino]
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mericad193724
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does potassium iodide turn the water dark? I know the powder is white.
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The_Davster
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No
KI is just a catalyst, it does not get oxidized to iodine so will stay colorless.
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Fleaker
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"Sodium Bromide huh.....I just tried it and IT DOES NOT WORK!!!! It was 99% Sodium Bromide from the pool store and it did not catalyze the
decomposition!!! So...what about Potassium Iodide...has anyone actually tried it. Or Iron Sulfate. Can someone tell me from experience if these work?"
Sure it will. I have seen this happen (much to my dismay!), it will take some minutes (at least 15 for what happened to me, but mine was in the dark
of the basement, then went outside). I was making bromine with this happened, I already gave a full description of the runaway oxygen production
elsewhere on this site. I used 27.5% hydrogen peroxide though, and it was perhaps 18*C initially. It does work, and I base this on personal
experience.
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mericad193724
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Sodium bromide probably works for 27.5% or 30% or higher, but I tried it with 3% H2O2 and sodium Percarbonate, both of which had no oxygen generated
at all.
--------------------------------------------------------------------------------
I just got potassium iodide form the pharmacy to use as a catalyst. 65mg tablets, 200 total so there is 13g in the bottle! The tablets are slightly
brown, probably oxidized KI. I am going to need to extract the potassium iodide from these tablets which contains:
potassium iodide - Soluble
Dibasic Calcium phosphate - Insoluble
Stearic acid - insoluble
croscaremellose sodium - insoluble
silicon dioxide - insoluble
Magnesium stearate - insoluble
Ethylcellulose - ???(What is it?) No info in web!
If i just dissolve the tablets in water, decantate and evaporate with slight heating, will the KI be oxidized?
thanks for all the help guys.
Mericad
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franklyn
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Hypochlorite mutually anihilates with peroxide
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AllanD
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| Quote: | Originally posted by my nootloss
Steps to getting O2
1 Go to the 99-cent store
2 Buy the cheep (D cell) batteries (will cost you 99 cents for about 4)
3 Get some h2o2 (cost = 99 cents)
4 Get the batteries open, take the black stuff out (MnO2)
5 poor on the h2o2, and there you go.
price = 1.98+tax+gas+time
Oh a word of advice, keep the zinc and carbon. Oh and the batteries are mostly called “heavy duty”
H2O2+MnO2= MnO2+O+H2O |
Why take the time to cut open dry cell batteries?
Wouldn't taking the toner cartridge out of any nearby copy machine (or Laser printer) provide as much MnO2 as you could want?
AD
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