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Author: Subject: NH8 S2O8
waheeb
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[*] posted on 23-12-2004 at 16:05
NH8 S2O8


hi

I am trying to get rid of NH3 and H2 SO4 to get ammonium persulfate.

How do i make it? I don't remember the hemistry of persulfate.
The reaction of NH3 with H2SO4 is (NH4)2 SO4

any help is appreciated

thanks

waheeb
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neutrino
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[*] posted on 23-12-2004 at 16:13


I’m sure we’d all be happy to help you if we could understand what you’re talking about. Please make your post intelligible. There is already a thread about persulfates here.
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waheeb
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[*] posted on 23-12-2004 at 16:55


hi neutrino

As simple as this:
How do you make ammonium persulfate

thanks

waheeb
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The_Davster
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[*] posted on 23-12-2004 at 17:33


I understood the origional question. It was essentially how to get ammonium persulfate from ammonia and sulfuric acid, thus how to get ammonium persulfate from ammonium sulfate.



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neutrino
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[*] posted on 23-12-2004 at 17:50


I think I’m starting to exercise selective understanding: crap posts don’t make sense, while good ones do. It’s annoying that so many newbies have such poor grammar. To answer your original post, look at the link.
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BromicAcid
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[*] posted on 23-12-2004 at 18:19


There is a good chance waheeb does not have English as his/her native language, although it is always nice to do a grammatically correct post without spelling errors and such, some people cannot pull this off, but if they are trying then there is no reason to belittle them, I understood exactly what waheeb was asking in the opening post, although waheeb said it in a round about way and should have used the search engine.



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JohnWW
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[*] posted on 24-12-2004 at 03:53


Ammonium peroxysulfate, (NH4)2S2O8, would be quite highly explosive, similarly to the perchlorate and nitrate, but probably less stable. It would be about as dangerous as the chlorate, bromate, and permanganate, if they could be made.
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cyclonite4
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[*] posted on 24-12-2004 at 04:49


Quote:
Originally posted by JohnWW
Ammonium peroxysulfate, (NH4)2S2O8, would be quite highly explosive...


Are you serious?:o
I can get this for $6 per 600g bottle from an electronics supplier as an PCB etchant.
I assume it is an oxidising agent and would need to be mixed with a fuel.
Do you know the equation for its release of oxygen (for stoich. purposes)?




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JohnWW
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[*] posted on 24-12-2004 at 11:14


In the explosive decomposition of (NH4)2S2O8, e.g. induced by heating, the peroxide linkages would break, and partially oxidize the ammonium to mostly N2 and H2O, with H2SO4, H2S2O7, (NH4)2SO4 and (NH4)2S2O7 also formed. Some N2H4 and NH2OH as sulfates are also possibilities. It is difficult to write a plausible stoichiometrically correct equation for it, especially as there is an excess of ammonium over available oxygen, but then explosive detonations are seldom stoichiometrically exact.
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cyclonite4
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[*] posted on 25-12-2004 at 04:25


So basically no fuel is required (self redox).
Well... I'm just going to hafta try this out. How strong would heating need to be? Could a blasting cap be used?




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S.C. Wack
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[*] posted on 25-12-2004 at 09:06


No, fuel is required. The salt itself does not explode.
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cyclonite4
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[*] posted on 25-12-2004 at 19:37


Yes, but there is an excess of ammonia to oxygen, so whats going to burn the fuel?



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