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Author: Subject: What could be the products of oxidation of Ca3N2 with H2O2?
John paul III
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[*] posted on 7-7-2018 at 14:50
What could be the products of oxidation of Ca3N2 with H2O2?


What could be the products of oxidation of Ca3N2 with H2O2?
Specifically, could this reaction evolve nitric oxides/produce nitrate?
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CobaltChloride
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[*] posted on 7-7-2018 at 15:19


I'm guessing you are talking about aqueous H2O2, so the first thing to happen would be the hydrolysis of Ca3N2 to make NH3 and Ca(OH)2. None of these react with H2O2. H2O2 isn't a strong enough oxidant to oxidize ammonia to nitrate in aqueous solution.
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Metacelsus
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[*] posted on 7-7-2018 at 18:27


As CobaltChloride pointed out, ammonia will be produced by hydrolysis. Depending on what else is present, and the temperature, small amounts of hydroxylamine may be produced by oxidation. (See for example: https://www.sciencedirect.com/science/article/pii/S016729910... which showcases the reaction in presence of a titanium-based catalyst.) Nitrate and nitrite are highly unlikely to be formed. If any copper is present, the hydrogen peroxide will quickly decompose to oxygen and water. Other metals may also catalyze this.

[Edited on 7-8-2018 by Metacelsus]




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John paul III
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[*] posted on 8-7-2018 at 05:32


let me throw in another one so as to not start another thread:
According to wikipedia ammonia reacts with ozone
2 NH3 + 4O3 -> NH4NO3 + 4O2 + H2O
https://en.m.wikipedia.org/wiki/Ozone
Could the decomposition of H2O2 be used as a source of ozone? Would the yield of O3 ever reach above 10%? Or would singlet oxygen undergo similiar reaction?

[Edited on 8-7-2018 by John paul III]
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Metacelsus
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[*] posted on 8-7-2018 at 07:53


Quote: Originally posted by John paul III  

Could the decomposition of H2O2 be used as a source of ozone? Would the yield of O3 ever reach above 10%?


No. In fact, ozone is decomposed by hydrogen peroxide, via hydroxyl radical intermediates.

See: https://onlinelibrary.wiley.com/doi/pdf/10.1002/cjce.5450770...




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John paul III
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[*] posted on 8-7-2018 at 08:12


I was thinking about generating an oxygen gas mix rather than introducing the ammonia into H2O2. Do you think that it still wouldn’t work? (with temperature control the water content of the gas could be kept to a minimum)
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[*] posted on 8-7-2018 at 09:10


A mixture like this
Oswalt style nitric acid needs a flow of ammonia gas and oxygen gas
http://www.sciencemadness.org/talk/viewthread.php?tid=71282&...




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John paul III
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[*] posted on 8-7-2018 at 09:23


But the difference here is the active oxygen - singlet O and ozone, hopefully in large enough concentration to get an acceptable yield (by H2O2)
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