symboom
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Nitric Acid Production - Amine oxidation (NH2)
Dimethyldioxirane wich is made from cheap materials
acetone, sodium bicarbonate, and potassium peroxymonosulfate (commercially known as "oxone")
more doable
Sodium amide reacts violently with water to produce ammonia and sodium hydroxide and will burn in air to give oxides of sodium and nitrogen.
NaNH2 + H2O → NH3 + NaOH
2 NaNH2 + 4 O2 → Na2O2 (and sodium peroxide) + 2 NO2 + 2 H2O
preparation
Sodium amide can be prepared by the reaction of sodium with ammonia gas, but it is usually prepared by the reaction in liquid ammonia using
iron(III) nitrate as a catalyst. The reaction is fastest at the boiling point of the ammonia, c. −33 °C.
using dry ice and denatured alcohol
of course this way to nitric acid is not very economical you do end up with sodium peroxide
2 Na + 2 NH3 → 2 NaNH2 + H2
[Edited on 6-1-2012 by symboom]
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Pulverulescent
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NO<sub>2</sub> is moderately in water producing nitric and nitrous acid - for efficient conversion to HNO<sub>3</sub>
a tall absorption tower is generally required except when the absorption is aided by using high pressure!
And sodamide is not easily acquired, or prepared, though a new member here has offered a smallish quantity for sale recently!
P
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UnintentionalChaos
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....This is about the most inane proposed method that I have ever heard of to make nitric acid. Bravo. Also, what does the DMDO have to do with
anything?
Department of Redundancy Department - Now with paperwork!
'In organic synthesis, we call decomposition products "crap", however this is not a IUPAC approved nomenclature.' -Nicodem
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Sedit
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Im assuming for the oxidation of Ammonia....
Im shocked we sit here and have someone wish to discuss how to make HNO3 out of NaNH2..... We are supposed to believe that you can get Sodium Amide
yet can't get Nitric acid... Wow dude... just wow.
Knowledge is useless to useless people...
"I see a lot of patterns in our behavior as a nation that parallel a lot of other historical processes. The fall of Rome, the fall of Germany — the
fall of the ruling country, the people who think they can do whatever they want without anybody else's consent. I've seen this story
before."~Maynard James Keenan
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symboom
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Quote: Originally posted by UnintentionalChaos  | | ....This is about the most inane proposed method that I have ever heard of to make nitric acid. Bravo. Also, what does the DMDO have to do with
anything? |
oops its able to oxidize amines to nitrates and nitrites
electrolysis of sodium hydroxide
but yes you right this is very uneconomical
just buying potassium nitrate or sodium nitrate is wayyy easier
i was just interested in the chemistry
and mostly the sodium peroxide which is damn expensive
to get really pure
20% if made by burning sodium in air hopefully you get close to 99% burning sodium amine in air
[Edited on 6-1-2012 by symboom]
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AndersHoveland
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I can see why you might think this could be a feasible route to nitric acid. I suppose it depends on how easy it is for one to prepare sodium metal.
Preparation of sufficient amounts of anhydrous NH3 might also be inconvenient.
Might I suggest another creative, but similarly inconvenient method to prepare the NH3, if you have the sodium metal to begin with?
Na + LiCl --> NaCl + Li
(the lithium product would form a molten alloy into the sodium, which has a conveniently low melting point)
6 Li + N2 --> 2 Li3N
(this reaction would be done with the lithium still dissolved in the molten sodium. nitrogen will react with Li or Mg, but not Na or K. The
reasons for this are complicated and discussed elsewhere in this forum)
Li3N + 3 H2O --> 3 LiOH + NH3
(or use Mg instead of Li)
As for the equation you have shown from wikipedia, I am not sure it is entirely accurate or correct. Most of the NO2 would tend to combine with the
Na2O2 to form NaNO3.
White sodium amide gradually becomes yellow after exposure to air. Unlike white sodamide, after yellow sodamide has been reacted with water, there
will be formation of additional gasses after some dilute acid is added, which include nitric oxide and more nitrogen. This suggests that
ambient oxidation of sodium amide forms other products, possibly including sodium azide.
"An investigation of sodamide and of its reaction-products with phosphorus ...", William Phillips Winter, p21
http://books.google.com/books/about/An_investigation_of_soda...
[Edited on 7-1-2012 by AndersHoveland]
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symboom
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hydrogen reducing NO gas
electrolysis of sodium hydroxide
hydrogen gas protects the sodium metal as it does not react with it in normal conditions
anhydrous ammonia NH4Cl and calcium hydroxide seems the best reaction solid products of course generating ammonia gas and liquifying it with dry ice
and denatured alcohol forming cool bath
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