Alkoholvergiftung
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With TiO2 Nitrate directly from the Atmosphere
I ve finde few Artikels About TiO2 that it can bind N2 directly from Atmosphere under UV light or sunlight. Does any one have more Information About
it or has tried to manufacture some Nitrate with it?
Oh and here is an link to one of the Artikels.
https://www.nature.com/articles/ncomms3249.pdf?origin=ppub
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RedDwarf
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I can't work out if the surface area in the nitrate production figures given (mg/sq metre/hr) is particle surface area or the area of the coated
paper. If it's the area of the coated paper at an average of 6mg/sq metre/hr over 12 hours of daylight, then you could be waiting an awful long time
for any reasonable quantity of nitrate! (26g/sq meter/year).
I should say that this could be significant from an environmental point of view but not as a source of raw materials.
[Edited on 27-6-2019 by RedDwarf]
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AJKOER
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For those without access to KNO3, sold as a stump remover, here is a suggestion.
It appears NH4NO2 (caution: toxic and also nitrites, in general, are cited as likely carcinogenic) is readily created, and annoyingly decomposes into
much N2 gas (which, if collected, could indicate the amount of NH4NO2 that was created), by the action of NH3(aq) in 3% H2O2 acting on copper metal
(plus a touch of sea salt, as this is, in a part, an electrochemical reaction, see my prior cited references and comments at https://www.sciencemadness.org/whisper/viewthread.php?tid=77...), which I jump start for 30 seconds in a microwave.
Adding to this mix, at some point (prior to N2 evolution), NaOH (target reaction NH4NO2 + NaOH --> NaNO2 + H2O + NH3 (g), see https://books.google.com/books?id=6OcDAAAAMBAJ&pg=PA277&... , or perhaps Na2CO3, Washing Soda) may obviate the obvious gaseous decomposition
of the pH sensitive NH4NO2 perhaps creating some stable NaNO2 upon air evaporation of the solution along with a tetraamine copper salt (caution:
possibly energetic on heating the dry salt).
At least an interesting experiment, and use appropriate safety measures.
The possible nitrite would bring one a step (or more) away from a nitrate.
[Edited on 29-6-2019 by AJKOER]
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Alkoholvergiftung
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Interesting Experiment. But you can make nitrites with Fresh Copper turnings and concentrate ammonia solution.Copper powder form oxide and ascorbic
Acid works too. Copper is the only metal who can oxidize ammonia at roomtemperatur. (source: Friedrich Schönbein)
Ironoxidhydroxide in an bottle with air and ammonia solution shaken forms HNO2. Thats why iron rich soils are rich with Nitrates.
I thought it would be interesting if you can make Nitrates directly not over ammonia and with free sunenergie. 
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AJKOER
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Quote: Originally posted by Alkoholvergiftung  | Interesting Experiment. But you can make nitrites with Fresh Copper turnings and concentrate ammonia solution.Copper powder form oxide and ascorbic
Acid works too. Copper is the only metal who can oxidize ammonia at roomtemperatur. (source: Friedrich Schönbein)
Ironoxidhydroxide in an bottle with air and ammonia solution shaken forms HNO2. Thats why iron rich soils are rich with Nitrates.
I thought it would be interesting if you can make Nitrates directly not over ammonia and with free sunenergie. |
Your comment on an Iron path to nitrite/nitrate, together with the better known Copper metal, both transition metals, appears to confirms my prior
comment on SM below on a possible fenton or fenton-type (based on Cu) path to NO2-/NO3- at https://www.sciencemadness.org/whisper/viewthread.php?tid=13... presented again below:
| Quote: Originally posted by AJKOER | Some theory suggests, to create nitrite/nitrate from ammonia, start by employing a hydroxyl radical generating mechanism including photolysis (see http://pubs.acs.org/doi/abs/10.1021/jp0349132 ), fenton and fenton-type reactions involving transition metals (discussed below), radiation
(microwave pulse), electrolysis, sonochemistry,...
Then, the action of the •OH on ammonia in the presence of dissolved oxygen (or employ H2O2) is claimed by one reference to proceed as follows:
NH3 + •OH → H2O + •NH2 (see Laszlo extract and link below)
•NH2 + O2 → NH2O2• (aminylperoxyl radical unstable) → NO + H2O (See , "On the aqueous reactions of the aminyl radical with molecular oxygen
and the superoxide anion", Table 2.1 at https://www.google.com/url?sa=t&source=web&rct=j&... )
Having formed some NO, in the further presence of a hydroxyl radical source generator and hydrogen peroxide the following reactions, for example,
could introduce the formation of NO2:
H2O2 + •OH → H2O + •HO2
•HO2 + NO → •OH + NO2 (see https://www.google.com/url?url=http://scholar.google.com/sch... )
or, as the net of last two reactions equals:
H2O2 + NO ---UV or Fe(++), Cu(+), Co(++),..→ H2O + NO2
And further:
NO2 + H2O → HNO2 + HNO3
which introduces aqueous nitrite that is a better light induced promoter of hydroxyl radicals then nitrate, which is superior to H2O2. In the presence
of uv, strong solar light or select transition metals, this postulated reaction chain can likely accelerates the conversion of ammonia to
nitrite/nitrate. Interestingly, there are researchers reporting tissue cell damage from the seeming direct action of NO on H2O2 in biological systems
(see, for example, "Hydroxyl radical formation resulting from the interaction of nitric oxide and hydrogen peroxide.",by Nappi AJ, Vass E. ) although,
in my opinion, such a direct radical reaction need not take place given the enabling effects of light or transition metals. Note, my simple reaction
chain consumes and regenerates the very short lived hydroxyl radical which, in essence, could increase its apparent reactivity life span (as measured
by random cell collisions leading to cellular damage) having been, in effect, resurrected.
...........
[Edited on 16-9-2016 by AJKOER] |
Link to extract: http://www.sciencemadness.org/talk/viewthread.php?tid=30473 .
Correction to the above, the free radical •NO2 does not directly react with water. More correctly, the reaction proceeds as follows:
•NO2 + •NO2 → N2O4
N2O4 + H2O = HNO2 + HNO3
I would also add the reaction involving the superoxide •O2- which exists at pH > 4.88 (and as •HO2 at pH < 4.88, or •O2- in an aerosol
with H2O, also functionally behaving as •HO2 ):
•O2- + •NO --> ONOO-
which converts into nitrate.
My suggested path involves the use of both O2 (via an air pump) and H2O2. Also add NH4+ to the mix from an added ammonium salt (as NH4+ = H+ + NH3),
as is performed in the commercial leaching of copper ore.
[Edited on 29-6-2019 by AJKOER]
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