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Author: Subject: A new way to make NCl3?
Triflic Acid
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[*] posted on 8-2-2021 at 22:23
A new way to make NCl3?


I was just thinking that, if you bubbled chlorine through liquid ammonia, wouldn't you get NCl3. And if you let the excess ammonia and mono/di chloramines evaporate off, you would get the pure liquid, right? Also, I don't plan to actually do this, this is just an idea.
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njl
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[*] posted on 9-2-2021 at 08:16


Yeah, but the chlorination of ammonia is the standard method for NCl3. How is this new?
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[*] posted on 9-2-2021 at 11:16


I suspect that a mixture of NH3- a strong reducing agent- and Cl2- a strong oxidant would be explosive, even if NCl3 wasn't formed.

The reaction to give N2 and HCl would be very favourable.
It might even be hypergolic.



It's a very very bad idea.
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[*] posted on 9-2-2021 at 11:18


Quote: Originally posted by njl  
Yeah, but the chlorination of ammonia is the standard method for NCl3. How is this new?


Because it leaves out the water that usually moderates the reaction which means that it's only stupidly dangerous. Without the water it's even less of a good move.
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Jome
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[*] posted on 9-2-2021 at 12:39


https://www.youtube.com/watch?v=bX33R5uk-Kc

The king of obscure chemical reactions has been there, done that!
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chornedsnorkack
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[*] posted on 17-2-2021 at 23:40


Quote: Originally posted by Triflic Acid  
I was just thinking that, if you bubbled chlorine through liquid ammonia,


You cannot.
The boiling point of liquid ammonia is given as -33,34 C
The boiling point of liquid chlorine is given as -34,04 C.
Quote: Originally posted by Triflic Acid  

wouldn't you get NCl3. And if you let the excess ammonia and mono/di chloramines evaporate off,

If you add liquid chlorine to excess liquid ammonia, you would tend to get mostly monochloramine. To get mostly NCl3, you should add liquid ammonia to excess of liquid chlorine.
Pure monochloramine decomposes "violently" at -40 Celsius. So if you get a solution of monochloramine in excess of liquid ammonia, as you concentrate it, it can decompose violently.
Quote: Originally posted by Triflic Acid  
you would get the pure liquid, right? Also, I don't plan to actually do this, this is just an idea.

NCl3 is liable to explode when set off. So if you have a mixture of NCl3 and NH2Cl and try to separate it by warming, violent decomposition of NH2Cl might set off explosion of NCl3.
Further, a problem with NCl3 is that it is energetic and explosively so to decompose even alone:
2NCl3=N2+3Cl2
The reaction with NH3 would be even more energetic
NCl3+NH3=N2+3HCl
Whereas excess liquid Cl2 should be an inert diluent for NCl3.
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