When I was young I bubbled chlorine into strong ammonia solution and got a yellow layer of nitrogen trichloride (at least I think this was how I did it). It formed as long as it was in an ice bath and exploded violently on heat and i think even impact. Did a similar process for nitrogen triiodide. Still have all my fingers.
I bet that smells wonderful(even with a fume hood i presume you still get some smell coming out with the door open) Like a diaper bin mixed with a pool.....
That reaction is almost a work of art. Two liquids with almost the same boiling point coming together to form a white vapor seemingly from nowhere. Beautiful.
It does not really matter which reaction takes place. There are several all all of them are exothermic and the liquids are at the boiling point, so they start boiling rapidly, which is what we can observe as an explosion. Look closely and you can see that the explosion does not only take place where the liquids mix, but you can see the liquid ammonia expanding all by itself, because it got hot.
So is monochloramine that unstable? Or is it due to the temperature. I work in the water industry and drinking water has primarily mono and di chloramines and they are pretty stable (for the most part). When an addition of chlorine is necessary to boost chlorine residual, a rough stoichiometric amount of liquid ammonia is added to combine to form monochloramine. Nice videos btw, came from extraction and ire channel.
i'm not convinced ncl3 residue isn't forming like dropping tcca tablets into liquid ammonia and getting that same yellow color followed by the violent reaction,as it's formed in even tiny amounts even light can set the stuff off or you saying mean things about it in general
elemental fluorine might be a bit challenging to handle, given that it destroys glass and is hypergolic with most flammable substances, people included...
I was curious before you should the equation how NH3 and Cl2 formed NH4CL when there was no extra H kicking around as in NH4OH, but I see it splits an NH3 and uses some of the H+ from there producing N2 gas.
@@joeylawn36111 Yes, atmospheric moisture, but inside the test tubes due to the liquids boiling it would be NH3/Cl2 liquid and vapour displacing atmospheric moisture. 0:47 As the test tubes were brought together the vapour we see would be reacting with moisture, but inside the test tube due to lack of atmospheric moisture by being displaced reactions 1 and 2 are most likely happening favouring 1 since it's products are most stable.
i searched whole internet and got no where any reaction between ammonia and dinitrogen tetroxide please try the experiment and if it didnt explode or combust spontaneously please inform
1:10 Oh no, I hope none of those drops got your clamp. I don't even want to think about how corrosive pure liquid chlorine is... Ok, upon further reflection, that's a lie. I actually do want to know how corrosive liquid chlorine is. Could you, by chance, show its interaction with some bulk metals? Perhaps just some foils that are thick enough to be called bulk materials? I think I recall interactions with some metals powders, but I don't recall anyone showing the effects on bulk metals.
I would be interested to know what happens, if you pay careful attention to producing absolutely anhydrous liquid ammonia and liquid chlorine, then mix the two under an inert and anhydrous atmosphere. You would probably need access to some expensive lab equipment to try this of course ...
Can you please make experiment wit mixing of liquid NH3 with liquid (anhydrous as possible by simple procedure of preparing) HCl solid NaOH and 98%H2SO4 reacts as gunpowder or overheated water exp. also electrolysis of liquid "100%" HCl is very intresting
Do the solid forms react with each other as well? Even at liquid Helium temperatures? Also, WHAT-IF you tried it the other way round as well? (Pour some liquid Ammonia into Liquid Chlorine, behind a Polycarbonate shield of course! :))
Yes, In basically if you put NH3 in Cl2 there is an exceed of NH3 and vice versa, now this doesn't matter for most reactions but in this one it does, cuz there is not enough chlorine to generate NCl3
