| Pages:
1
2 |
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
Triethylamine synthesis
I remember reading that triethylamine can be made by the alkylation of ammonia with ethanol
This is the eqation
NH3 + 3 C2H5OH = N(C2H5)3 + 3 H20
Here is my working out of the quantities
1 mol NH3 = 17.031g
3 mol C2H5OH = 3 x 46.068g = 138.204g
Density of my ammonia = 18g/l
So for 1 mol NH3 i need 0.946 litres = 946ml
Density of 99% ethanol (i am treating it as 100%) = 79g/l
I got the density of ethanol from a website and i am not sure it is correct
3 mol C2H5OH= 1.749 litres
I would scale it down of course
Does this look right?
Should i have an excess of any of these ingredients?
Can i just mix them together or do i have to heat them or something to get them to react?
[Edited on 20-3-2015 by Ramium]
|
|
|
gdflp
Super Moderator
Posts: 1320
Registered: 14-2-2014
Location: NY, USA
Member Is Offline
Mood: Staring at code
|
|
Unfortunately, it's not that simple. For that reaction to work, I believe that the vapors have to be mixed, then passed over a heated catalyst,
though this is a vague recollection.
(Apparently at high pressures too.) A more suitable synthesis of triethylamine in an amateur setting can be found here : http://chemistry.mdma.ch/hiveboard/chemistrydiscourse/000330...
[Edited on 3-20-2015 by gdflp]
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Ammonia doesn't react with ethanol easily. When it does, you'll get a mixture of mono, di, and trisubstituted ethylamine. I found a patent: https://www.google.com/patents/US20080194879
which uses transition metal catalysts for the reaction at 15 to 25 MPa and 170 to 230° C.
Not an easy proposition.
[Edited on 20-3-2015 by Cheddite Cheese]
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
Thanks for your replies.i will find another method
|
|
|
CuReUS
National Hazard
Posts: 928
Registered: 9-9-2014
Member Is Offline
Mood: No Mood
|
|
what about an eschenweiler clark using NH3,acetaldehyde and HCOOH ?
|
|
|
Metacelsus
International Hazard
Posts: 2539
Registered: 26-12-2012
Location: Boston, MA
Member Is Offline
Mood: Double, double, toil and trouble
|
|
Why use acetaldehyde making triethylamine? Yes, it's possible, but then again triethylamine is much easier to get than acetaldehyde. I got some pretty
recently from Elemental Scientific.
|
|
|
Nicodem
|
Thread Moved
21-3-2015 at 12:29 |
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
I don't have access to acetaldehyde sadly
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
Quote: Originally posted by Cheddite Cheese  | | Why use acetaldehyde making triethylamine? Yes, it's possible, but then again triethylamine is much easier to get than acetaldehyde. I got some pretty
recently from Elemental Scientific. |
I don't want to buy triethylamine I want to make it to explore the chemistry.
|
|
|
PHILOU Zrealone
International Hazard
Posts: 2893
Registered: 20-5-2002
Location: Brussel
Member Is Offline
Mood: Bis-diazo-dinitro-hydroquinonic
|
|
@ Ramium,
Your calculations are wrong.
Density of ethanol 100% is more like 790g/L (0.79kg/L) than 79g/L!
You will get more chance at triethylamine from ammonia and CH3-CH2-X instread of ethanol.
CH3-CH2-I > CH3-CH2-Br > CH3-CH2-Cl (gaseous).
CH3-CH2-X can be easily obtained from HX/ZnX2 or H2SO4/NaX and ethanol.
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
|
|
|
papaya
National Hazard
Posts: 615
Registered: 4-4-2013
Member Is Offline
Mood: reactive
|
|
I'm sorry if I ask this in wrong place, but what about Delepine reaction route to amines (https://en.wikipedia.org/w/index.php?title=Del%C3%A9pine_rea...), where you can use hexamethylenetetraamine instead of ammonia, isn't this more
convenient than ammonia? How practical is it if I try to synthesize ethylenediamine from dichloroethane + urotropine under reflux, does this work?
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
| Quote: Originally posted by PHILOU Zrealone | @ Ramium,
Your calculations are wrong.
Density of ethanol 100% is more like 790g/L (0.79kg/L) than 79g/L!
You will get more chance at triethylamine from ammonia and CH3-CH2-X instread of ethanol.
CH3-CH2-I > CH3-CH2-Br > CH3-CH2-Cl (gaseous).
CH3-CH2-X can be easily obtained from HX/ZnX2 or H2SO4/NaX and ethanol. |
thanks
Could u please tell me what the name of CH3-CH2-x
(the thing u sugested instead of ethanol)
|
|
|
Steam
Hazard to Others
Posts: 238
Registered: 25-3-2014
Location: Minnesota
Member Is Offline
Mood: Triple Point
|
|
Ethyl iodide/bromide/chloride aka. chloroethane
http://en.wikipedia.org/wiki/Chloroethane
**edit** as PHI said, iodoethane is more reactive than bromoethane, which is more reactive than chloroethane.
The difficultly will be finding chloroethane... you will probably have to make it yourself. Chlorination of alcohols can be done using Thionyl
Chloride or Zinc chloride. I have chlorinated benzyl alcohol before by using an excess of HCl, but you will need something a bit stronger for ethanol
(benzylchloride is particularly nasty stuff- best have a a nice fume hood or where swimming goggles  ) It was discussed in depth in thisThread!
[Edited on 23-3-2015 by Steam]
DISCLAIMER: The information in this post is provided for general informational purposes only and may not reflect the current law in your jurisdiction.
No information contained in this post should be construed as legal advice from the individual author, nor is it intended to be a substitute for legal
counsel on any subject matter. No reader of this post should act or refrain from acting on the basis of any information included in, or accessible
through, this post without seeking the appropriate legal or other professional advice on the particular facts and circumstances at issue from a lawyer
licensed in the recipient’s state, country or other appropriate licensing jurisdiction.
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
So will iodoethane react easily with ammonia to form triethylamine?
Thanks
|
|
|
Steam
Hazard to Others
Posts: 238
Registered: 25-3-2014
Location: Minnesota
Member Is Offline
Mood: Triple Point
|
|
Yes, but getting/making iodoethane will be hard. I speak form experience because I have tried to synthesize iodoethane without success. ( using method
2)
https://www.erowid.org/archive/rhodium/chemistry/nitroalkane...
**edit** I suggest Starting here! https://www.youtube.com/watch?v=7Jn0z5BGpR0
[Edited on 23-3-2015 by Steam]
DISCLAIMER: The information in this post is provided for general informational purposes only and may not reflect the current law in your jurisdiction.
No information contained in this post should be construed as legal advice from the individual author, nor is it intended to be a substitute for legal
counsel on any subject matter. No reader of this post should act or refrain from acting on the basis of any information included in, or accessible
through, this post without seeking the appropriate legal or other professional advice on the particular facts and circumstances at issue from a lawyer
licensed in the recipient’s state, country or other appropriate licensing jurisdiction.
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
thanks steam! The bromoethane in the video link u posted looked easy to make
i will use that instead of iodoethane
[Edited on 23-3-2015 by Ramium]
|
|
|
CuReUS
National Hazard
Posts: 928
Registered: 9-9-2014
Member Is Offline
Mood: No Mood
|
|
won't you get a lot of quat ?
actually,there isn't much difference in reactivity of bromo and iodo compounds
you could say bromo is the poor man's(or in my opinion,the clever man's) reagent whereas iodo is for the rich and fussy
you could make iodoethane using finkelstein's reaction
http://en.wikipedia.org/wiki/Finkelstein_reaction
it would be better if you tried to make hunig's base instead.then you can use it for future reactions as well
[Edited on 24-3-2015 by CuReUS]
|
|
|
Steam
Hazard to Others
Posts: 238
Registered: 25-3-2014
Location: Minnesota
Member Is Offline
Mood: Triple Point
|
|
Nice find there CuReUs! Finkelstein is an cool name for a reaction!
I got some bromoethane and NaI, I might try to do this reaction this coming weakened!
DISCLAIMER: The information in this post is provided for general informational purposes only and may not reflect the current law in your jurisdiction.
No information contained in this post should be construed as legal advice from the individual author, nor is it intended to be a substitute for legal
counsel on any subject matter. No reader of this post should act or refrain from acting on the basis of any information included in, or accessible
through, this post without seeking the appropriate legal or other professional advice on the particular facts and circumstances at issue from a lawyer
licensed in the recipient’s state, country or other appropriate licensing jurisdiction.
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
I cant find any NaBr to make the bromoethane!!!
Pool shops here don't stock NaBr or any other bromide salt. Instead there bromine tablets are 1-bromo-3-chloro-5 5- dimethylhydantion. Is there any
way to convert this to NaBr?
Thanks
[Edited on 26-3-2015 by Ramium]
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
My new plan is to use chloroethane instead.
Could i make it using this http://youtu.be/7Jn0z5BGpR0 procedure if I substituted the NaBr for NaCl?
Chloroethane is a gas so i would bubble it through an ammonia solution to yield triethylamine.
Would that work???
|
|
|
FedeJuninArg
Harmless
Posts: 10
Registered: 31-1-2015
Member Is Offline
Mood: No Mood
|
|
Some time ago I wondered about that too.. I can't find the article I read but that reaction it's not possible.. I think because reactivity of
Chlorine.. instead you need to add a cathalyst like zinc chloride to NaCl.. find some Zinc/Carbon batteries and add the metal (well cleaned) to the
reaction flask + water to keep chlorine in solution. You can calculate the HCl excess by Redox.
With this you will prepare the HCl + cathalyst solution. Then you can add it dropwise to ethanol in a ice/water bath..
Here a ref for the reaction :
http://nepis.epa.gov/Exe/ZyNET.exe/00002EZG.txt?ZyActionD=Zy...
Good luck!
[Edited on 29-3-2015 by FedeJuninArg]
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
Thanks!
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
so I thought I'd come back and finish this project. I found the unbalanced equation online and I managed to balance it myself. have I balanced it
correctly?
NH3 + 3 C2H5Cl = (C2H5)3N + 3 HCl
so I need
NH3 = 17.031g
C2H5Cl = 64.51 x3 = 193.53g
divide by 3
NH3 = 5.677g
C2H5Cl = 64.51g
this is my plan: pour the ammonia solution into a conical flask and attach a cork with a hole in it to the top of the conical flask. push some tubing
through the hole in the cork (use glue tack to create a seal) till the end of the tubing touch's the bottom of the flask then pump the chloroethane
gas through the tubing and into the flask of ammonia solution then distil out the triethylamine. do you think this would work?
my only concern is that the HCl produced in the reaction would react with the ammonia to produce ammonium chloride.
I think I'll just buy the chloroethane rather then make it.
[Edited on 6-6-2015 by Ramium]
insoluble in society
|
|
|
byko3y
National Hazard
Posts: 721
Registered: 16-3-2015
Member Is Offline
Mood: dooM
|
|
You could order the bromide salt from some other country. Of course you will need a larger batch, but if you are going to perform multiple experiments
with halogenation, then you will need the bromide a lot.
You can use a regular ice for keeping hte EtCl liquid, but this way ethyl chloride would be quickly evaporating because of its high vapor pressure.
You gonna need to neutralize the HCl, because the alkylation can proceed only in non-acidic conditions. You should read the http://chemistry.mdma.ch/hiveboard/chemistrydiscourse/000330... if you haven't done this yet:
7EtNH2 + 5EtBr = 2Et3N + 4EtNH2.HBr + Et2NH.HBr
I think the best way to perform the reaction would be to add the ethyl chloride slowly together with an appropriate portion of alkali hydroxide. Acid
neutralization is exothermic, so your EtCl might boil because of this if not enough cooled, leading to diminishing yields.
One very important reason why the last setup you described will not work: ethyl chloride is not soluble in water, thus it will just pass to the exit
almost without reaction.
Methylamine is more volatile than triethylamine, so if you try to distill it, you will get a methylamine on exit. In case if you haven't lost your
ammonia earlier.
DMSO as a solvent might work well, it is easily alkylated by methyl halides, but ethyl halides can barely react with DMSO, although if you give them a
lot of time, like few weeks, then they will alkylate it. http://pubs.acs.org/doi/pdf/10.1021/jo01104a611
And you can't use acetonitrile as a solvent, because it catalyzes production of quaternary ammonium salt (overalkylation). Although, some quaternary
ammonium salt could catalyze the reaction even with water as solvent, but the salt has to be prepared first.
As you might understand, the temperature of the reaction will be close to 0°C, and I'm not sure whether it will proceed in any decent rate at these
conditions.
You should try to find a well developed procedure for the synthesis, because you are not capable of designing one yet.
|
|
|
Ramium
Hazard to Others
Posts: 144
Registered: 3-12-2014
Location: new zealand
Member Is Offline
Mood: Licit fish
|
|
Interesting. Thanks I hadn't read that hiveboard synth.
So if I understand correctly, the precursor ethylamine can be made in this way
ETHYLAMINE HYDROCHLORIDE
75ml of ethyl bromide plus 50ml of conc ammonia are put in a 750ml glass flask. Anhydrous ethanol is added. The flask is then immediately closed with
a rubber cork. Next the flask is put into an oven for 3 hours then allowed to cool .
The ethanol is then distilled off. The residue is next dissolved in a minimum amount of water and distilled with an excess of NaOH solution. The
distillate is collected in a flask containing dilute hydrochloric acid. The HCl distillate mixture is then evaporated until it no lounger smells of
HCl. The mixture is left to cool and after a few minutes it should solidify into a crystalline mass. This crystalline mass contains ethylamine
hydrochloride and ammonium chloride.
A mixture of diethyl ether and ethanol can then be used to extract the ammonium chloride, leaving ethylamine hydrochloride.
THE CHEMISTRY
This is what I think is going on:
The ethyl bromide reacts with the ammonia:
C2H5Br + NH3 = C2H7N + HBr
hydrobromic acid reacts with ammonia:
HBr + NH3 = NH4Br
hydrochloric acid and ethylamine react when the distillate is collected in hydrochloric acid:
HCl + C2H7N = C2H5NHCl
the distillate contains NH4Br and C2H7N so the hydrochloric acid also reacts with the NH4Br:
NH4Br + HCl = NH4Cl + HBr
Is this what happens?
sorry
[Edited on 7-6-2015 by Ramium]
[Edited on 7-6-2015 by Ramium]
insoluble in society
|
|
|
byko3y
National Hazard
Posts: 721
Registered: 16-3-2015
Member Is Offline
Mood: dooM
|
|
Alkylated amines are stronger bases than non-alkylates ones, that's they will be mostly left in a solution as a salt, while less basic amines will be
distilled away. However, this doesn't means that only one type of amine will be distilled, the dependence of composition is pretty complex.
In the quoted procedure, NaOH is added to the mixture, turning everything to free base.
And also NH4Br probably decomposes on distillation at atmospheric pressure, also, nobody is going to try that.
|
|
|
| Pages:
1
2 |
![[*]](images/xpblue/default_icon.gif){kind=icon}
