Sciencemadness Discussion Board
Not logged in [Login ]
Go To Bottom

Printable Version  
 Pages:  1  2    4    6
Author: Subject: Nitromethane, nitroethane, nitropropane synthesis via industrial route
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 3-7-2010 at 04:28


One of the pdf that S.C. Whack uploaded mentioned that during their experiements, an explosion occured when fuming nitric acid was used!

I thought that the dissolved NOx will be readily swept out by means of the hydrocarbon feed, so my plan was to use ~98w% red nitric, and bubble lighter filler gas through it, without heating the bubbler, until the nitric becomes colourless.

I poured ~250ml >98% HNO3 into a 1l bubbler, and started to feed hydrocarbon into it, after about 30min the nitric became hot to the touch (damn) and a lot of brown fumes come out of it, after one hour the bubbler was stilll hot. Unfortunately the dissolved NOx cannot be swept out so easily as I thought, so it cannot be used as it is.

The dissolved NOx oxidize the butane and heat the nitric as a result of that, more NOx forms which oxidizes more butane, so one will definitely ends up in hospital if use fuming nitric to GP nitration, hope I saved some life with this post, mine included:)

Based on my small scale experiments, I found that the vapour pressure of the cc nitric is high enough to make a HNO3 hydrocarbon mix by simply bubble the gas through the acid, and also the bursting bubbles that come up to the surface will volatilize more nitric which ensures more HNO3 in the vapour phase by which I managed to react the CH.
Now cc HNO3 cannot be used, and diluted HNO3 is sucks too because of the aforementioned. I will try to decolorize the nitric with a lil urea and pass hydrocarbon through it to see if it warms.
View user's profile View All Posts By User
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 3-7-2010 at 09:35


The nitric acid warmed after urea treatement as I'd expected, so I poured about 150ml cc H2SO4 to 100ml ccHNO3 and bubbled the CH into the mixture. Fortunately there was not any NOx produced as can be seen on the photos.. the brown was taken from pure nitric + CH, the colourless was taken from the H2SO4+HNO3 mixture, the acid mixture only slightly warmed when CH was being passed through it, so I will definitely continue the experiments with that.

Attachment: CH HNO3 mixer.doc (236kB)
This file has been downloaded 1055 times

View user's profile View All Posts By User
Melgar
Anti-Spam Agent
*****




Posts: 2004
Registered: 23-2-2010
Location: Connecticut
Member Is Offline

Mood: Estrified

[*] posted on 3-7-2010 at 13:03


When I was doing this experiment, I got an aldehyde smell when I turned up the temperature too high. Typically, it was a combination of formaldehyde and acetaldehyde. My glass tubing was either 4mm or 5mm in diameter, and I never got any violent reactions. A few times I saw jets of flame shoot through it when nitric acid would condense in the tube leading from the nitric acid bottle to the reaction tube. That would cause some liquid nitric acid to get in the reaction tube and make the flame jet.

Are you sending the nitric acid/butane mixture through a 1mm tube at any point? That could make it explode due to a buildup in pressure and the higher boiling point of butane. Propane seems like it'd be a bit safer as it would have less tendency to be in a liquid phase outside of its container.
View user's profile View All Posts By User
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 4-7-2010 at 07:00


You can avoid the small explosions by sloping the initial part of the tubing in such a way, that any condensed nitric will flow back to the bubbler. I do not think personally that is represents any danger.

As for the small diameter of the quartz tube, see attached photo:) I think that was the study of gas phase nitration on smallest scale ever, the bubbler capacity is less than 5ml, I make it explode many times, and it only made sound but did not crack.

I am currently working on implementing the cooling and protection apparatus outside of my lab, I prepare to the worst, 250ml nitric is not something that I would fuck around with carelessly.

Unfortunately lighter filler gas is my only sourse of hydrocarbons, except for some other exotics:)

Attachment: small scale.doc (89kB)
This file has been downloaded 1141 times

View user's profile View All Posts By User
Melgar
Anti-Spam Agent
*****




Posts: 2004
Registered: 23-2-2010
Location: Connecticut
Member Is Offline

Mood: Estrified

[*] posted on 4-7-2010 at 11:43


You don't have those little propane tanks for blowtorches where you are? If you have a slightly larger diameter tube, it'd probably be safer to use that, since you'd be less likely to get a pressure buildup behind the tube. That narrow tube might also have too much surface area. The literature did say a high surface area to volume ratio could cause oxidation instead of nitration, although that may depend more on the tube material.
View user's profile View All Posts By User
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 4-7-2010 at 21:40


I am going to use d=1cm glass tubing. I asked the glassblower to make it from such a long tube that eventually the tubing capacity would be about 200-250ml. I have not checked its capacity yet, and I think it does not matter, because you can adjust the temperature and the flow rate anyway. And literature suggests 0,1-20sec residence time, which means it is not that important.

I am going to adjust the temperature first, and when I get some product, continue with the flow rate.

Propane tank for blow torches are mainly contains the same gas mix, I checked it, no pure propane. but I also does not worry about that, as my goal is hydroxylamine.

Seemingly there is not much thing I worry about, there is only one, the yield :(

I foreseen that, after a number of cans I will only get 10-20ml impure product:(
View user's profile View All Posts By User
Nicodem
Super Moderator
*******




Posts: 4230
Registered: 28-12-2004
Member Is Offline

Mood: No Mood

[*] posted on 7-7-2010 at 01:02


Substrates other than alkanes can also give nitroalkanes upon radical nitration in the gas phase. For example, nitration of acetone with NO2 in the gas phase gives a mixture containing nitromethane as the only nitro compound and acetic acid as the main product (see US4517393). Even though the yield is poor, it should be safer to run than nitrations using HNO3 on alkanes, though it might not work well at 1 atm.
Furthermore, even alcohols, ethers and carboxylic acids can be nitrated in the gas phase to give nitroalkanes in most cases (see JACS, 76, 2692–2694 and references therein).
View user's profile View All Posts By User
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 7-7-2010 at 10:15


The acetone one would be nice. I am playing with the idea ever since took up this project of using alcohol, acetone and the like as a carbon source, but I am in short of image of workable setups.

My idea would be to use an Y element, one arm would be for the alcohol, and another for nitric.
Nitric acid would simply be heated by a mantle, and the acohol would be evaporated by dripping it into a heated quartz tube. Problems that I can see are that the nitric acid would be kept near its boiling point for hours, so a lot of NOx would be generated instead of HNO3 vapour.
Also the flow rate should be relatively fast at each feed to keep a constant mole ratio, so the reactants wouldnt spend much time in the hot tube which means lower reaction temp.
To keep a constant mass flow by dripping something, is also problematic.
The mixing of the two reactants at the initial stage of the hot tube would also be probably inadequate. I fear that without mixing I simply burn the nitric then pass through alcohol and water vapour.

Do you guys have some nice idea that would eliminate all these problems?
View user's profile View All Posts By User
watson.fawkes
International Hazard
*****




Posts: 2793
Registered: 16-8-2008
Member Is Offline

Mood: No Mood

[*] posted on 7-7-2010 at 11:37


Quote: Originally posted by Jimmymajesty  
Do you guys have some nice idea that would eliminate all these problems?
For constant reagent rates through a drip orifice, use peristaltic pumps with variable rate drives. This will get you close enough in ratio.

For a reaction chamber, use a long, vertical tube. Introduce alcohol vapor at the bottom and have a gas takeoff on the top that contains unreacted alcohol and all the reaction products. Introduce nitric acid through a spray nozzle at the top in very fine droplets. Collect unreacted liquid acid at the bottom of the tube. You'll might want a condenser or cold finger in the dead space below the inlet to reduce NOx vapor pressure.

I've addressed the mixing issue, in part, with the counter-current flows that this apparatus has. The reaction tube should be, at the least, insulated and probably also heated. Standard glass tube lengths from the factory are 120 cm, or about 4 feet, and I'd start with a single full length. You could use two of them in a room with high ceilings before you need to consider special building construction.
View user's profile View All Posts By User
Jimmymajesty
Hazard to Others
***




Posts: 153
Registered: 9-7-2009
Member Is Offline

Mood: No Mood

[*] posted on 12-7-2010 at 07:11


Before the large scale test I also conducted a small scale test with the H2SO4+HNO3 mix, it worked equally well again HCHO and a peculiar smell at some point.
I measured the bubbler and the gas can weight and measured them after 15 and 45 min of operation. Based on the results the CH/HNO3 mole ratio is well above infinite.. 59g propane butane mixture vaporized only one g HNO3, after the bubbler continuous HNO3 fumes were escaping though. After these experiments, I assembled the setup that can be seen in the attachment. (everything was grounded glass jointed except the connection between the two condensers).
The reactor capacity was about 200ml d=1cm. The furnace was made of two hotplates welded opposite to each other (each hotplate wattage was 1000W) and temperature controlled. The first condenser was a spiral type the second an allihn type, the first only cooled the gas mixture the second condensed back any vaporized stuff.
I poured ~150ml cc HNO3 and 150ml cc H2SO4 into the bubbler and waited till it cooled.
I started to heat up the furnace and at about 100°C I attached a CH can to the end, to flush the air out of the setup.
Then I attached the can to the front part and slightly opened it, waited till the temp of the furnace reached 380°C, at 250°C the brown fumes after the reactor tube disappeared, so probalby the flow rate was at its optimum at that temperature. At 380°C I could smell the carrot like smell again, which I think the pyrolysis products of the nitroparaffin, so I set back the SP of the controller to 350°C and adjusted the CH flow in such a way, that the brown fumes had just disappeared. At this point a peculiar smell could be noticed at the outlet of the second condenser, It was like isopropyl nitrite, a condensate is started to drip into the flask of the first condenser, with a rate about one drop/25 sec. The condensate separated into two phase, but they reacted with each other since the bottom of the flask warmed. This was probably due to the formed HCHO and HNO3 made it at the heating up period into the first receiver flask.
After about 30min I sucked up the condensate from the first flask with a syringe, then washed with water, and smelled, its smell was between menthol and nitro toluene, or rather between paraldehyde and nitro toluene, it was a pleasant smell.
In the second receiver flask only oxidized organic stuff was present which were completely dissolved upon addition of water.
I lit a couple of drops with open flame and it burned with a nice grey colour.
I do not recommend to reproduce this experiment, since it is low yielding, especially at these circumstances. It was only good for get some product to smell it.. I did not heat the bubbler though, by which I think I could attain better results. The explosion hazard problem should be solved by lowering the bubbler head space to zero without HNO3 droplets being sprayed into the hot tube, any ideas on this?
BTW the HNO3+H2SO4 mixture, also heated on its own, it was at about 35°C at the end of the experiment, also I do not think that the nitric could be regenerated from the mixture, I suscpect that there is a lot of semi oxidised CH crap in the mixture that would cause serious frothing upon heating.
Watson interesting approach:) I tried that too, but how can you make an even spray, that will be volatilized before falling into the high temp CH vapours? Its seems to be a problem that only industrial bastards can solve over a designer table, I took a 1m long quartz tube and wounded some kanthal wire to the bottom, then I heated the bottom and slowly flooded the bottom of the tube, in such a way that a reflux of CH developed, (I could only hold this state for a min though, then overflow, etc.) during that short time I tried to drip, spray, pour HNO3 into the tube but this always resulted in a cracking noise & barking dog sound..

Attachment: GP nitration exp setup.doc (265kB)
This file has been downloaded 1033 times

View user's profile View All Posts By User
zed
International Hazard
*****




Posts: 2284
Registered: 6-9-2008
Location: Great State of Jefferson, City of Portland
Member Is Offline

Mood: Semi-repentant Sith Lord

[*] posted on 12-7-2010 at 12:26


Considering that the industrial methods usually employed are pretty tough to conduct with home made stuff... Once again, I might consider some alternative.

IF Shulgins procedure for de-constructing the B-Nitro-propene to produce Myristicin Aldehyde and Nitroethane is applicable. Then, the nitration of styrene with I2/NaNo2, in ethylene glycol, to produce B-Nitrostyrene....might be a good starting point, to produce Nitromethane and Benzaldehyde.

I can easily and cheaply obtain all of the ingredients, and solvents. And, the yield of Beta-Nitrostyrene is purported to be about 80%.

With luck, refluxing the resultant B-Nitro-Styrene with N-Methyl Benzylamine will produce the Benzaldehyde-imine.....Plus very pure Nitromethane as gas.

High grade Nitromethane, and an equivalent amount of Benzaldehyde should be recovered (After performing hydrolysis on the imine). I can also recover and recycle my Iodine and N-Methyl-Benzylamine.

Likewise, if this Nitration could be performed successfully on Iso-Eugenol , The deconstructed Nitropropene would yield Vanillin and Nitroethane. I'm not sure if this nitration can be performed on Iso-Eugenol.....Maybe not.

http://www.erowid.org/archive/rhodium/chemistry/nitryliodide...

[Edited on 12-7-2010 by zed]

[Edited on 12-7-2010 by zed]

[Edited on 12-7-2010 by zed]
View user's profile View All Posts By User
madcedar
Hazard to Others
***




Posts: 116
Registered: 10-9-2009
Member Is Offline

Mood: No Mood

[*] posted on 19-9-2010 at 00:11
Nitroethane from ethanol and nitric acid


Since you are in the mood for experimentation here is a patent for making nitroethane from ethanol and nitric acid (and other useful information). :P

Attachment: nitroethane pat4431842 (ethanol and nitric acid).pdf (257kB)
This file has been downloaded 2258 times

Attachment: Nitroethane, Properties and Azeotropes.pdf (139kB)
This file has been downloaded 1954 times

Attachment: Nitroethane, Purification by Azeotropic Distillation US3480517.pdf (118kB)
This file has been downloaded 1190 times
View user's profile View All Posts By User
arsphenamine
Hazard to Others
***




Posts: 236
Registered: 12-8-2010
Location: I smell horses, Maryland, USA
Member Is Offline

Mood: No Mood

[*] posted on 19-9-2010 at 17:10


Quote: Originally posted by zed  
IF Shulgins procedure for de-constructing the B-Nitro-propene to produce Myristicin Aldehyde and Nitroethane is applicable. Then, the nitration of styrene with I2/NaNo2, in ethylene glycol, to produce B-Nitrostyrene....might be a good starting point, to produce Nitromethane and Benzaldehyde.


Maybe I'm too easily amused, but the thought of a "reverse Henry Reaction" is chortle producing.

Here someone has a perfectly good illicit precursor and they want to disproportionate it back into Henry reactants.
View user's profile View All Posts By User
stygian
Hazard to Others
***




Posts: 242
Registered: 19-9-2004
Member Is Offline

Mood: No Mood

[*] posted on 19-9-2010 at 17:17


It's a more interesting idea if you could make it work with 2-nitropropene.. and fancied working with 2-nitropropene
View user's profile View All Posts By User
zed
International Hazard
*****




Posts: 2284
Registered: 6-9-2008
Location: Great State of Jefferson, City of Portland
Member Is Offline

Mood: Semi-repentant Sith Lord

[*] posted on 20-9-2010 at 01:33


Ummmm. Well, P-Propenyl anisole and Iso-Eugenol, are inexpensive and fairly worthless as precursors.

Using them to generate, difficult to obtain Nitroethane, ala Shulgin....has some merit.

Additionally , Vanillin and Anisaldehyde, have their own uses.

Shulgin ripping apart the MMDA skeleton to produce Myristicin Aldehyde, may seem
crazy to us, but it suited his goal. And, it served to reveal a potential Nitroethane synthesis, that could prove very handy in this era when Nitroethane is very tough to come by.

View user's profile View All Posts By User
Waffles SS
Fighter
****




Posts: 998
Registered: 7-12-2009
Member Is Offline


[*] posted on 1-1-2011 at 12:35



Quote:

Nitromethane can be prepared by the action of dimethyl sulfate on potassium nitrite
Walden, Ber. 40, 3216 (1907)

http://www.orgsyn.org/orgsyn/prep.asp?prep=cv1p0401

Anyone know detail of this reaction?
View user's profile View All Posts By User
franklyn
International Hazard
*****




Posts: 3026
Registered: 30-5-2006
Location: Da Big Apple
Member Is Offline

Mood: No Mood

[*] posted on 4-1-2011 at 19:35


Quote: Originally posted by Waffles SS  
Nitromethane can be prepared by the action of dimethyl sulfate on potassium nitrite
Walden, Ber. 40, 3216 (1907)

Anyone know detail of this reaction?

read second half here
http://www.sciencemadness.org/talk/viewthread.php?tid=13633&...
A good reason not to make that way
http://www.sciencemadness.org/talk/viewthread.php?tid=1608&a...

http://www.sciencemadness.org/talk/viewthread.php?tid=1608
http://www.sciencemadness.org/talk/viewthread.php?tid=2995
http://www.sciencemadness.org/talk/viewthread.php?tid=9570

.
View user's profile View All Posts By User
MeSynth
Hazard to Others
***




Posts: 107
Registered: 29-7-2011
Member Is Offline

Mood: http://www.youtube.com/watch?v=5ZltqlVuDIo

[*] posted on 30-8-2011 at 20:25


Quote: Originally posted by 497  
This patent might be interesting to some here. It is a patent that gives the conditions to produce a mixture of 83% nitroethane and 17% nitromethane by vapor phase nitration of propyl nitrite with 50% HNO3 vapor at 400*C (or NO2 at 300*C), at atmospheric pressure. Interestingly, they use an aluminum tube immersed in a molten salt as the reactor. It is advantageous because it results in a simpler mixture of products that should be much easier to purify... Assuming you can get n-propyl alcohol, propyl nitrite is ultra easy to synthesize.. The extra carbon is lost as formaldehyde. If you wanted nice pure nitromethane, you could use isopropyl nitrite instead, which results in only nitromethane (and acetaldehyde byproduct).

[Edited on 18-6-2010 by 497]


US3209038

I have tried to work out how this would be done. Saftey is a major issue due to n-propyl nitrite being an explosive. Due to the explosive nature of the reactants I would not hand operate this and would rather operate the air pump from behind a concrete wall. Other than this explosion hazard I feel no threat and have drawn out the first part and the second leaving out the n-propyl nitrite stage since I'm not certain about what they mean in the patent when they say the n-propyl nitrite was allowed to enter a stream of 50% nitric acid vapor that has been preheated to 260* C. The pictures have been added as attachments.

My best guess is small amounts of n-propyl nitrite will boil out when the nitric acid vapor heated to 260* C. is passed through causing just the right amount to vaporize and mix with the gas.

The missing stage is where the nitric acid combines with the n-propyl nitrite before entering the reactor.

1.png - 9kB 2.png - 7kB
View user's profile View All Posts By User
497
National Hazard
****




Posts: 778
Registered: 6-10-2007
Member Is Offline

Mood: HSbF6

[*] posted on 31-8-2011 at 01:55


PrONO has a terrible oxygen balance on its own, it would be tough if not impossible to detonate in my opinion. Mixing it with HNO3 would improve the OB and sensitivity no doubt, but it shouldn't be hard to avoid that fully by using an inert gas to dilute the gas mixture. Concrete walls are always a good precaution though if you have them. It shouldn't much need hands on attention anyway.

I'm not certain, but I would bet that the mixture of HNO3, H2O and RONO proposed in the patent forms an equilibrium with ROH, NO, and NO2 via 2RONO + H2O <---> 2ROH + NO + NO2.

Since NO2 can be formed from air by electric discharge pretty easily, you might be able to have a continous process where the output from the electric discharge is fed into an absorption column/bubbler filled with liquid ROH + H2O. These react to form RONO + HNO3, at least until too much HNO3 builds up. Then the ROH + RONO + HNO3 + H2O from the NO2 absorber is dripped into a vaporizer and piped into you reactor tube. Supplemental HNO3 could also be added from a separate NO2 absorber filled with only H2O if need be. HNO3 recycled back from the product mixture would likely be sufficient though.

Electricity, air, water, and an alcohol in, nitroalkanes and aldehydes of your choice out. Sound pretty elegant to me. The inert gas could hopefully be recycled. CO2 is pretty cheap though. I'd be interested in using it for both the acetaldehyde + nitromethane, and the formaldehyde + nitroethane possibilities.

Not sure about the best ways to process the end mixture of HNO3, ROH, water, nitroalkanes and aldehyde(s). Nitroethane does form azeotropes with n-propanol and water for sure. Maybe an extractive distillation could help?

What do you think?




A word to the wise: NEUROFEEDBACK

http://citizenworks.org/corp/dg/s2r1.pdf
http://www.newscientist.com/mobile/article/mg21228354.500-re...
http://www.shadowstats.com/article/no-414-hyperinflation-spe...

"To expose a 15 Trillion dollar ripoff of the American people by the stockholders of the 1000 largest corporations over the last 100 years will be a tall order of business."
Buckminster Fuller

"No problem can be solved from the same level of consciousness that created it."
Albert Einstein
View user's profile View All Posts By User
AndersHoveland
Hazard to Other Members, due to repeated speculation and posting of untested highly dangerous procedures!
*****




Posts: 1986
Registered: 2-3-2011
Member Is Offline

Mood: No Mood

[*] posted on 21-9-2011 at 23:46


The vapor phase nitration of propane with nitric acid at 420degC produces various nitroalkanes in 40% yield total.
The yield for nitromethane is only 4%, for nitroethane 10%, for 2-Nitropropane the yield is 16%.
The various nitroalkanes are then separated by distillation. Nitromethane boils off first at 101degC, then nitroethane at 114degC. The vapor-phase nitration can alternatively be done with nitrogen dioxide, giving better yields, with the additional advantage that the products contain less 2-nitropropane.

2-Nitropropane boils at 120degC. 1-Nitropropane boils at 131degC. 2-Nitropropane is a carcinogen, breathing of its vapor should be avoided.


[Edited on 22-9-2011 by AndersHoveland]
View user's profile Visit user's homepage View All Posts By User
497
National Hazard
****




Posts: 778
Registered: 6-10-2007
Member Is Offline

Mood: HSbF6

[*] posted on 22-9-2011 at 03:47


I don't see how effective separation of of nitromethane, nitroethane, and nitropropanes can be accomplished with their boiling points all being within 30 degrees of each other.. Even worse is that nitroethane and 2-nitropropane are within 6 degrees or each other.. I think a method that produces nitroethane more selectively would be much more useful. Unless there is a magic bullet way to purify it?



A word to the wise: NEUROFEEDBACK

http://citizenworks.org/corp/dg/s2r1.pdf
http://www.newscientist.com/mobile/article/mg21228354.500-re...
http://www.shadowstats.com/article/no-414-hyperinflation-spe...

"To expose a 15 Trillion dollar ripoff of the American people by the stockholders of the 1000 largest corporations over the last 100 years will be a tall order of business."
Buckminster Fuller

"No problem can be solved from the same level of consciousness that created it."
Albert Einstein
View user's profile View All Posts By User
simba
Hazard to Others
***




Posts: 175
Registered: 20-5-2011
Member Is Offline

Mood: No Mood

[*] posted on 22-9-2011 at 07:53


Quote: Originally posted by 497  
I don't see how effective separation of of nitromethane, nitroethane, and nitropropanes can be accomplished with their boiling points all being within 30 degrees of each other.. Even worse is that nitroethane and 2-nitropropane are within 6 degrees or each other.. I think a method that produces nitroethane more selectively would be much more useful. Unless there is a magic bullet way to purify it?


Maybe they can be purified by freezing...nitromethane freezes at −29 °C, nitroethane at -90 °C, and I don't know about nitropropanes.
View user's profile View All Posts By User
AndersHoveland
Hazard to Other Members, due to repeated speculation and posting of untested highly dangerous procedures!
*****




Posts: 1986
Registered: 2-3-2011
Member Is Offline

Mood: No Mood

[*] posted on 22-9-2011 at 11:30


It might be better to do a vapor phase nitration using ethane, or possibly even methane (natural gas), to avoid formation of hazardous 2-nitropropane.

Typically, when two similar compounds have very close boiling points, the mixture needs to be distilled several times repeatedly. This can generally minimize impurities in the separated compounds.

For example, the portion that initially distills off from a mixture of nitromethane and nitroethane would be redistilled again, and the portion that distills off from the second distillation would be nearly pure nitromethane, although some of the nitromethane got left behind with the nitroethane.

The industrial process only uses propane because nitroethane, which is used as an industrial solvent, actually sells for a higher price than nitromethane. Nitromethane is considered the byproduct.

[Edited on 22-9-2011 by AndersHoveland]
View user's profile Visit user's homepage View All Posts By User
Alastair
Hazard to Self
**




Posts: 59
Registered: 13-7-2011
Member Is Offline

Mood: Barely any solvent in my emulsion

[*] posted on 25-9-2011 at 01:23


''For example, sodium (nitrite) and potassium nitrite reacting with iodomethane would produce mostly nitromethane, with methyl nitrite as the minor product''
Source: wikipedia. ref: Donald L. Pavia, Gary M. Lampman, George S. Kriz (2004). Organic Chemistry. 2. Mason, Ohio: Thompson Custom Publishing. ISBN 0030148138. OCLC 236055357 But i couldnt find the ref.

Could this be applied to iodoethane?
Or maybe nitroethane can be separated as a side product from nitrite syntheses via alcohols + NaNO2 (or N2O3) ?
View user's profile View All Posts By User
simba
Hazard to Others
***




Posts: 175
Registered: 20-5-2011
Member Is Offline

Mood: No Mood

[*] posted on 25-9-2011 at 09:41


Quote: Originally posted by Alastair  
''For example, sodium (nitrite) and potassium nitrite reacting with iodomethane would produce mostly nitromethane, with methyl nitrite as the minor product''
Source: wikipedia. ref: Donald L. Pavia, Gary M. Lampman, George S. Kriz (2004). Organic Chemistry. 2. Mason, Ohio: Thompson Custom Publishing. ISBN 0030148138. OCLC 236055357 But i couldnt find the ref.

Could this be applied to iodoethane?
Or maybe nitroethane can be separated as a side product from nitrite syntheses via alcohols + NaNO2 (or N2O3) ?


yeah...iodoethane or any other haloethane will yield nitroethane.
View user's profile View All Posts By User
 Pages:  1  2    4    6

  Go To Top