Protium - 12-1-2005 at 03:25
Can NiO be used as a catalyst in Hydrogenations?
If so, would it have to be affixed to activated C or something?
If so, what would be a method of such fixation?
[Edited on 12-1-2005 by Protium]
Random - 23-2-2011 at 12:43
Does someone know the answer for that? I am really interested in it.
Sedit - 23-2-2011 at 14:32
Im not 100% sure if that was the intended use or not but there is a thread around here titled seperation of Cu++ from Ni++ or something along them
lines where I posted a patent for the production of Nickle oxide on carbon. They accomplished it by mixing a water soluble Ni salt with carbon and the
precipitating the Nickle oxide onto the Carbon using (aq) Ammonia. That patent was the basis for the Nickle purification process I have been working
on.
[edit]
Heres that thread, It appears there function was to produce Nickle peroxide and you can see our dicussion on the precipitation of the Nickle in that
thread. As NotImportant pointed out in order to get the oxide instead of the hydroxide a reflux should be performed on the solution. I must say
however I would have thought elemental Nickle precipitated onto a surface would be more effective then the oxide for hydrogenation. What is the
mechanism for Nickle oxide hydrogenation, do you have a reference perhaps?
http://www.sciencemadness.org/talk/viewthread.php?tid=10527&...
[Edited on 23-2-2011 by Sedit]
Sedit - 23-2-2011 at 19:46
This states Silica as the ideal support media so with that in mind Silica gel would logically achieve a large surface area for reactions to proceed.
Nickel hydrogenation catalyst United States Patent 5258346
Attachment: US5258346.pdf (227kB)
This file has been downloaded 436 times
I love the idea of Nickle based reduction catalyst because of the simularity to Platinum group metals and the relative cheapness of it.
If I had time and a substrate to test it on I would take a Nickle salt and concentrated it as much as possible onto Silica gel, after that I would
base it with concentrated warm Ammonia. Further review of the previous thread I linked to reveiled to me that I believe the reason that I get the
hydroxide/oxide...WTF ever xide that forms from ammonia and a nickle salt instead of the complex is because you need as little water in the complex as
possible evident by the mention that it should be formed over H2SO4. Since I have been using very dilute NH3 solutions the complex just can not form
and I challenge anyone to prove me wrong because I would be very happy if you did. I have done all in my power with this dilute solution to make the
Nickle amine complex but all I get is the precipitated oxide.
This I feel would be the best means for generating a fine Nickle catalyst for the reaction you have in mind.
mnick12 - 23-2-2011 at 20:34
Sedit, it is interesting that you bring up that patent. A couple of weeks ago I was investigating a co-precipitated Cobalt, Nickel, and copper on a
solid silica support. I ended up doing this for my schools science fair, and I will post up my experiments in the next few days. You may be wondering
why I wont just post what I turned in, but I have good reason for not doing so. Alot of the report is flulff, just satisfy some of the dumb
requirements our school has. So tomorrow I will start editing my results for a SM friendly version.
Just to give you an idea of the procedure:
The procedure involves co-precipitating metal salts with sodium silicate on diatomaceous earth, then filtering the resulting precipitate and allowing
it to dry. The precipitated material is then calcined at a certain temp for a certain amount time. This is done to decompose the carbonates and
hydroxides into there oxides. Then the catalyst is reduced under an H2 atmosphere, and bla bla bla...
I will post the more detailed version later, once I get it edited.