At 10:22 AM 10/30/2002 -0500, Alex Fraser wrote:
The devil is in the details, comments interspersed.
Pierce Nichols wrote:
Looking at the tables, I noticed a lot of metals, including silver seem to have
two oxide states where they can combine either with one or two oxygen molecules
depending on conditions. Is there any point in talking of this as far as
utility in catalyst design?
Yes, as it happens. The different oxide states will have different electron affinities and different physical properties. Although it wasn't clear to her thinking off the cuff, she thought that the metal might swap oxidization states during the two intermediate reactions. However, which one it starts out as will affect the catalytic activity.
I also wonder at the energy levels of O, O2 and O3
and what state the oxygen can exist at right after the catylization (at
pressure and temperature)? Could a metal oxide be created by O or O 3 that only
exist at high temperatures and pressures, but reverts to normal oxides when
cool? A di silver or tri silver oxide?
Actually, the reaction process is going to start by breaking peroxide into two OH groups, which will then recombine later into H2O and O2.
Of course this we want to promote, is it wetting or something more? What force here makes the peroxide want to destroy itself? In certain cases would small amounts of additives (non catalyst poisons) act to encourage the "sticking". If you sit a drop of peroxide on a piece of glass will it sit as water does (surface tension)?
The analogy is probably poorly worded. What's meant here is that the intermediate products remain fastened to the surface of the catalyst and do not move. The base catalyst begins to react when a peroxide molecule collides with the surface such that it undergoes the first intermediate reaction.
Oh this is good! I wonder what this intermediate is?
It will be some oxide/hydroxide complex of the base metal. It depends on the exact composition of the catalyst.
If the Hydrogen and Oxygen are entirely separated for a short period of time
They aren't -- peroxide is broken into two hydroxyl (OH) groups, which then recombine exothermically.
-p
Mars or Bust!
www.marssociety.com
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