Re: What form of matter will last the longest? (OT)
From: Uncle Al (UncleAl0_at_hate.spam.net)
Date: 07/19/04
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Date: Mon, 19 Jul 2004 18:21:03 -0500
Angelo wrote:
>
> Uncle Al <UncleAl0@hate.spam.net> wrote in message news:<40FB1755.82E84E8E@hate.spam.net>...
>
> (snip higher levels)
>
> > Hastelloy C-2000 (Haynes International, Inc.) Ain't near nothin'
> > chemical in the world what hits it. The easiest way to fire an
> > analytical tech is to give him a C-2000 coupon to dissolve. Good
> > luck, buddy.
> >
> > <http://www.haynesintl.com/C2000alloy/C2000folder.htm>
> > <http://members.rogers.com/acidmanual/materials_metals_c2000.htm>
> > http://www.haynesintl.com/pdf/h2111.pdf>
>
> Yes, I see it hard for an analytical tech, as you say.
> Anyway, from organic or inorganic point of view, it may come to
> mind using superacids, i.e. FSO3H--SbF5--SO3 or
> HF--SbF5, to cite the commonest (not for you Uncle Al, of course).
> Don't you think they could dissolve such a coupon of C-2000 in
> a reasonable time?
No. Look at how the alloy was designed. Nothing hits it.
Acidity by itself doesn't do anything - it's the redox
potential. You might have some luck with a strongly coordinating
ligand and bubbling air through, maybe adding a catalytic redox
couple like Cu(I,II) or Fe(II,III), but I doubt it.
316SS is physically weak and chemically reactive, but it
withstands most everything anybody commonly throws at it. Heck,
6061-T6 aluminum is all over the place, and zinc-based pot
metal. They survive. Can you even begin to imagine what
Hastelloy C-2000 will withstand? It would be a superb grave
marker if you took care of the weight (hollowed, of course) with
a proper footing.
> BTW, I have a conjecture I'd like to submit to your expert judging, as
> follows. I've seen from NIST that electron affinities of the species
> SbF6 (or SbF5-F) and AuF6 (or AuF5-F) amount, respectively, to 6
> and 10 eV. So I thought that, in view of so much energy difference,
> that a mix of AuF5 and HF (but don't know about the solubility)
> should result in a much stronger superacid.
Kinda pricey and prone to irreversible reduction.
> This may be taken with
> some confidence when realizing that extracting an electron (in the
> gas phase) from HF has an enthalpic cost very close (within 0.1 eV)
> to that for extracting a F(-) leaving a H(+). The latter, obviously,
> would attach itself to another HF molecule, gaining about 5 eV of
> proton affinity, plus a good deal of solvation energy.
> I understand that the above may be rather vague considerations, but
> I'm in a hurry at the moment and can't afford biblio-search for some
> time. And sorry for my approximate English.
PtF6 is another violently powerful electron sucker. Look what it
does to oxygen or xenon.
-- Uncle Al http://www.mazepath.com/uncleal/ (Toxic URL! Unsafe for children and most mammals) http://www.mazepath.com/uncleal/qz.pdf
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