Re: [Phys-l] Triple point pressure

[Bernard Cleyet <bernardcleyet@redshift.com>]

"There was a period of time when I was trying to dissolve some gases
(such as 3He) into cryogenic liquids (such as liquid argon) and I
observed some pretty interesting temperature-pressure phenomena that I
would not have predicted ahead of time.  Solutions, as physical chemists
would know, often behave non-ideally.  That means our customary
idealized formulas and "rule-of-thumb" don't always work (seldom
work?)with mistures."


Yes,  recently a thread discussed conductivity of mixtures and at some 
point I suspect "we've" discussed phase diagrams regarding melting 
points and crystal structure.

bc, once an "expert" on the Fe-C phase diagram (taught engineering 
materials.)

Edmiston, Mike wrote:

> I think I understand the question, but let me repeat the question a
> little differently to make sure.
>
> If we have pure H2O at 273.16 K and 611.73 kPa we can have all three
> phases present in equilibrium.  If we change the temperature or
>  
cut

> solid
> phase, and if you should be able to find a T and P that you see three
> phases present in apparent phase equilibrium, that would not be 273.16 K
> nor 611.73 kPa partial pressure of H2O.
>
> There was a period of time when I was trying to dissolve some gases
> (such as 3He) into cryogenic liquids (such as liquid argon) and I
> observed some pretty interesting temperature-pressure phenomena that I
> would not have predicted ahead of time.  Solutions, as physical chemists
> would know, often behave non-ideally.  That means our customary
> idealized formulas and "rule-of-thumb" don't always work (seldom
> work?)with mistures.
>
>
> Michael D. Edmiston, Ph.D.
> Professor of Chemistry and Physics
> Bluffton University
> Bluffton, OH 45817
> (419)-358-3270
> edmiston@bluffton.edu
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