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I think I understand the question, but let me repeat the question acut
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
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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