On Aug 10, 2007, at 10:03 AM, Jones Beene wrote:
--- Horace Heffner wrote:
Too bad the above melting point is for D2O and not
DHO.
I have not been able to find the exact melting point
for DHO, but perhaps it does not matter all that
much....
... since in any situation where there is substantial
DHO, a certain equilibrium proportion of D2O will form
naturally,
If things are in equilibrium then I think offhand you just square the
percentage of DHO to get the percentage of D2O. If the ice is 1% DHO
then it is 0.01% D2O.
However, D2O in the ice can't say at equilibrium if the melting point
of DHO is lower than for D2O. The D from a D2O can exchange with an
H from water, but the water isn't likely to give a D back to a DHO in
the ice, and the newly formed DHO will not adhere to the ice puppy
unless the temperature of the ice is below the melting point of
DHO. Once the temperature drops to the point H2O ice forms then
almost no DHO will be added in proportion. I guess the temperature
has to be just right to get nearly pure DHO ice, and there is not
much chance for D2O ice.
and that process itself is probably
accentuated by the repeated freeze/thaw cycles.
It would be interesting to harvest some of this ice
and have it run through a spectrometer.
I'll give it try this fall. I don't have a boat I can get there
with, but I'll hopefully be able to get some from shore if I can get
there the right days and the weather is right for their formation.
Horace Heffner
http://www.mtaonline.net/~hheffner/
