Ed, I don't understand your reasoning concerning H below. The 'finger' was
filled with He, not H. The only H was in the initial 0.067 g NaH sample.
That surely cannot account for the pressures you give for the H. CRC gives a
melting point of 800 C with decompoisition. Mills DSC plot shows very
different behavior, causing wonderment at how the CRC data was obtained.Na
melts just under 100C, but this is not given as the melting point of NaH.
Robin suggests that the energy of the reactions given by Mills can saltisfy
the apparent energy to ionize the Na, initiating the catalysis. This seems
to violate causation. Can you comment on this?
Mike Carrell
----- Original Message -----
From: "Edmund Storms" <[EMAIL PROTECTED]>
To: <[email protected]>
Cc: "Edmund Storms" <[EMAIL PROTECTED]>
Sent: Monday, October 27, 2008 1:05 AM
Subject: Re: [Vo]:Sodium Hydride and Differential Scanning Calorimetry - no
Raney Nickel involved
Let's get back basics. NaH is a material that decomposes to H2 and Na
liquid containing dissolved H above 100°C. This is a process that
causes the pressure of H2 to rise as temperature is increased
according to the equation log P(atm) = 9.49-5070/T(K). As a result,
the pressure of H2 goes from 22.5 atm at 350°C to 90.5 atm at 400°,
within the region that the endothermic reaction is said to occur. At
650°, the pressure is 9932 atm, while the Na liquid contains
considerable H.
Because of this behavior, a sharp endothermic reaction is not expected
if the H2 is in equilibrium with the liquid, especially in the range
measured. However, if the loss of H2 is inhibited, the loss rate might
occur rapidly over a narrow range of temperature.
The pressure of H2 at the start of the exothermic reaction is higher
than most normal devices can take. Therefore, either the pressure was
reduced or a small amount of NaH was used so that the pressure
remained in the safe range. This means that the liquid Na contained
less dissolved H than its maximum. Unfortunately I could only find a
value for the solubility of H in Na at 450°C, which is 4 atom %. The
concentration increases with temperature.
So, the endothermic reaction appears to be caused either by a
inhibited decomposition of NaH or a reaction with the container. My
question is, what kind of material was used to contain the liquid Na
during the test?
In the BLP reactor configuration, the liquid Na might fill the pores
in the Raney Ni. Therefore, the gas would be in contact with Na
liquid. Question, is the proposed reaction occurring between the Na(H)
and Ni or between the Na(H) and H2? I don't know the partial pressure
of NaH gas, but I expect it would be very low.
What are we to conclude in light of these expected behaviors?
Ed
On Oct 26, 2008, at 8:30 PM, Jeff Driscoll wrote:
Does someone have the capability of doing a Differential Scanning
Calorimeter measurement on Sodium Hydride (NaH)? NaH can be bought
from chemical suppliers where it is sold as 60% weight NaH and 40%
weight mineral oil. The oil keeps air and water from contacting it
and chemically reacting with it. There is no Raney Nickel involved.
According to wikipedia, the oil can be rinsed off the NaH with pentane
or tetrahydrofuran.
Mills gets an exothermic reaction of 354 kJ/mole H2 (or 177 kJ/mole H)
when he put .067 grams of Sodium Hydride in the Differential Scanning
Calorimeter (reaction started at 640 C). That's 45% higher energy
than the 242 kJ/mole for burning hydrogen in air - even though the
sample volume had been flushed with helium twice before the start of
the test.
Is it possible that there was enough oxygen contamination (from
leaking or whatever) to burn with the hydrogen? Could they have
incorrectly measured the amount of NaH in their sample? If not, then
this test (when carefully done) could be a verification method of
Mills data. Just rule out oxygen contamination and weight measuring
mistakes.
Magnesium Hydride (MgH2) was used in a separate test and displayed the
predicted endothermic reaction of decompisition and endothermic
reaction of melting magnesium. Since this test didn't have oxygen
contamination issues then I would assume the NaH test didn't either.
look at page 21 here from BLP's paper regarding this differential
scanning calorimeter test:
http://www.blacklightpower.com/papers/WFC101608WebS.pdf
One thing I don't understand is that there was an endothermic reaction
at 350 C where sodium hydride decomposed before the exothermic
reaction (hydrino creation) starting at 640 C. If the sodium hydride
decomposed then all of the hydrogen has evaporated and there is no
longer a NaH molecule. According to Mike Carrell the NaH molecule is
necessary for the hydrogen shrinkage reaction because the breaking of
the bond energy between the Na and H is involved in absorbing a
portion of the 54.4 eV from the hydrogen shrinkage (along with double
ionization of Na to Na++).
Does the monatomic hydrogen released during decomposition recombine
with another H to make H2? That would prevent the hydrino reaction.
Somehow the monatomic H has to recombine with the Na to make NaH at
640 C so as to trigger the hydrino reaction.
Does this mean you could coat sodium metal onto nanoparticles and
expose them to hydrogen at 640 C and trigger the hydrino reaction?
you can read about differential scanning calorimetry here
http://en.wikipedia.org/wiki/Differential_scanning_calorimetry
Jeff D.
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