In an electrolysis system, How do I obtain hydrogen gas from water in order to move the H2 into a free standing platinum plate?
For the electrolysis system, we may use palladium for the cathode, and platinum for the anode to break down water into hydrogen gas and oxygen.
The palladium electrode will of course be soldered to a wire to provide an electrical current, to achieve electrolysis, but our objective is not to produce palladium hydride. Our objective is to then find a way to move the hydrogen gas into a free standing platinum rod or plate, wherein the crystal lattice structure of same will break up the hydrogen gas into free protons and electrons. Once we have free protons to work with inside a conductive body of a particular length, we may then tune in to said protons to obtain fusion.
Dear Professor Jacobson,
What about two electrolysis systems running in parallel ? For example, of course, the first one must be the electrolysis of water and the second one could be a salt of platinum, for exemple chloride of platium (2+). In this case it must be expected around the cathode the precipitation of the particles of Pt containing molecules of hydrogen. Considering these 2 reactions quantitatively, as well as the analitycal methods might allow us to determine the stoichiometry of the Pt hydrade. I guess it might work, however, it require a little bit of calculus and of course, maybe the best are the carbon, respectively graphite electrodes. In the mean time, the voltage could be set as the the highest requiered for this electrolysis reaction, of course, after the Nerst's equation.
With my kindest regards,
Ioan Adrian Balea, MD
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