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So, i am trying to figure out the Thermodynamics of H2 adsorption onto a metal hydride. I need a bit of assistance if anyone knows these equations.
First off, since my MH alloy is the negative electrode in an electrolysis cell i use this equation DeltaT<(1/4D)-(Xad/x)^2 to figure out the percentage of protons on the electrode. To do any further equations i need to figure out the density of H2 ions on the surface of the Metal Hydride per 300ns.
The equations i need to do are:
MHydride reaction: M+x/2H2 <--> MHx+Q
Q=Temperature in Kilajoules/mole(g)
x= concentration of H2(moles/g)
A=Hydride forming substance
B=Non-hydride forming substance (lattice scaffold if you will)
n= atomic number of B atoms to every single A atom in the alloy alttice
Where since i am using an AB5 metal hydride the equation i need to use is ABn+(x/2)H2[@Pressure determined by the gibbs function]<---> AHx+nB+Q to figure out the overall concentration of Hydrogen into hydride state upon exposure of the 2 components (M+H2) to pressure. Different alloys require different pressures.
Once i know the thermodynamic characteristics of the particular alloy that i am working with, i can design a chamber ideal for producing the Metal Hydride reaction over many cycles. Once i know the relative H2 concentration on the cathode per pulse (each pulse being 300ns) i can figure out over, say 1 minute how much H2 migrated into the metal alloy electrode, as well as how much heat and pressure are needed to recover the H2, and to cause the MH reaction. Thus the feasibility of creating the device in-mind increases as i will know the exact parameters for the device to operate within (even under strictly ideal equations, the natural losses can be mitigated with a 5-10% scale, so increase pressure or temperature 5-10% what the equations say to make up for natural losses in the process. Whether ohmic, thermal, material etc.
First off, since my MH alloy is the negative electrode in an electrolysis cell i use this equation DeltaT<(1/4D)-(Xad/x)^2 to figure out the percentage of protons on the electrode. To do any further equations i need to figure out the density of H2 ions on the surface of the Metal Hydride per 300ns.
The equations i need to do are:
MHydride reaction: M+x/2H2 <--> MHx+Q
Q=Temperature in Kilajoules/mole(g)
x= concentration of H2(moles/g)
A=Hydride forming substance
B=Non-hydride forming substance (lattice scaffold if you will)
n= atomic number of B atoms to every single A atom in the alloy alttice
Where since i am using an AB5 metal hydride the equation i need to use is ABn+(x/2)H2[@Pressure determined by the gibbs function]<---> AHx+nB+Q to figure out the overall concentration of Hydrogen into hydride state upon exposure of the 2 components (M+H2) to pressure. Different alloys require different pressures.
Once i know the thermodynamic characteristics of the particular alloy that i am working with, i can design a chamber ideal for producing the Metal Hydride reaction over many cycles. Once i know the relative H2 concentration on the cathode per pulse (each pulse being 300ns) i can figure out over, say 1 minute how much H2 migrated into the metal alloy electrode, as well as how much heat and pressure are needed to recover the H2, and to cause the MH reaction. Thus the feasibility of creating the device in-mind increases as i will know the exact parameters for the device to operate within (even under strictly ideal equations, the natural losses can be mitigated with a 5-10% scale, so increase pressure or temperature 5-10% what the equations say to make up for natural losses in the process. Whether ohmic, thermal, material etc.