OK, you don't seem to be getting this. The reason you get energy from burning hydrocarbons is because the H-O bonds in water and C=O bonds in carbon dioxide are of a lower energy than the C-H and C-C/C=C/C?C bonds in hydrocarbons. In this case, we're already starting with the stable, low energy bonds in water, and with the
very stable, low energy forms of sodium and chloride ions dissolved in the water. The only high energy bonds in this situation are the O=O bonds in O2, but let me show you why that isn't enough.
Here are the chemical equations for the proposed situation of the RF waves reducing the sodium ions to sodium metal, the sodium metal reacting with the water to form NaOH and H2, and the H2 being burned:
1) Reduction of sodium and oxidation of chlorine (requires massive amounts of energy, btw)
Na?(aq) + Cl?(aq) --> Na + 1/2Cl?
2) Formation of NaOH and Hydrogen gas
Na + H?O --> Na? + OH? + 1/2H?
3) Combustion of Hydrogen gas
H? + 1/2O? --> H?O
Overall Reaction:
2Cl?(aq) + H?O + 1/2O? --> Cl? + 2OH?(aq)
Heat of formation for H?O: -285.830 kJ/mol
Heat of formation for Cl?
(aq): -167.4 kJ/mol
Heat of formation for OH?
(aq): -229.9 kJ/mol
Heat of formation for O? and Cl?: 0
Overall heat of reaction = 0 + 2(-229.9) - 2(-167.4) - (-285.83) - 0 =
160.83 kJ/mol <-- the reaction is
endothermic, which means it absorbs this much energy per gram-mole of reactants.
Are you
still so sure that this could work?