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TO HELP W/ THE DEBATE ON HYDROGEN/OXYGEN PRODUCTION DURING ELECTROLYSIS:
This is what my Thermodynamics Book says (Fundementals of Engineering Thermodynamics):
There are 2.016 kg/kmol of H2
32.00 kg/kmol of O2
Wikipedia - Hydrogen @ 0 degrees Celcius (32 degrees F) & 1 atm
H2 - 0.08988 g/L or 0.00008988 kg/L
Wikipedia - Oxygen @ 0 degrees Celcius (32 degrees F) & 1 atm
O2 - 1.429 g/L or 0.001428 kg/L
or
H2 - 11126 L/kg
O2 - 700 L/kg
Since there are 2kmol of H2 per kmol of O2:
4.032 kg H2
32.00 kg O2
in 36.032 kg H2O
Multiplying through:
44860 L of H2
22400 L of O2
Determining the ratio:
44860/(44860+22400) = .667 = 66.7% Hydrogen
100% - 66.7% = 33.3% Oxygen
TO CONCLUDE: There should be 2x as much gaseous Hydrogen after electrolysis than Oxygen.
If my math is faulted please correct me.
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