posted on Jan, 13 2003 @ 09:13 PM
The combustion reaction of Hydrogen and Oxygen is as follows:
H2(g) + 1/2O2(g) >>> H2O(l) (Delta)H* = -286kJ
or basically it gives off 286 kilo Joules. This is 2.5 times greater than the energy produced
by combusting natural gas.
H2O(l) >>>> H2(g) + 1/2O(g) (Delta)H* = 286kJ
or basically it takes 286 kilo Joules of energy to break Hydrogen from Water into a gas, this makes sense following the first rule of conservation of
...what is the point of all this? To show you that in a PERFECT
reaction at most you break even, never do you get more energy out for what you
put in. HOWEVER!!!!! Perfect reactions are probably impossible
And more likely some energy will be wasted on producing steam.
H2O(l) >>> H2O(g) (Delta)H* = 44kJ
which means you are losing some energy in the combustion, so never can you have an infinite energy
Since the actual electrolysis of water is quite implausible, hydrogen is only a good fuel source, not a good energy source.
Energy sources that are really good are "solar power" "wind power" and such, things where you put in relatively no energy (because nature does it
for you) but you can get energy out of it.
But in hydrogen's case, you must put in the same amount of energy as you get out, so you build huge power facilities to electrolysis water into
hydrogen gas, and in effect, get a great fuel, more efficient and cleaner than Gasoline.