I have a science project and I have decided to find out if the amount of energy (joules) produced when combustion of hydrogen gas in air takes place. I need someone to check if there are any problems, and here is what I worked out:
Volume of Hydrogen gas (H2)collected: 51.2cm3
= 0.0000512dm3
No. of moles of H2= Volume/Molar Volume
= 0.0000512/24 (at rtp)
= 0.00000213mol
Enthalpy of Combustion forHydrogen: -286 kJ/mol
Energy produced: 286 kJ/mol x 0.00000213mol
= 0.00060918kJ (H2)
I'm also comparing it with 10 x 9volts battery, which also requires me to calculate the energy (joules) produced...
Battery (Eveready 9 Volts): 325mAh
= 0.325 Ah
Energy produced: IV = Js-1
90(0.325) = (200 x 60)-1J (in 200minutes)
29.25 = 12000-1J
J = 351000
351000J = 351kJ
∴Energy (Battery) > Energy (combustion of Hydrogengas)
Looks flawed to me, and assuming that the battery have a constant mAh throughout. Would be glad for any help given, thanks!