Hydrogen: Difference between revisions
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*Enthalpy of combustion - 286kJ/mol - [http://en.wikipedia.org/wiki/Hydrogen]. | *Enthalpy of combustion - 286kJ/mol - [http://en.wikipedia.org/wiki/Hydrogen]. | ||
:*Compare to gasoline or diesel - enthalpy of combustion of hydrogen is about 3x as large - [http://en.wikipedia.org/wiki/Heat_of_combustion] | |||
:*Wait, is that molecular and atomic hydrogen? | |||
*Hydrogen has about 1/8 and 1/3 the volumetric density, resepctively, compared to propane and natural gas. | *Hydrogen has about 1/8 and 1/3 the volumetric density, resepctively, compared to propane and natural gas. | ||
*Let's look at basic calculations. | *Let's look at basic calculations. | ||
Revision as of 06:44, 4 February 2015
- Enthalpy of combustion - 286kJ/mol - [1].
- Compare to gasoline or diesel - enthalpy of combustion of hydrogen is about 3x as large - [2]
- Wait, is that molecular and atomic hydrogen?
- Hydrogen has about 1/8 and 1/3 the volumetric density, resepctively, compared to propane and natural gas.
- Let's look at basic calculations.
- Compare to energy fuel efficiency of gasoline engin - 200 g/kWh, best marine diesel - 150 g/kWhr - [3]
Pressurized storage of hydrogen: molar mass of hydrogen molecules is 2 g/mol. 1 mole is about 5 gallons. Pressurized to 100 atm (under 1500 PSI) - readily doable with high pressure electrolyzer - you get 200 grams per 5 gallon container. Max practical for volumetric reasons would be say up to 100 gallons of 20 cu ft volume in cylindrical tanks- say 2 meters by 1 meter wide (base of a single person car). Thus, 100 gallons volume at 100 atm gets you 4 kg of hydrogen.