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The following table shows a range of estimates of the levelized costs of gray, blue, and green hydrogen, expressed in terms of US$ per kg of H 2 (where data provided in other currencies or units, the average exchange rate to US dollars in the given year are used, and 1 kg of H 2 is assumed to have a calorific value of 33.3kWh).
The energy or temperature to induce release affects the cost of any chemical storage strategy. If the hydrogen is bound too weakly, the pressure needed for regeneration is high, thereby cancelling any energy savings. The target for onboard hydrogen fuel systems is roughly <100 °C for release and <700 bar for recharge (20–60 kJ/mol H 2). [10]
The contribution of the muscle to the specific heat of the body is approximately 47%, and the contribution of the fat and skin is approximately 24%. The specific heat of tissues range from ~0.7 kJ · kg−1 · °C−1 for tooth (enamel) to 4.2 kJ · kg−1 · °C−1 for eye (sclera). [13]
At an electricity cost of $0.06/kWh, as set out in the Department of Energy hydrogen production targets for 2015, [73] the hydrogen cost is $3/kg. The US DOE target price for hydrogen in 2020 is $2.30/kg, requiring an electricity cost of $0.037/kWh, which is achievable given recent PPA tenders for wind and solar in many regions. [ 74 ]
But as a source of heat or for use in a heat engine, the relevant quantity is the change in standard enthalpy or the heat of combustion. There are two kinds of heat of combustion: The higher value (HHV), or gross heat of combustion, includes all the heat released as the products cool to room temperature and whatever water vapor is present ...
Liquid hydrogen bubbles forming in two glass flasks at the Bevatron laboratory in 1955 A large hydrogen tank in a vacuum chamber at the Glenn Research Center in Brook Park, Ohio, in 1967 A Linde AG tank for liquid hydrogen at the Museum Autovision in Altlußheim, Germany, in 2008 Two U.S. Department of Transportation placards indicating the presence of hazardous materials, which are used with ...
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The SI unit of specific heat capacity is joule per kelvin per kilogram, J⋅kg −1 ⋅K −1. [2] For example, the heat required to raise the temperature of 1 kg of water by 1 K is 4184 joules, so the specific heat capacity of water is 4184 J⋅kg −1 ⋅K −1. [3]