Energy density

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Template:Short description Template:Infobox physical quantity

In physics, energy density is the quotient between the amount of energy stored in a given system or contained in a given region of space and the volume of the system or region considered. Often only the useful or extractable energy is measured. It is sometimes confused with stored energy per unit mass, which is called specific energy or Template:Em.

There are different types of energy stored, corresponding to a particular type of reaction. In order of the typical magnitude of the energy stored, examples of reactions are: nuclear, chemical (including electrochemical), electrical, pressure, material deformation or in electromagnetic fields. Nuclear reactions take place in stars and nuclear power plants, both of which derive energy from the binding energy of nuclei. Chemical reactions are used by organisms to derive energy from food and by automobiles from the combustion of gasoline. Liquid hydrocarbons (fuels such as gasoline, diesel and kerosene) are today the densest way known to economically store and transport chemical energy at a large scale (1 kg of diesel fuel burns with the oxygen contained in ≈ 15 kg of air). Burning local biomass fuels supplies household energy needs (cooking fires, oil lamps, etc.) worldwide. Electrochemical reactions are used by devices such as laptop computers and mobile phones to release energy from batteries.

Energy per unit volume has the same physical units as pressure, and in many situations is synonymous. For example, the energy density of a magnetic field may be expressed as and behaves like a physical pressure. The energy required to compress a gas to a certain volume may be determined by multiplying the difference between the gas pressure and the external pressure by the change in volume. A pressure gradient describes the potential to perform work on the surroundings by converting internal energy to work until equilibrium is reached.

In cosmological and other contexts in general relativity, the energy densities considered relate to the elements of the stress–energy tensor and therefore do include the rest mass energy as well as energy densities associated with pressure.

Chemical energy

When discussing the chemical energy contained, there are different types which can be quantified depending on the intended purpose. One is the theoretical total amount of thermodynamic work that can be derived from a system, at a given temperature and pressure imposed by the surroundings, called exergy. Another is the theoretical amount of electrical energy that can be derived from reactants that are at room temperature and atmospheric pressure. This is given by the change in standard Gibbs free energy. 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 condenses.
  • The lower value (LHV), or net heat of combustion, does not include the heat which could be released by condensing water vapor, and may not include the heat released on cooling all the way down to room temperature.

A convenient table of HHV and LHV of some fuels can be found in the references.[1]

In energy storage and fuels

Selected energy densities plot[2][3][4][5][6][7][8]

For energy storage, the energy density relates the stored energy to the volume of the storage equipment, e.g. the fuel tank. The higher the energy density of the fuel, the more energy may be stored or transported for the same amount of volume. The energy of a fuel per unit mass is called its specific energy.

The adjacent figure shows the gravimetric and volumetric energy density of some fuels and storage technologies (modified from the Gasoline article). Some values may not be precise because of isomers or other irregularities. The heating values of the fuel describe their specific energies more comprehensively.

The density values for chemical fuels do not include the weight of the oxygen required for combustion. The atomic weights of carbon and oxygen are similar, while hydrogen is much lighter. Figures are presented in this way for those fuels where in practice air would only be drawn in locally to the burner. This explains the apparently lower energy density of materials that contain their own oxidizer (such as gunpowder and TNT), where the mass of the oxidizer in effect adds weight, and absorbs some of the energy of combustion to dissociate and liberate oxygen to continue the reaction. This also explains some apparent anomalies, such as the energy density of a sandwich appearing to be higher than that of a stick of dynamite.

Given the high energy density of gasoline, the exploration of alternative media to store the energy of powering a car, such as hydrogen or battery, is strongly limited by the energy density of the alternative medium. The same mass of lithium-ion storage, for example, would result in a car with only 2% the range of its gasoline counterpart. If sacrificing the range is undesirable, much more storage volume is necessary. Alternative options are discussed for energy storage to increase energy density and decrease charging time, such as supercapacitors.[9][10][11][12]

No single energy storage method boasts the best in specific power, specific energy, and energy density. Peukert's law describes how the amount of useful energy that can be obtained (for a lead-acid cell) depends on how quickly it is pulled out.

Efficiency

In general an engine will generate less kinetic energy due to inefficiencies and thermodynamic considerations—hence the specific fuel consumption of an engine will always be greater than its rate of production of the kinetic energy of motion.

Energy density differs from energy conversion efficiency (net output per input) or embodied energy (the energy output costs to provide, as harvesting, refining, distributing, and dealing with pollution all use energy). Large scale, intensive energy use impacts and is impacted by climate, waste storage, and environmental consequences.

Nuclear energy

The greatest energy source by far is matter itself, according to the mass–energy equivalence. This energy is described by Template:Nowrap, where c is the speed of light. In terms of density, Template:Nowrap, where ρ is the volumetric mass density, V is the volume occupied by the mass. This energy can be released by the processes of nuclear fission (~ 0.1%), nuclear fusion (~ 1%), or the annihilation of some or all of the matter in the volume V by matter–antimatter collisions (100%).Template:Citation needed

The most effective ways of accessing this energy, aside from antimatter, are fusion and fission. Fusion is the process by which the sun produces energy which will be available for billions of years (in the form of sunlight and heat). However as of 2024, sustained fusion power production continues to be elusive. Power from fission in nuclear power plants (using uranium and thorium) will be available for at least many decades or even centuries because of the plentiful supply of the elements on earth,[13] though the full potential of this source can only be realized through breeder reactors, which are, apart from the BN-600 reactor, not yet used commercially.[14]

Fission reactors

Nuclear fuels typically have volumetric energy densities at least tens of thousands of times higher than chemical fuels. A 1 inch tall uranium fuel pellet is equivalent to about 1 ton of coal, 120 gallons of crude oil, or 17,000 cubic feet of natural gas.[15] In light-water reactors, 1 kg of natural uranium – following a corresponding enrichment and used for power generation– is equivalent to the energy content of nearly 10,000 kg of mineral oil or 14,000 kg of coal.[16] Comparatively, coal, gas, and petroleum are the current primary energy sources in the U.S.[17] but have a much lower energy density.

The density of thermal energy contained in the core of a light-water reactor (pressurized water reactor (PWR) or boiling water reactor (BWR)) of typically Template:Val (Template:Val electrical corresponding to ≈ Template:Val thermal) is in the range of 10 to 100 MW of thermal energy per cubic meter of cooling water depending on the location considered in the system (the core itself (≈ Template:Val), the reactor pressure vessel (≈ Template:Val), or the whole primary circuit (≈ Template:Val)). This represents a considerable density of energy that requires a continuous water flow at high velocity at all times in order to remove heat from the core, even after an emergency shutdown of the reactor.

The incapacity to cool the cores of three BWRs at Fukushima after the 2011 tsunami and the resulting loss of external electrical power and cold source caused the meltdown of the three cores in only a few hours, even though the three reactors were correctly shut down just after the Tōhoku earthquake. This extremely high power density distinguishes nuclear power plants (NPP's) from any thermal power plants (burning coal, fuel or gas) or any chemical plants and explains the large redundancy required to permanently control the neutron reactivity and to remove the residual heat from the core of NPP's.

Antimatter–matter annihilation

Because antimatter–matter interactions result in complete conversion of the rest mass to radiant energy, the energy density of this reaction depends on the density of the matter and antimatter used. A neutron star would approximate the most dense system capable of matter-antimatter annihilation. A black hole, although denser than a neutron star, does not have an equivalent anti-particle form, but would offer the same 100% conversion rate of mass to energy in the form of Hawking radiation. Even in the case of relatively small black holes (smaller than astronomical objects) the power output would be tremendous.

Electric and magnetic fields

Template:Main

Electric and magnetic fields can store energy and its density relates to the strength of the fields within a given volume. This (volumetric) energy density is given by u=ε2𝐄2+12μ𝐁2 where Template:Math is the electric field, Template:Math is the magnetic field, and Template:Mvar and Template:Mvar are the permittivity and permeability of the surroundings respectively. The SI unit is the joule per cubic metre.

In ideal (linear and nondispersive) substances, the energy density is u=12(𝐄⋅𝐃+𝐇⋅𝐁) where Template:Math is the electric displacement field and Template:Math is the magnetizing field. In the case of absence of magnetic fields, by exploiting Fröhlich's relationships it is also possible to extend these equations to anisotropic and nonlinear dielectrics, as well as to calculate the correlated Helmholtz free energy and entropy densities.[18]

In the context of magnetohydrodynamics, the physics of conductive fluids, the magnetic energy density behaves like an additional pressure that adds to the gas pressure of a plasma.

Pulsed sources

When a pulsed laser impacts a surface, the radiant exposure, i.e. the energy deposited per unit of surface, may also be called energy density or fluence.[19]

Table of material energy densities

Template:See also Template:Self-contradictory Template:Unreliable sources The following unit conversions may be helpful when considering the data in the tables: 3.6 MJ = 1 kW⋅h ≈ 1.34 hp⋅h. Since 1 J = 10−6 MJ and 1 m3 = 103 L, divide joule/m3 by 109 to get MJ/L = GJ/m3. Divide MJ/L by 3.6 to get kW⋅h/L.

Chemical reactions (oxidation)

Template:See also Unless otherwise stated, the values in the following table are lower heating values for perfect combustion, not counting oxidizer mass or volume. When used to produce electricity in a fuel cell or to do work, it is the Gibbs free energy of reaction (ΔG) that sets the theoretical upper limit. If the produced Template:H2O is vapor, this is generally greater than the lower heat of combustion, whereas if the produced Template:Chem is liquid, it is generally less than the higher heat of combustion. But in the most relevant case of hydrogen, ΔG is 113 MJ/kg if water vapor is produced, and 118 MJ/kg if liquid water is produced, both being less than the lower heat of combustion (120 MJ/kg).[20] Template:Table alignment Template:Sticky header

Energy released by chemical reactions (oxidation)
Material Specific energy
(MJ/kg) 		Energy density
(MJ/L) 		Specific energy
(W⋅h/kg) 		Energy density
(W⋅h/L) 		Comment
Hydrogen, liquid 141.86 (HHV)
119.93 (LHV) 		10.044 (HHV)
8.491 (LHV) 		Template:Val (HHV)
33,313.9 (LHV) 		Template:Val (HHV)
2,358.6 (LHV) 		Energy figures apply after reheating to 25 °C.[21]

See note above about use in fuel cells.

Hydrogen, gas (681 atm, 69 MPa, 25 °C) 141.86 (HHV)
119.93 (LHV) 		5.323 (HHV)
4.500 (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		Data from same reference as for liquid hydrogen.[21]

High-pressure tanks weigh much more than the hydrogen they can hold. The hydrogen may be around 5.7% of the total mass,[22] giving just 6.8 MJ per kg total mass for the LHV.

See note above about use in fuel cells.

Hydrogen, gas (Template:Cvt, 25 °C) 141.86 (HHV)
119.93 (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		3.3 (HHV)
2.8 (LHV) 		[21]
Diborane 78.2 88.4 Template:Val Template:Val [23]
Beryllium 67.6 125.1 Template:Val Template:Val
Lithium borohydride 65.2 43.4 Template:Val Template:Val
Boron 58.9 137.8 Template:Val Template:Val [24]Template:Better source needed
Methane (101.3 kPa, 15 °C) 55.6 Template:Val Template:Val 10.5
LNG (NG at −160 °C) 53.6[25] 22.2 Template:Val Template:Val
CNG (NG compressed to 247 atm, 25 MPa ≈ Template:Val) 53.6[25] 9 Template:Val Template:Val
Natural gas 53.6[25] Template:Val Template:Val 10.1
LPG propane 49.6 25.3 Template:Val Template:Val [26]
LPG butane 49.1 27.7 Template:Val Template:Val [26]
Petrol (Gasoline) 46.4 34.2 Template:Val Template:Val [26]
Polypropylene plastic 46.4[27] 41.7 Template:Val Template:Val
Polyethylene plastic 46.3[27] 42.6 Template:Val Template:Val
Residential heating oil 46.2 37.3 Template:Val Template:Val [26]
Diesel fuel 45.6 38.6 Template:Val Template:Val [26]
100LL Avgas 44.0[28] 31.59 Template:Val Template:Val
Jet fuel (e.g. kerosene) 43[29][30][31] 35 Template:Val Template:Val aircraft engine
Gasohol E10 (10% ethanol 90% gasoline by volume) 43.54 33.18 Template:Val Template:Val
Lithium 43.1 23.0 Template:Val Template:Val
Biodiesel oil (vegetable oil) 42.20 33 11,722.2 9,166.7
DMF (2,5-dimethylfuran) 42[32] 37.8 11,666.7 10,500.0 Template:Clarify
Paraffin wax 42[33] 37.8 Template:Val Template:Val
Crude oil (tonne of oil equivalent) 41.868 37[25] Template:Val Template:Val
Polystyrene plastic 41.4[27] 43.5 Template:Val Template:Val
Body fat 38 35 Template:Val Template:Val metabolism in human body (22% efficiency[34])
Butanol 36.6 29.2 Template:Val Template:Val
Gasohol E85 (85% ethanol 15% gasoline by volume) 33.1 25.65Template:Citation needed Template:Val Template:Val
Graphite 32.7 72.9 Template:Val Template:Val
Coal, anthracite 26–33 34–43 Template:Val–Template:Val Template:Val–Template:Val Figures represent perfect combustion not counting oxidizer, but efficiency of conversion to electricity is ≈36%[5]
Silicon 32.6 75.9 9,056 21,080 See Table 1 [35]
Aluminium 31.0 83.8 Template:Val Template:Val
Ethanol 30 24 Template:Val Template:Val
DME 31.7 (HHV)
28.4 (LHV) 		21.24 (HHV)
19.03 (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		Template:Val (HHV)
Template:Val (LHV) 		[36][37]
Polyester plastic 26.0[27] 35.6 Template:Val Template:Val
Magnesium 24.7 43.0 Template:Val 11,944.5
Phosphorus (white) 24.30 44.30 Template:Val Template:Val [38]
Coal, bituminous 24–35 26–49 Template:Val–Template:Val Template:Val–Template:Val [5]
PET plastic (impure) 23.5[39] < ~32.4 Template:Val < ~Template:Val
Methanol 19.7 15.6 Template:Val Template:Val
Titanium 19.74 88.93 Template:Val Template:Val burned to titanium dioxide
Hydrazine 19.5 19.3 Template:Val Template:Val burned to nitrogen and water
Liquid ammonia 18.6 11.5 Template:Val Template:Val burned to nitrogen and water
Potassium 18.6 16.5 Template:Val Template:Val burned to dry potassium oxide
PVC plastic (improper combustion toxic) 18.0[27] 25.2 Template:Val Template:Val Template:Clarify
Wood 18.0 Template:Val [40]
Peat briquette 17.7 Template:Val [41]
Sugars, carbohydrates, and protein 17 26.2 (dextrose) Template:Val Template:Val metabolism in human body (22% efficiency[42])Template:Citation needed
Calcium 15.9 24.6 Template:Val Template:Val Template:Citation needed
Glucose 15.55 23.9 Template:Val Template:Val
Dry cow dung and camel dung 15.5[43] Template:Val
Coal, lignite 10–20 Template:Val–Template:Val Template:Citation needed
Sodium 13.3 12.8 Template:Val Template:Val burned to wet sodium hydroxide
Peat 12.8 3,555.6
Nitromethane 11.3 12.85 Template:Val Template:Val
Manganese 9.46 68.2 Template:Val Template:Val burned to manganese dioxide
Sulfur 9.23 19.11 Template:Val Template:Val burned to sulfur dioxide[44]
Sodium 9.1 8.8 Template:Val Template:Val burned to dry sodium oxide
Household waste 8.0[45] Template:Val
Iron 7.4 57.7 Template:Val Template:Val burned to iron(III) oxide[46]
Iron 6.7 52.2 Template:Val Template:Val burned to Iron(II,III) oxide[46]
Zinc 5.3 38.0 Template:Val Template:Val
Teflon plastic 5.1 11.2 Template:Val Template:Val combustion toxic, but flame retardant
Iron 4.9 38.2 Template:Val Template:Val burned to iron(II) oxide[46]
Gunpowder 4.7–11.3[47] 5.9–12.9 Template:Val–Template:Val
TNT 4.184 6.92 Template:Val Template:Val
Barium 3.99 14.0 Template:Val Template:Val burned to barium dioxide
ANFO 3.7 Template:Val

Electrochemical reactions (batteries)

Template:Table alignment

Energy released by electrochemical reactions or similar means
Material Specific energy
(MJ/kg) 		Energy density
(MJ/L) 		Specific energy
(W⋅h/kg) 		Energy density
(W⋅h/L) 		Comment
Zinc-air battery 1.59[48] 6.02 441.7 Template:Val controlled electric discharge
Lithium air battery (rechargeable) 9.0[49] 2,500.0 controlled electric discharge
Sodium sulfur battery 0.54–0.86 150–240
Lithium metal battery 1.8 4.32 500 Template:Val controlled electric discharge
Lithium-ion battery 0.36–0.875Template:Refn 0.9–2.63 100.00–243.06 250.00–730.56 controlled electric discharge
Lithium-ion battery with silicon nanowire anodes 1.566 4.32 435[50] 1,200[50] controlled electric discharge
Alkaline battery 0.48[51] 1.3[52] controlled electric discharge
Nickel-metal hydride battery 0.41[53] 0.504–1.46[53] controlled electric discharge
Lead-acid battery 0.17 0.56 47.2 156 controlled electric discharge
Supercapacitor (EDLC) 0.01–0.030[54][55][56][57][58][59][60] 0.006–0.06[54][55][56][57][58][59] up to 8.57[60] controlled electric discharge
Electrolytic capacitor Template:Val–Template:Val[61] Template:Val–Template:Val[61][62][63] controlled electric discharge

Common battery formats

Battery energy capacities
Storage device Energy content
(J) 		Energy content
(W⋅h) 		Typical
mass (g) 		Typical dimensions
(diameter × height in mm) 		Typical volume (mL) Specific energy (MJ/kg) Energy density (MJ/L)
Alkaline AA battery[64] Template:Val 2.6 24 14.2 × 50 7.92 0.39 1.18
Alkaline C battery[64] Template:Val 9.5 65 26 × 46 24.42 0.53 1.41
NiMH AA battery Template:Val 2.5 26 14.2 × 50 7.92 0.35 1.15
NiMH C battery Template:Val 5.4 82 26 × 46 24.42 0.24 0.80
Lithium-ion 18650 battery Template:Val–Template:Val 8–13 44–49[65] 18 × 65 16.54 0.59–1.06 1.74–2.83

Nuclear reactions

Template:Table alignment

Energy released by nuclear reactions
Material Specific energy
(MJ/kg) 		Energy density
(MJ/L) 		Specific energy
(W⋅h/kg) 		Energy density
(W⋅h/L) 		Comment
Antimatter Template:Val ≈ Template:Val Depends on the density of the antimatter's form Template:Val ≈ 25 TW⋅h/kg Depends on the density of the antimatter's form Annihilation, counting both the consumed antimatter mass and ordinary matter mass
Hydrogen (fusion) Template:Val[66] but at least 2% of this is lost to neutrinos. Depends on conditions Template:Val Depends on conditions Reaction 4H→4He
Deuterium (fusion)
 571,182,758[67] Depends on conditions Template:Val Depends on conditions Proposed fusion scheme for D+D→4He, by combining D+D→T+H, T+D→4He+n, n+H→D and D+D→3He+n, 3He+D→4He+H, n+H→D
Deuterium+tritium (fusion) Template:Val[66] Depends on conditions Template:Val Depends on conditions D + T → 4He + n
Being developed.
Lithium-6 deuteride (fusion) Template:Val[66] Depends on conditions Template:Val Depends on conditions Template:SupLiD → 24He
Used in weapons.
Plutonium-239 Template:Val Template:Val–Template:Va (depends on crystallographic phase) Template:Val Template:Val–Template:Val (depends on crystallographic phase) Heat produced in Fission reactor
Plutonium-239 31,000,000 Template:Val–Template:Val (Depends on crystallographic phase) Template:Val Template:Val–Template:Val (depends on crystallographic phase) Electricity produced in Fission reactor
Uranium Template:Val[68] Template:Val Template:Val Heat produced in breeder reactor
Thorium Template:Val[68] Template:Val Template:Val Heat produced in breeder reactor (experimental)
Plutonium-238 Template:Val Template:Val Template:Val Radioisotope thermoelectric generator. The heat is only produced at a rate of 0.57 W/g.

In material deformation

The mechanical energy storage capacity, or resilience, of a Hookean material when it is deformed to the point of failure can be computed by calculating tensile strength times the maximum elongation dividing by two. The maximum elongation of a Hookean material can be computed by dividing stiffness of that material by its ultimate tensile strength. The following table lists these values computed using the Young's modulus as measure of stiffness:

Mechanical energy capacities
Material Energy density by mass

(J/kg)

Resilience: Energy density by volume

(J/L)

Density

(kg/L)

Young's modulus

(GPa)

Tensile yield strength

(MPa)

Rubber band Template:Val–Template:Val[69] Template:Val–Template:Val[69] 1.35[69]
Steel, ASTM A228 (yield, 1 mm diameter) Template:Val–Template:Val Template:Val–Template:Val 7.80[70] 210[70] Template:Val–Template:Val[70]
Acetals 908 754 0.831[71] 2.8[72] 65 (ultimate)[72]
Nylon-6 233–1,870 253–2,030 1.084 2–4[72] 45–90 (ultimate)[72]
Copper Beryllium 25-1/2 HT (yield) 684 Template:Val[73] 8.36[74] 131[73] Template:Val[73]
Polycarbonates 433–615 520–740 1.2[75] 2.6[72] 52–62 (ultimate)[72]
ABS plastics 241–534 258–571 1.07 1.4–3.1[72] 40 (ultimate)[72]
Acrylic Template:Val 3.2[72] 70 (ultimate)[72]
Aluminium 7077-T8 (yield) 399 Template:Val[73] 2.81[76] 71.0[73] 400[73]
Steel, stainless, 301-H (yield) 301 Template:Val[73] 8.0[77] 193[73] 965[73]
Aluminium 6061-T6 (yield @ 24 °C) 205 553 2.70[78] 68.9[78] 276[78]
Epoxy resins 113–Template:Val 2–3[72] 26–85 (ultimate)[72]
Douglas fir Wood 158–200 96 Template:Val–Template:Val[79] 13[72] 50 (compression)[72]
Steel, Mild AISI 1018 42.4 334 7.87[80] 205[80] 370 (440 Ultimate)[80]
Aluminium (not alloyed) 32.5 87.7 2.70[81] 69[72] 110 (ultimate)[72]
Pine (American Eastern White, flexural) 31.8–32.8 11.1–11.5 0.350[82] 8.30–8.56 (flexural)[82] 41.4 (flexural)[82]
Brass 28.6–36.5 250–306 8.4–8.73[83] 102–125[72] 250 (ultimate)[72]
Copper 23.1 207 8.93[83] 117[72] 220 (ultimate)[72]
Glass 5.56–10.0 13.9–25.0 2.5[84] 50–90[72] 50 (compression)[72]

Other release mechanisms

Template:Table alignment

Energy released by other means
Material Specific energy
(MJ/kg) 		Energy density
(MJ/L) 		Specific energy
(W⋅h/kg) 		Energy density
(W⋅h/L) 		Comment
Silicon (phase change) 1.790 4.5 500 1,285 Energy stored through solid to liquid phase change of silicon[85]
Strontium bromide hydrate 0.814 [86] 1.93 628 Thermal energy of phase change at Template:Cvt
Liquid nitrogen 0.77[87] 0.62 213.9 172.2 Maximum reversible work at 77.4 K with 300 K reservoir
Compressed air at Template:Convert 0.5 0.2 138.9 55.6 Potential energy
Latent heat of fusion of ice (thermal) 0.334 0.334 93.1 93.1
Flywheel 0.36–0.5 5.3 Kinetic energy
Water at 100 m dam height Template:Val Template:Val 0.272 0.272 Figures represent potential energy, but efficiency of conversion to electricity is 85–90%[88][89]

See also

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References

Template:Reflist

Further reading

  • The Inflationary Universe: The Quest for a New Theory of Cosmic Origins by Alan H. Guth (1998) Template:ISBN
  • Cosmological Inflation and Large-Scale Structure by Andrew R. Liddle, David H. Lyth (2000) Template:ISBN
  • Richard Becker, "Electromagnetic Fields and Interactions", Dover Publications Inc., 1964
  • Template:Note "Aircraft Fuels". Energy, Technology and the Environment Ed. Attilio Bisio. Vol. 1. New York: John Wiley and Sons, Inc., 1995. 257–259
  • "Fuels of the Future for Cars and Trucks" – Dr. James J. Eberhardt – Energy Efficiency and Renewable Energy, U.S. Department of Energy – 2002 Diesel Engine Emissions Reduction (DEER) Workshop San Diego, California - August 25–29, 2002
  • Template:Cite web

Template:Authority control

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  3. ↑ Cite error: Invalid <ref> tag; no text was provided for refs named tzar3
  4. ↑ Cite error: Invalid <ref> tag; no text was provided for refs named tzar4
  5. ↑ 5.0 5.1 5.2 Template:Cite web
  6. ↑ Cite error: Invalid <ref> tag; no text was provided for refs named tzar6
  7. ↑ Cite error: Invalid <ref> tag; no text was provided for refs named tzar7
  8. ↑ Cite error: Invalid <ref> tag; no text was provided for refs named tzar8
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  21. ↑ 21.0 21.1 21.2 College of the Desert, “Module 1, Hydrogen Properties”, Revision 0, December 2001 Hydrogen Properties. Retrieved 2014-06-08.
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  45. ↑ David E. Dirkse. energy buffers. "household waste 8..11 MJ/kg"
  46. ↑ 46.0 46.1 46.2 Thomas C. Allison. (2013). NIST-JANAF Thermochemical Tables - SRD 13 (1.0.2) [dataset]. National Institute of Standards and Technology. https://doi.org/10.18434/T42S31
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