Standard Gibbs free energy of formation

Short description: Change in energy from formation of 1 mole of substance

The standard Gibbs free energy of formation (Gf°) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).

The table below lists the standard Gibbs function of formation for several elements and chemical compounds and is taken from Lange's Handbook of Chemistry. Note that all values are in kJ/mol. Far more extensive tables can be found in the CRC Handbook of Chemistry and Physics and the NIST JANAF tables.[1] The NIST Chemistry WebBook (see link below) is an online resource that contains standard enthalpy of formation for various compounds along with the standard absolute entropy for these compounds from which the standard Gibbs free energy of formation can be calculated.

Species  | Phase (matter)  | Chemical formula  | ΔGf° (kJ/mol)

|
|
|

Aluminum
Aluminum | Solid  | Al  | 0
Aluminum chloride  | Solid  | AlCl3 | −628.9
Aluminum oxide  | Solid  | Al2O3 | −1582.3
Barium
Barium | Solid  | Ba  | 0
Barium chloride | Solid  | BaCl2 | −806.7
Barium carbonate | Solid  | BaCO3 | −1134.4
Barium oxide | Solid  | BaO  | −520.4
Barium sulfate | Solid  | BaSO4 | −1362.2
Beryllium
Beryllium | Solid  | Be  | 0
Beryllium hydroxide | Solid  | Be(OH)2 | −815.0
Boron
Boron trichloride | Solid  | BCl3 | −388.7
Bromine
Bromine | Liquid  | Br2 | 0
Bromine trifluoride | Gas  | BrF3 | −229.4
Hydrobromic acid | Gas  | HBr  | −53.4
Calcium
Calcium | Solid  | Ca  | 0
Calcium carbide | Solid  | CaC2 | −64.9
Calcium carbonate (Calcite)  | Solid  | CaCO3 | −1129.1
Calcium chloride | Solid  | CaCl2 | −748.8
Calcium chloride | Aqueous  | CaCl2 | −816.05
Calcium hydride | Solid  | CaH2 | −142.5
Calcium hydroxide | Solid  | Ca(OH)2 | −897.5
Calcium oxide | Solid  | CaO  | −603.3
Calcium sulfate | Solid  | CaSO4 | −1309.1
Calcium sulfide | Solid  | CaS  | −477.4
Carbon
Carbon (graphite)  | Solid  | C  | 0
Carbon (diamond)  | Solid  | C  | 2.900
Carbon dioxide | Gas  | CO2 | −394.39
Carbonic acid | Aqueous  | H2CO3 | −623.1
Bicarbonate | Aqueous  | HCO3− | −586.85
Carbonate ion  | Aqueous  | CO32− | −527.8
Carbon disulfide | Gas  | CS2 | 67.1
Carbon monoxide | Gas  | CO  | −137.16
Glucose | Solid  | C6H12O6 | −910.56
Ethanol | Liquid  | C2H5OH  | −174.8
Carbonyl chloride (phosgene)  | Gas  | COCl2 | −204.9
Caesium
Caesium | Solid  | Cs  | 0
Caesium chloride | Solid  | CsCl  | −414.4
Chlorine
Chlorine | Gas  | Cl2 | 0
Chromium
Chromium | Solid  | Cr  | 0
Copper
Copper | Solid  | Cu  | 0
Copper(I) sulfide | Solid  | Cu2S  | −86.2
Fluorine
Fluorine | Gas  | F2 | 0
Hydrogen
Hydrogen | Gas  | H2 | 0
Water | Liquid  | H2O  | −237.14
Water | Gas  | H2O  | −228.61
Hydrogen peroxide | Liquid  | H2O2 | −120.42
Hydrogen cyanide | Gas  | HCN  | +124.7
Hydrogen iodide | Gas  | HI  | +1.3
Hydrogen fluoride | Gas  | HF  | −275.4
Hydrogen chloride | Gas  | HCl  | −95.30
Iodine
Iodine | Solid  | I2 | 0
Iodine | Gas  | I2 | 19.37
Iron
Lead
Lithium
Magnesium
Magnesium carbonate | Solid  | MgCO3 | −1012.1
Magnesium chloride | Solid  | MgCl2 | −591.8
Magnesium hydroxide | Solid  | Mg(OH)2 | −833.7
Magnesium hydroxide | Aqueous  | Mg(OH)2 | −769.4
Magnesium oxide | Solid  | MgO  | −596.3
Magnesium sulfate | Solid  | MgSO4 | −1170.6
Manganese
Manganese(II) oxide | Solid  | MnO  | −362.9
Manganese(IV) oxide  | Solid  | MnO2 | −465.2
Mercury
Mercury(II) oxide (red)  | Solid  | HgO  | −58.49
Mercury sulfide (red, cinnabar)  | Solid  | HgS  | −50.6
Nickel
Nitrogen
Ammonia | Aqueous  | NH3 | −26.57
Ammonia | Gas  | NH3 | −16.4
Ammonium chloride | Solid  | NH4Cl  | −203.89
Nitrogen dioxide | Gas  | NO2 | 51.3
Nitrogen monoxide | Gas  | NO  | 87.60
Oxygen
Monatomic oxygen  | Gas  | O  | 231.7
Dioxygen | Gas  | O2 | 0
Ozone | Gas  | O3 | 163.2
Hydroxide | Aqueous  | OH− | −157.2
Phosphorus
Phosphorus trichloride | Liquid  | PCl3 | −272.4
Potassium
Potassium bromide | Solid  | KBr  | −380.7
Potassium chlorate | Solid  | KClO3 | −296.31
Potassium chloride | Solid  | KCl  | −408.5
Potassium fluoride | Solid  | KF  | −537.8
Potassium perchlorate | Solid  | KClO4 | −303.1
Silicon
Silica (quartz)  | Solid  | SiO2 | −856.4
Silver
Silver bromide | Solid  | AgBr  | −96.90
Silver chloride | Solid  | AgCl  | −109.8
Silver iodide | Solid  | AgI  | −66.19
Silver oxide | Solid  | Ag2O  | −11.21
Silver sulfide | Solid  | Ag2S  | −40.67
Sodium
Sodium carbonate | Solid  | Na2CO3 | −1044.4
Sodium carbonate | Aqueous  | Na2CO3 | −1051.6
Sodium chloride | Aqueous  | NaCl  | −393.17
Sodium chloride | Solid  | NaCl  | −384.1
Sodium fluoride | Solid  | NaF  | −546.3
Sodium hydroxide | Aqueous  | NaOH  | −419.2
Sodium hydroxide | Solid  | NaOH  | −379.4
Sodium nitrate | Aqueous  | NaNO3 | −373.21
Sodium nitrate | Solid  | NaNO3 | −367.06
Sulfur
Hydrogen sulfide | Gas  | H2S  | −33.4
Sulfur dioxide | Gas  | SO2 | −300.13
Sulfur trioxide | Gas  | SO3 | −370.4
Sulfuric acid | Liquid  | H2SO4 | −689.9
Tin
Titanium
Zinc

## See also

* Thermochemistry
* Calorimetry

## References

1. ↑ M. W. Chase, NIST – JANAF Thermochemical Tables, 4th Edition, Journal of Physical and Chemical Reference Data, Monograph 9, 1998.

* Dean, John A., ed (1999). Lange's Handbook of Chemistry (15th ed.). New York: McGraw-Hill. ISBN 978-0-07-016384-3. https://books.google.com/books?id=p6MRAQAAMAAJ.

## External links

* NIST Chemistry WebBook

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