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{{one source|date=December 2011}}The standard Gibbs free energy of formation 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 | ΔGfo (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
References1. ^M.W. Chase, NIST - JANAF Thermochemical Tables, 4th Edition, Journal of Physical and Chemical Reference Data, Monograph 9, 1998
- {{cite book|editor-last=Dean|editor-first=John A.|title=Lange's Handbook of Chemistry|url=https://books.google.com/books?id=p6MRAQAAMAAJ|edition=15th|year=1999|publisher=McGraw-Hill|location=New York|isbn=978-0-07-016384-3}}
External links{{DEFAULTSORT:Gibbs free energy Of formation, Standard}} 1 : Thermodynamic free energy |