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Processes in the thermal degradation of organic matter at atmospheric pressure.

Thermal decomposition (or thermolysis) is a chemical decomposition caused by heat. The decomposition temperature of a substance is the temperature at which the substance chemically decomposes. The reaction is usually endothermic as heat is required to break chemical bonds in the compound undergoing decomposition. If decomposition is sufficiently exothermic, a positive feedback loop is created producing thermal runaway and possibly an explosion or other chemical reaction.

Decomposition temperature definition

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A simple substance (like water) may exist in equilibrium with its thermal decomposition products, effectively halting the decomposition. The equilibrium fraction of decomposed molecules increases with the temperature. Since thermal decomposition is a kinetic process, the observed temperature of its beginning in most instances will be a function of the experimental conditions and sensitivity of the experimental setup. For a rigorous depiction of the process, the use of thermokinetic modeling is recommended.[1]

main definition: Thermal decomposition is the breakdown of a compound into two or more different substances using heat, and it is an endothermic reaction


CaCO3 → CaO + CO2
The reaction is used to make quick lime, which is an industrially important product.
Another example of thermal decomposition is 2Pb(NO3)2 → 2PbO + O2 + 4NO2.

Decomposition of nitrates, nitrites and ammonium compounds

Ease of decomposition

When metals are near the bottom of the reactivity series, their compounds generally decompose easily at high temperatures. This is because stronger bonds form between atoms towards the top of the reactivity series, and strong bonds are difficult to break. For example, copper is near the bottom of the reactivity series, and copper sulfate (CuSO4), begins to decompose at about 200 °C (473 K; 392 °F), increasing rapidly at higher temperatures to about 560 °C (833 K; 1,040 °F). In contrast potassium is near the top of the reactivity series, and potassium sulfate (K2SO4) does not decompose at its melting point of about 1,069 °C (1,342 K; 1,956 °F), nor even at its boiling point.

Practical applications

Many scenarios in the real world are affected by thermal degradation. One of the things affected is fingerprints. When anyone touches something, there is residue left from the fingers. If fingers are sweaty, or contain more oils, the residue contains many chemicals. De Paoli and her collogues conducted a study testing thermal degradation on certain components found in fingerprints. For heat exposure, the amino acid and urea samples started degradation at 100 °C (373 K; 212 °F) and for lactic acid, the decomposition process started around 50 °C (323 K; 122 °F).[3] These components are necessary for further testing, so in the forensics discipline, decomposition of fingerprints is significant.

See also


  1. ^ Koga, Nobuyoshi; Vyazovkin, Sergey; Burnham, Alan K.; Favergeon, Loic; Muravyev, Nikita V.; Pérez-Maqueda, Luis A.; Saggese, Chiara; Sánchez-Jiménez, Pedro E. (2023). "ICTAC Kinetics Committee recommendations for analysis of thermal decomposition kinetics". Thermochimica Acta. 719: 179384. doi:10.1016/j.tca.2022.179384. S2CID 253341877.
  2. ^ Baykara S (2004). "Hydrogen production by direct solar thermal decomposition of water, possibilities for improvement of process efficiency". International Journal of Hydrogen Energy. 29 (14): 1451–1458. doi:10.1016/j.ijhydene.2004.02.014.
  3. ^ De Paoli G, Lewis SA, Schuette EL, Lewis LA, Connatser RM, Farkas T (July 2010). "Photo- and thermal-degradation studies of select eccrine fingerprint constituents". Journal of Forensic Sciences. 55 (4): 962–969. doi:10.1111/j.1556-4029.2010.01420.x. PMID 20487155. S2CID 37942037.