Calcination (also referred to as
calcining) is a thermal treatment process applied to
ores and other solid materials in order to bring about a
thermal decomposition,
phase transition, or removal of a volatile fraction. The calcination process normally takes place at temperatures below the
melting point of the product materials. Calcination is to be distinguished from
roasting, in which more complex gas-solid reactions take place between the furnace atmosphere and the solids.
Industrial processes
The process of calcination derives its name from the Latin
calcinare (to burn lime) due to its most common application, the decomposition of calcium carbonate (
limestone) to
calcium oxide (
lime) and
carbon dioxide, in order to produce
cement. The product of calcination is usually referred to in general as "calcine," regardless of the actual minerals undergoing thermal treatment. Calcination is carried out in
furnaces or reactors (sometimes referred to as
kilns) of various designs including
shaft furnaces,
rotary kilns,
multiple hearth furnaces, and
fluidized bed reactors.
Examples of calcination processes include the following:
decomposition of carbonate minerals, as in the calcination of limestone to drive off carbon dioxide;
decomposition of hydrated minerals, as in calcination of bauxite, to remove crystalline water as water vapor;
decomposition of volatile matter contained in raw petroleum coke;
heat treatment to effect phase transformations, as in conversion of anatase to rutile or devitrification of glass materials
removal of ammonium ions in the synthesis of zeolites
Calcination reactions
Calcination reactions usually take place at or above the thermal decomposition temperature (for decomposition and volatilization reactions) or the transition temperature (for phase transitions). This temperature is usually defined as the temperature at which the standard
Gibbs free energy for a particular calcination reaction is equal to zero. For example, in limestone calcination, a decomposition process, the chemical reaction is
:CaCO
3 → CaO + CO
2(g)
The standard Gibbs free energy of reaction is approximated as ΔG°r = 177,100 − 158 T (J/mol). The standard free energy of reaction is zero in this case when the temperature, T, is equal to 1121 K, or 848 °C.
Examples of chemical decomposition reactions common in calcination processes, and their respective thermal decomposition temperatures include:
:CaCO3 → CaO + CO2; 848 °C
See also calcination equilibrium of calcium carbonate
Oxidation
In some cases, calcination of a metal results in
oxidation of the metal.
Jean Rey noted that
lead and
tin when calcinated gained weight, presumably as they were being oxidized.
Alchemy
In
alchemy, calcination was believed to be one of the 12 vital processes required for the transformation of a substance.
Alchemists distinguished two kinds of calcination, actual and potential. Actual calcination is that brought about by actual fire, from wood, coals, or other fuel, raised to a certain temperature. Potential calcination is that brought about by potential fire, such as corrosive chemicals; for example, gold was calcined in a reverberatory furnace with mercury and sal ammoniac; silver with common salt and alkali salt; copper with salt and sulfur; iron with sal ammoniac and vinegar; tin with antimony; lead with sulfur; and mercury with aqua fortis.
There was also philosophical calcination, which was said to occur when horns, hooves, etc., were hung over boiling water, or other liquor, until they had lost their mucilage, and were easily reducible into powder.
References
Category:Chemical processes
Category:Alchemical processes
