Chemical decomposition: Difference between revisions
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reece kington is sexy '''analysis''' or '''breakdown''' is the separation of a [[chemical compound]] into [[chemical element|elements]] or simpler compounds. It is sometimes defined as the exact opposite of a [[chemical synthesis]]. Chemical decomposition is often an undesired [[chemical reaction]]. The stability that a chemical compound ordinarily has is eventually limited when exposed to extreme environmental conditions like [[heat]], [[radiation]], [[humidity]] or the [[acidity]] of a [[solvent]]. The details of decomposition processes are generally not well defined, as a [[molecule]] may break up into a host of smaller fragments. Chemical decomposition is exploited in several analytical techniques, notably [[mass spectrometry]], traditional [[gravimetric analysis]], and [[thermogravimetric analysis]]. |
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A broader definition of the term '''decomposition''' also includes the breakdown of one phase into two or more phases.<ref name="Gold">{{GoldBookRef|title=decomposition|url=http://goldbook.iupac.org/D01547.html}}</ref> |
A broader definition of the term '''decomposition''' also includes the breakdown of one phase into two or more phases.<ref name="Gold">{{GoldBookRef|title=decomposition|url=http://goldbook.iupac.org/D01547.html}}</ref> |
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Revision as of 23:57, 15 September 2011
reece kington is sexy analysis or breakdown is the separation of a chemical compound into elements or simpler compounds. It is sometimes defined as the exact opposite of a chemical synthesis. Chemical decomposition is often an undesired chemical reaction. The stability that a chemical compound ordinarily has is eventually limited when exposed to extreme environmental conditions like heat, radiation, humidity or the acidity of a solvent. The details of decomposition processes are generally not well defined, as a molecule may break up into a host of smaller fragments. Chemical decomposition is exploited in several analytical techniques, notably mass spectrometry, traditional gravimetric analysis, and thermogravimetric analysis.
A broader definition of the term decomposition also includes the breakdown of one phase into two or more phases.[1]
There are broadly three types of decomposition reactions: thermal, electrolytic and catalytic.[citation needed]
Reaction formula
The generalized reaction for chemical decomposition is:
- AB → A + B
with a specific example being the electrolysis of water to gaseous hydrogen and oxygen:
- 2H2O(I) → 2H2 + O2
Additional examples
An example of spontaneous decomposition is that of hydrogen peroxide, which will slowly decompose into water and oxygen:
- 2H2O2 → 2H2O + O2
Carbonates will decompose when heated, a notable exception being that of carbonic acid, H2CO3. Carbonic acid, the "fizz" in sodas, pop cans and other carbonated beverages, will decompose over time (spontaneously) into carbon dioxide and water
- H2CO3 → H2O + CO2
Other carbonates will decompose when heated producing the corresponding metal oxide and carbon dioxide. In the following equation M represents a metal:
- MCO3 → MO + CO2
A specific example of this involving calcium carbonate:
- CaCO3 → CaO + CO2
Metal chlorates also decompose when heated. A metal chloride and oxygen gas are the products.
- 2MClO3 → 2MCl + 3O2
A common decomposition of a chlorate to evolve oxygen utilizes potassium chlorate as follows:
- 2KClO3 → 2KCl + 3O2
Many metal carbonates decompose to form metal oxides and carbon dioxide when heated.
See also
References
- ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "decomposition". doi:10.1351/goldbook.C01020
External links
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