العربية
中国
Français
Deutsch
Ελληνική
हिन्दी
Italiano
日本語
Português
Русский
EspañolCHEMICAL DECOMPOSITION
'Chemical decomposition' or 'analysis' is the fragmentation of a chemical compound into elements or smaller compounds. It is sometimes defined as the 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]
The generalized reaction formula for chemical decomposition is:
: AB → A + B
with a specific example being the electrolysis of water to gaseous hydrogen and oxygen:
: 2H2O → 2H2 + O2
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.
: MClO3 → MCl + O2
A common decomposition of a chlorate to evolve oxygen utilizes potassium chlorate as follows:
: 2 KClO3 → 2 KCl + 3 O2
★ Analytical chemistry
1.
★ Biodegradation database
A broader definition of the term 'decomposition' also includes the breakdown of one phase into two or more phases.[1]
| Contents |
| Reaction formulas |
| Additional examples |
| See also |
| References |
| External links |
Reaction formulas
The generalized reaction formula for chemical decomposition is:
: AB → A + B
with a specific example being the electrolysis of water to gaseous hydrogen and oxygen:
: 2H2O → 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.
: MClO3 → MCl + O2
A common decomposition of a chlorate to evolve oxygen utilizes potassium chlorate as follows:
: 2 KClO3 → 2 KCl + 3 O2
See also
★ Analytical chemistry
References
1.
External links
★ Biodegradation database
This article provided by Wikipedia. To edit the contents of this article, click here for original source.
psst.. try this: add to faves
