A few binary compounds decompose to their constituent elements upon heating. This is an oxidation-reduction reaction since the elements undergo a change in oxidation number. For example, the oxides and halides of noble metals (primarily Au, Pt, and Hg) decompose when heated. When red solid Mercury(II) oxide is heated, it decomposes to liquid metallic mercury and oxygen gas:
2HgO (s) → 2Hg (l) + O2 (g)
Some nonmetal oxides, such as the halogen oxides, also decompose upon heating:
2Cl2O5 (g) → 2Cl2 (g) + 5O2 (g)
Other nonmetal oxides, such as dinitrogen pentoxide, decompose to an element and a compound:
2N2O5 (g) → O2 (g) + 4NO2 (g)
Many metal salts containing oxoanions decompose upon heating. These salts either give off oxygen gas, forming a metal salt with a different nonmetal anion, or they give off a nonmetal oxide, forming a metal oxide. For example, metal nitrates containing Group 1A or 2A metals or aluminum decompose to metal nitrites and oxygen gas:
Mg(NO3)2 (s) → Mg(NO2)2 (s) + O2 (g)
2SO3 (g) → 2SO2 (g) + O2 (g)
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There are many examples of decomposition reaction. A notable example is hydrogen peroxide, which will decompose into water and oxygen over a slow period of time.
Examples:
CaCO3-----------CaO + CO2
Ca(OH)2---------CaO + H2O
NH4Cl------------NH3 + HCl
All of the decomposition reactions in an organism taken together is called catabolism, while the synthesis reactions are called anabolism.
These are decomposition reactions.
Decomposition reactions are used in various industrial processes to break down compounds into simpler substances. They are also important in nature for processes such as decay and nutrient recycling. In chemistry, decomposition reactions are studied to understand the behavior of substances when they are broken down.
Decomposition reactions always have one complex reactant and two or more simpler products.
anabolism