Editing Azide (section)

=== Destruction by oxidation by nitrite ===
Azides decompose with nitrite compounds such as [[sodium nitrite]]. Each elementary [[redox]] reaction is also a [[comproportionation]] reaction because two different N-species ({{Chem2|N3- and NO2-}}) converge to a same one (respectively {{Chem2|N2, N2O and NO}}) and is favored when the solution is acidified. This is a method of destroying residual azides, prior to disposal.<ref>{{cite book | title = Prudent practices in the laboratory: handling and disposal of chemicals | year = 1995 | publisher = [[National Academy Press]] | location = Washington, D.C. | isbn = 0-309-05229-7 | url = http://books.nap.edu/openbook.php?record_id=4911&page=165 | author = Committee on Prudent Practices for Handling, Storage, and Disposal of Chemicals in Laboratories, Board on Chemical Sciences and Technology, Commission on Physical Sciences, Mathematics, and Applications, National Research Council}}</ref> In the process, nitrogen gas ({{chem2|N2}}) and nitrogen oxides ({{chem2|N2O}} and NO) are formed:

:{{chem2|3 N3- + NO2- + 2 H2O → 5 N2 + 4 OH-}}

:{{chem2|2 N3- + 4 NO2- + 3 H2O → 5 N2O + 6 OH-}}

:{{chem2|N3- + 7 NO2- + 4 H2O → 10 NO + 8 OH-}}

Azide (<em>−⅓</em>) (the [[Reducing agent|reductant]], [[electron donor]]) is [[Redox|oxidized]] in {{Chem2|N2}} (0), [[nitrous oxide]] ({{Chem2|N2O}}) (+1), or [[nitric oxide]] (NO) (+2) while [[nitrite]] (+3) (the [[Oxidizing agent|oxidant]], [[electron acceptor]]) is simultaneously [[Redox|reduced]] to the same corresponding species in each elementary redox reaction considered here above. The respective stability of the reaction products of these three [[comproportionation]] redox reactions is in the following order: {{Chem2|N2 > N2O > NO}}, as can be verified in the Frost diagram for nitrogen.