Oxygen Production

Industrially, oxygen is typically produced in bulk quantity as a liquid produced by distillation from atmospheric air.

In the laboratory small quantities of oxygen can be produced through heating potassium permanganate (KMnO₄):

2KMnO₄ = K₂MnO₄ + MnO₂ + O₂

The decomposition of hydrogen peroxide using manganese dioxide as a catalyst also results in the production of more pure oxygen gas:

MnO₂: 2H₂O₂ = 2H₂O + O₂^

Oxygen is yielded after intensive (at the temperature higher than 600°C) baking of sodium nitrate:

2NaNO₃ = 2NaNO₂ + O₂^

as well as heating of some higher oxides:

4CrO₃ = 2Cr₂O₃ + 3O₂^
2PbO₂ = 2PbO + O₂^
3MnO₂ = Mn₃O₄ + O₂^

The reaction between the mixture of sodium peroxide and potassium superoxide KO₂ and carbon dioxide is the main source of oxygen in confined spaces such as space ships, submarines etc.:

2Na₂O₂ + 2CO₂ => 2Na₂CO₃ + O₂^
4KO₂ + 2CO₂ => 2K₂CO₃ + O₂^

If their molar ratio is 1:1, then each mole of air carbon dioxide will yield one mole of oxygen, so the air proportions will not be changed due to respiration.