Formation of Sodium Peroxide

2Na + O2 → Na2O2

Overview

When sodium burns in excess oxygen, it forms sodium peroxide rather than sodium oxide. This yellowish-white compound is a powerful oxidizer. Unlike the lighter alkali metals, sodium preferentially forms the peroxide due to the size ratio of the ions.

Participants

Role Substance Coefficient State
Reactant Oxygen O 1 (g)
Reactant Sodium Na 2 (s)

Everyday Example

Sodium peroxide has been used in submarine air purification systems, reacting with CO2 to release oxygen.

Industrial Importance

Used as an oxygen-generating agent in emergency breathing apparatus, as a bleaching agent for textiles, and as a powerful oxidizer in organic chemistry.

Properties

Type
Synthesis
Reversible
No
Energy
Exothermic
ΔH
-510.9 kJ/mol

Related Reactions

Fischer-Tropsch Synthesis (General) Formation of Aluminum Oxide Formation of Ammonia (Haber Process) Formation of Barium Oxide Formation of Barium Sulfate Formation of Beryllium Oxide Formation of Cadmium Oxide Formation of Calcium Carbonate from Oxides Formation of Calcium Hydroxide Formation of Calcium Oxide (Quicklime)

Frequently Asked Questions

What is the equation for Formation of Sodium Peroxide?
The balanced equation is: 2Na + O₂ → Na₂O₂.
What type of reaction is Formation of Sodium Peroxide?
Formation of Sodium Peroxide is a synthesis reaction.
Is Formation of Sodium Peroxide exothermic or endothermic?
Formation of Sodium Peroxide is exothermic (releases energy). The enthalpy change (ΔH) is -510.9 kJ/mol.