What is sodium oxide
Light yellow powder
or light yellow beads
|molar mass 77.979 g / mol |
AGW not specified
density 2.805 g / cm3
Melting point +675 ° C
reacts violently with water
|Hazard classes + category |
Oxidising solids 1
Corrosive / irritant effect. on the skin 1A
|HP rates (see note) |
H 271, 314 P 210, 221, 280.1-4, 301 + 330 + 331, 305 + 351 + 338, 309 + 310
disposal Collect separately in a container or in a fume cupboard in a water disposal
|German name||English name|
|CAS1313-60-6||Sodium peroxide||Sodium peroxide|
Note for schools: Sodium peroxide is highly corrosive and can react violently with water and all flammable substances. Safety glasses, goggles, protective gloves and a face shield must be worn. You may only work in the fume cupboard. It is stored in a separate mini chemical cabinet over a glass pan.
Light yellow spheres are commercially available, which in this form are more stable and chemically not quite as reactive as the powder. Pure sodium peroxide would be completely white, the yellow coloration is caused by sodium hyperoxide NaO2 caused. Sodium peroxide eagerly absorbs moisture and carbon dioxide from the air and reacts with them spontaneously. Sodium carbonate and oxygen are formed with carbon dioxide.N / A2O2 + 2 H.2O 2 NaOH + H2O2
Sodium peroxide comes on the market as light yellow globules.
Sodium peroxide reacts with water with bubbles and strong heat generation, forming sodium hydroxide and hydrogen peroxide. If it is not cooled with ice at the same time, the hydrogen peroxide immediately breaks down further into water and oxygen:
2 H2O2 2 H2O + O2
Sodium peroxide can trigger explosive reactions on contact with flammable substances such as aluminum and magnesium powder or phosphorus. Flammable organic liquids can ignite by themselves. A mixture of paper or wood wool and sodium peroxide will also ignite by itself if little water is added.
Sodium peroxide is produced when sodium is burned in an oxygen atmosphere. At the same time, sodium oxide Na is also formed2O. How much of each of the two oxides is produced during combustion depends on the moisture present, the oxygen content and the combustion temperature. At higher combustion temperatures, sodium peroxide is more likely to form.
4 Na + O2 2 Well2O ΔHR. = −418 kJ / mol
2 Na + O2 N / A2O2 ΔHR. = −513 kJ / mol
Sodium peroxide is used in the chemical industry as a bleaching agent for plant and animal products. It has not been used in laundry detergents since 1939. The detergents used at the time caused fires again and again. In fire brigade breathing apparatus or in submarines, it is used as a very efficient absorbent for carbon dioxide. Sodium peroxide is also a raw material for making other peroxo compounds.
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