Potassium peroxide

Potassium peroxide
Names
	IUPAC name Potassium peroxide
Identifiers
CAS Number	17014-71-0 ;
3D model (JSmol)	Interactive image;
ChemSpider	26237 ;
ECHA InfoCard	100.037.339
EC Number	241-089-8;
PubChem CID	28202;
UNII	ZHB4ZOE9PU ;
CompTox Dashboard (EPA)	DTXSID2066143 ;
	InChI InChI=1S/2K.O2/c;;1-2/q2+1;-2 Key: XXQBEVHPUKOQEO-UHFFFAOYSA-N ; InChI=1/2K.O2/c;;1-2/q2+1;-2 Key: XXQBEVHPUKOQEO-UHFFFAOYAV;
	SMILES [O-][O-].[K+].[K+];
Properties
Chemical formula	K2O2
Molar mass	110.196 g/mol
Appearance	yellow amorphous solid
Melting point	490 °C (914 °F; 763 K)
Solubility in water	reacts with water
Structure
Crystal structure	Orthorhombic
Space group	Cmca, oS16
Thermochemistry
Std molar; entropy (S⦵298)	113 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	−496 kJ·mol−1
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H315, H319
Precautionary statements	P210, P220, P221, P264, P280, P302+P352, P305+P351+P338, P321, P332+P313, P337+P313, P362, P370+P378, P501
NFPA 704 (fire diamond)	3 0 2 W; OX
Related compounds
Other anions	Potassium chloride
Other cations	Lithium peroxide; Sodium peroxide; Rubidium peroxide; Caesium peroxide
Related potassium oxides	Potassium oxide; Potassium superoxide; Potassium ozonide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Potassium peroxide is an inorganic compound with the molecular formula K₂O₂. It is formed as potassium reacts with oxygen in the air, along with potassium oxide (K₂O) and potassium superoxide (KO₂).

Potassium peroxide reacts with water to form potassium hydroxide and oxygen:

2 K₂O₂ + 2 H₂O → 4 KOH + O₂ ↑

Properties

Potassium peroxide is a highly reactive, oxidizing white to yellowish solid which, while not flammable itself, reacts violently with flammable materials. It decomposes violently on contact with water.^[1]

The standard enthalpy of formation of potassium peroxide is ΔH f 0 = −496 kJ/mol.

Usage

Potassium peroxide is used as an oxidizing agent and bleach (due to the peroxide), and to purify air.^[3]

References

1 2 Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 477, 520. ISBN 0-8493-0594-2.
1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
↑ Stull, J.O.; White, M.G. (1985). "Air revitalization compounds: A literature survey". Toxicological & Environmental Chemistry. 10 (2): 133–155. Bibcode:1985TxEC...10..133S. doi:10.1080/02772248509357098.

[hand-1] 1 2 Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 477, 520. ISBN 0-8493-0594-2.

[b1-2] 1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.

[3] Stull, J.O.; White, M.G. (1985). "Air revitalization compounds: A literature survey". Toxicological & Environmental Chemistry. 10 (2): 133–155. Bibcode:1985TxEC...10..133S. doi:10.1080/02772248509357098.

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