Potassium Peroxide

Potassium peroxide
Names
	IUPAC name Potassium peroxide
Identifiers
CAS Number	17014-71-0 ;
3D model (JSmol)	Interactive image;
ChemSpider	26237 ;
EC Number	241-089-8;
PubChem CID	28202;
UNII	ZHB4ZOE9PU ;
	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 (So298)	113 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	−496 kJ·mol−1
Hazards
GHS pictograms
GHS Signal word	Danger
GHS hazard statements	H272, H315, H319
GHS precautionary statements	P210, P220, P221, P264, P280, P302+352, P305+351+338, P321, P332+313, P337+313, P362, P370+378, P501
NFPA 704 (fire diamond)	0 3 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).
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	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).

Crystal structure

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

[math]\ce{ 2K2O2 + 2H2O -> 4KOH + O2 (^) }[/math]

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.

References

↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. pp. 477; 520. ISBN 0-8493-0594-2.
↑ ^2.0 ^2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.

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[hand-1] 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] 2.0 ^2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.