Potassium peroxide
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| Names | |
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| IUPAC name
Potassium peroxide
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| UNII | |
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| Properties | |
| K2O2 | |
| Molar mass | 110.196 g/mol |
| Appearance | yellow amorphous solid |
| Melting point | 490 °C (914 °F; 763 K) |
| reacts with water[1] | |
| Structure | |
| Orthorhombic | |
| Cmca, oS16 | |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
113 J·mol−1·K−1[2] |
Std enthalpy of
formation (ΔfH⦵298) |
−496 kJ·mol−1[2] |
| Hazards | |
| GHS labelling: | |
 
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| Danger | |
| H272, H315, H319 | |
| P210, P220, P221, P264, P280, P302+P352, P305+P351+P338, P321, P332+P313, P337+P313, P362, P370+P378, P501 | |
| NFPA 704 (fire diamond) | <imagemap>
File:NFPA 704.svg|80px|alt=NFPA 704 four-colored diamond poly 150 150 300 300 150 450 0 300 Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gas poly 300 0 450 150 300 300 150 150 Flammability 0: Will not burn. E.g. water poly 450 150 600 300 450 450 300 300 Instability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorus poly 300 300 450 450 300 600 150 450 Special hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer desc none </imagemap> |
| Related compounds | |
Other anions
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Potassium chloride |
Other cations
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Lithium peroxide Sodium peroxide Rubidium peroxide Caesium peroxide |
| 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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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.
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.