Copper peroxide
| Properties | |
|---|---|
| CuO2 | |
| Molar mass | 95.945 g/mol |
| Appearance | dark olive-green |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Copper peroxide is the inorganic compound with the formula CuO2. It is an oxide of copper, and appears as a dark olive green solid or similarly colored suspension. It is unstable, decomposing to oxygen and other copper oxides.
Preparation
Copper peroxide is prepared by the reaction of cold solutions of hydrogen peroxide and Schweizer's reagent, the latter prepared from copper hydroxide and dilute ammonia solution.[1] The Schweizer's reagent used must not contain excess ammonia.[1] Copper peroxide may also be produced by the reaction of an ice-cold solution of hydrogen peroxide with a suspension of copper hydroxide.[2] It may also form from the very slow reaction of finely divided cupric oxide with cold hydrogen peroxide.[3]
Properties
When wet, copper peroxide readily decomposes[4] at temperatures above 6°C; it "is far more stable when dry".[3]
References
- 1 2 The collected works of Sir Humphry Davy: Discourses delivered before the Royal society. Elements of agricultural chemistry, pt. I. The Chemical Society (Great Britain). 1894. p. 32.
- ↑ Friend, John Newton (1924). A Text-book of Inorganic Chemistry. C. Griffin, Ltd. p. 276.
- 1 2 Journal of the Chemical Society of London, Volume 48, Part 1. London. 1885. p. 124.
- ↑ Electrical World, Volume 39. 1902. p. 997.