K2O2

K2O2, commonly referred to as potassium peroxide, is an inorganic compound composed of potassium cations (K+) and the peroxide dianion (O2^2−). It is a white to pale yellow, hygroscopic solid and is a strong oxidizer. Potassium peroxide is not found naturally and is produced industrially or in laboratory settings under controlled conditions.

Preparation and occurrence

Potassium peroxide is typically prepared by the oxidation of molten potassium oxide with oxygen or by oxidation of potassium hydroxide with oxygen at elevated temperatures. Industrial routes aim to control moisture and impurities because peroxides are moisture-sensitive and reactive.

Reactions and properties

In water, potassium peroxide reacts vigorously to form potassium hydroxide and hydrogen peroxide: K2O2 + 2 H2O → 2 KOH + H2O2. With acids, it can yield potassium salts and hydrogen peroxide: K2O2 + 2 HCl → 2 KCl + H2O2. Upon heating, K2O2 decomposes to potassium oxide and oxygen: 2 K2O2 → 2 K2O + O2. As a peroxide, it is a potent oxidizer and can promote combustion of organic materials; therefore it is typically stored in dry conditions and kept away from reducing agents, moisture, and sources of heat.

Applications

K2O2 is used mainly as an oxidizing agent in chemical synthesis and as a source of reactive oxygen in certain industrial processes. Its handling requires precautions due to its moisture sensitivity and oxidizing nature, and it is generally used in controlled, dry environments rather than in consumer applications.

Safety

Due to its reactivity with water and acids, and its strong oxidizing properties, potassium peroxide should be stored in a dry, well-ventilated area away from incompatible materials. Protective equipment such as gloves and eye protection is recommended when handling.