Hydrogen peroxide
Hydrogen peroxide is a chemical compound. Its molecular formula is H2O2. It is used as a cleaner, and as hair bleach. In a concentration of 3% (meaning that there are 3 grams of hydrogen peroxide for 100 grams of a water solution), it can be used to treat wounds. Over time it will slowly become oxygen gas and water through decomposition.
Chemists often use hydrogen peroxide in chemical reactions. It is a very strong oxidising agent when used with acid and water. Oxidising agents take electrons from other compounds.
- 2 Fe2+(aq) + H2O2 + 2 H+(aq) → 2 Fe3+(aq) + 2 H2O(l)
Here hydrogen peroxide takes an electron from the Fe2+ ions and becomes water.
It can also be a reducing agent when used with other compounds. When it acts as a reducing agent, oxygen gas is also produced. Reducing agents give electrons to other compounds. This method is often used to make oxygen in laboratories.
- NaOCl + H2O2 → O2 + NaCl + H2O
Hydrogen peroxide can be bought in shops when mixed with lots of water but is very dangerous when the concentration is higher. It is flammable and causes burns.
Hydrogen Peroxide Media
Phase diagram of H
2O
2 and water: Area above blue line is liquid. Dotted lines separate solid–liquid phases from solid–solid phases.
Catalytic cycle for the anthraquinone process to produce hydrogen peroxide: an anthraquinone (right) is reduced using hydrogen to produce the corresponding anthrahydroquinone (left). This is oxidized using oxygen to produce hydrogen peroxide and recover anthraquinone.
ISO tank container for hydrogen peroxide transportation
A tank car designed for transporting hydrogen peroxide by rail
- Ascaridol
Australian bombardier beetle
Rocket-belt hydrogen-peroxide propulsion system used in a jet pack
Contact lenses soaking in a 3% hydrogen peroxide-based solution. The case includes a catalytic disc which neutralises the hydrogen peroxide over time.
Chemiluminescence of cyalume, as found in a glow stick
Skin shortly after exposure to 35% H
2O
2
