Hydrogen Peroxide - Gas Profile
Hydrogen peroxide (H₂O₂) is a colourless liquid that is slightly more viscous than water and has no discernible odour. It is a powerful oxidizing agent and belongs to the peroxide family of compounds, characterised by an oxygen-oxygen single bond. Hydrogen peroxide is highly reactive and can decompose explosively when concentrated, but doesn't burn itself - instead it supports combustion by releasing oxygen. Unlike many industrial chemicals, hydrogen peroxide is entirely natural and decomposes into only water and oxygen, making it an environmentally friendly oxidizing agent.
Deodorants, water and sewage treatment, rocket fuels, disinfection, and the production of other chemicals all use hydrogen peroxide as a versatile oxidising and bleaching agent.
The discovery of hydrogen peroxide dates back to 1818 when French chemist Louis Jacques Thénard first isolated it by reacting barium peroxide with nitric acid. Thénard named his discovery "eau oxygénée" in French, meaning "oxygenated water," as he was astounded by the high oxygen content present in the final product. One of the first things he discovered about hydrogen peroxide was that it attacked the skin, producing painful blotches that fortunately wore off completely within a few hours.
- Hydrogen peroxide occurs naturally in very small amounts in the atmosphere, formed when atmospheric oxygen reacts with water
- It is present in plant and animal cells as a natural byproduct of metabolic reactions
- The human body produces hydrogen peroxide naturally, which is then broken down by the enzyme catalase
- Catalase is found in nearly all living organisms and can convert millions of hydrogen peroxide molecules per second
- Hydrogen peroxide was first used commercially in the 1800s, primarily for bleaching textiles and hair
- By 1913, it was being used in dentistry for treating gum disease and teeth whitening
Gas Fact – Hydrogen peroxide naturally decomposes into water and oxygen so effectively that it's completely environmentally friendly, leaving no harmful residues - making it nature's own "green" chemical!
Industrial & Commercial Uses of Hydrogen Peroxide
Hydrogen peroxide is used in numerous applications due to its disinfecting and oxidising qualities:
- Water and sewage treatment: Oxidises contaminants, aiding purification
- Rocket fuel additive: High-concentration hydrogen peroxide acts as a propellant oxidiser
- Disinfection and sterilisation: Common in medical devices, cleanrooms, and pharmaceutical sterilisation
- Chemical synthesis: Acts as a precursor or reagent in manufacturing processes
- Personal care products: Found in deodorants, hair dyes, and wound cleaners
- Agriculture: Used in low concentrations to oxygenate soil and combat root rot
Environmental & Safety Profile of H₂O₂
Hydrogen peroxide breaks into oxygen and water, making it a cleaner alternative to harsh disinfectants like chlorine and formaldehyde. While it's considered safe in low concentrations, industrial-grade hydrogen peroxide (30–90%) is hazardous:
- Irritant to skin, eyes, and lungs
- Corrosive in high concentrations
- Reactive with organic materials
- Can cause thermal decomposition or explosive pressure buildup if improperly handled
Facilities using vapour-phase H₂O₂ must deploy hydrogen peroxide gas detectors to prevent accidental inhalation, overexposure, or equipment failure in sterilisation and production environments.
FAQs About Hydrogen Peroxide (H₂O₂)
What is hydrogen peroxide used for in industry?
Hydrogen peroxide is used for sterilisation, oxidation, wastewater treatment, rocket propellants and chemical manufacturing.
Is hydrogen peroxide safe to inhale?
No. Inhalation of vapour can cause respiratory tract irritation, coughing, and, in high doses, lung injury.
How do you detect hydrogen peroxide gas or vapour?
Using hydrogen peroxide gas detectors or vapour-phase sensors, especially in cleanrooms, biotech labs, and medical sterilisation units.
Why is hydrogen peroxide used in plant care?
Diluted H₂O₂ improves soil oxygenation, helping plants fight root rot and bacteria.