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Ozone

Ozone (O3) is a triatomic molecule, consisting of three oxygen atoms. It is an allotrope of oxygen that is much less stable than the diatomic species O2. It is present in low concentrations throughout the Earth's atmosphere. It has many industrial and consumer applications as well as being used in ozone therapy.

Ozone, the first allotrope of a chemical element to be described by science, was discovered by öChristian Friedrich Schnbein in 1840, who named it after the Greek word for smell (ozein), from the peculiar odor in lightning storms.[1] The odor from a lightning strike is from electrons freed during the rapid chemical changes, not the ozone itself.[2]

Ozone can be used for bleaching substances and for killing bacteria. Many municipal drinking water systems kill bacteria with ozone instead of the more common chlorine. Ozone does not form organochlorine compounds, but it also does not remain in the water after treatment, so some systems introduce a small amount of chlorine to prevent bacterial growth in the pipes, or may use chlorine intermittently, based on results of periodic testing. Where electrical power is abundant, ozone is a cost-effective method of treating water, as it is produced on demand and does not require transportation and storage of hazardous chemicals. Once it has decayed, it leaves no taste or odor in drinking water. Low level of Ozone is helpful to purify air inside the house. Eliminate mildew and mold build up.

Industrially, ozone or ozonated water is used to

  • · disinfect water before it is bottled;
  • · deodorize air and objects, such as after a fire;
  • · kill bacteria on food or on contact surfaces;
  • · scrub yeast and mold spores from the air in food processing plants;
  • · wash fresh fruits and vegetables to kill yeast, mold and bacteria;
  • · chemically attack contaminants in water (iron, arsenic, hydrogen sulfide, nitrites, and complex organics lumped together as "color");
  • · provide an aid to flocculation (agglomeration of molecules, which aids in filtration, where the iron and arsenic are removed);
  • · clean and bleach fabrics (the latter use is patented);
  • · assist in processing plastics to allow adhesion of inks;
  • · age rubber samples to determine the useful life of a batch of rubber;
  • · in surface water treatment plants to eradicate water borne parasites such as Giardia and Cryptosporidium. This process is known as ozonation.
  • Ozone is a reagent in many organic reactions in the laboratory and in industry. Ozonolysis is the cleavage of an alkene to carbonyl compounds.

    • Many hospitals in the U.S. and around the world use large ozone generators to decontaminate operating rooms between surgeries. The rooms are cleaned and then sealed airtight before being filled with ozone which effectively kills or neutralizes all remaining bacteria

    • General

      Systematic name

      Trioxygen

      Molecular formula

      O3

      Molar mass

      47.998 g/mol

      Appearance

      bluish colored gas

      CAS number

      [10028-15-6]

      Properties

      Density and phase

      2.144 g/l (0 °C), gas

      Solubility in water

      0.105 g/100 ml (0 °C)

      Melting point

      80.7 K, −-192.5 °C

      Boiling point

      161.3 K, −-111.9 °C

      Thermodynamic data

      Standard enthalpy of
      formation Δ?fH°solid

      +142.3 kJ/mol

      Standard molar entropy
      S°solid

      237.7 J.K−-1.mol−-1

      Hazards

      EU classification

      not listed

      NFPA 704

       

      Supplementary data page

      Structure and
      properties

      n, εer, etc.

      Thermodynamic
      data

      Phase behaviour
      Solid, liquid, gas

      Spectral data

      UV, IR, NMR, MS

      Regulatory data

      Flash point,
      RTECS number, etc.

      Except where noted otherwise, data are given for
      materials in their °standard state (at 25 C, 100 kPa)
      Infobox disclaimer and references

    Wikipedia © 2006