ENVIRONMENTAL CHEMISTRY

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ENVIRONMENTAL CHEMISTRY ( environmental-chemistry )

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412 troposphere. Two of the pollutants that are emitted are hydrocarbons (unburnt fuels) and nitric oxide (NO). When these pollutants build up to sufficiently high levels, a chain reaction occurs from their interaction with sunlight in which NO is converted into nitrogen dioxide (NO2). This NO2 in turn absorbs energy from sunlight and breaks up into nitric oxide and free oxygen atom (Fig. 14.2). NO2(g) NO(g) + O(g) (i) Oxygen atoms are very reactive and combine with the O2 in air to produce ozone. O(g) + O2 (g)  O3 (g) (ii) The ozone formed in the above reaction (ii) reacts rapidly with the NO(g) formed in the reaction (i) to regenerate NO2. NO2 is a brown gas and at sufficiently high levels can contribute to haze. NO(g)+O (g)→NO (g)+O (g) (iii) 322 Ozone is a toxic gas and both NO2 and O3 are strong oxidising agents and can react with the unburnt hydrocarbons in the polluted air CHEMISTRY to produce chemicals such as formaldehyde, acrolein and peroxyacetyl nitrate (PAN). 3CH4 + 2O3 →3CH2=O +3H2O Formaldehyde Fig. 14.2 Photochemical smog occurs where sunlight acts on vehicle pollutants. 2019-20 CH2=CHCH=O Acrolein CH3COONO2  O Peroxyacetyl nitrate (PAN) Effects of photochemical smog The common components of photochemical smog are ozone, nitric oxide, acrolein, formaldehyde and peroxyacetyl nitrate (PAN). Photochemical smog causes serious health problems. Both ozone and PAN act as powerful eye irritants. Ozone and nitric oxide irritate the nose and throat and their high concentration causes headache, chest pain, dryness of the throat, cough and difficulty in breathing. Photochemical smog leads to cracking of rubber and extensive damage to plant life. It also causes corrosion of metals, stones, building materials, rubber and painted surfaces.

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