Tropospheric ozone

Tropospheric ozone
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Tropospheric_ozone".

Seasonal average concentrations of tropospheric ozone in Dobson units over the period 1979 to 2000. In June to August photochemical ozone production causes very high concentrations over the East Coast of the USA and China.

Ozone (O₃) is a key constituent of the troposphere (it is also an important constituent of certain regions of the stratosphere commonly known as the Ozone layer). Photochemical and chemical reactions involving it drive many of the chemical processes that occur in the atmosphere by day and by night. At abnormally high concentrations brought about by human activities (largely the combustion of fossil fuel), it is a pollutant, a constituent of smog. Many highly energetic reactions produce it, ranging from combustion to photocopying. Often laser printers will have a smell of ozone, which in high concentrations is toxic. Ozone is a powerful oxidizing agent readily reacting with other chemical compounds to make many possibly toxic oxides.

The troposphere extends to between 10 and 18 kilometers above the surface of the Earth and consists of many layers. Ozone is more concentrated above the mixing layer, or ground layer. Ground-level ozone, though less concentrated than ozone aloft, is more of a problem because of its health effects.

Tropospheric ozone is a greenhouse gas and initiates the chemical removal of methane and other hydrocarbons from the atmosphere thus its concentration affects how long these compounds remain in the air.

Satellites can measure tropospheric ozone.[1][2] Measurements specifically of ground-level ozone require in situ monitoring technology.

content

1 Formation
2 Health effects
3 Problem areas
4 See also
5 References
6 External links

Formation

The majority of tropospheric ozone formation occurs when nitrogen oxides (NOx), carbon monoxide (CO) and volatile organic compounds (VOCs), such as xylene, react in the atmosphere in the presence of sunlight. NOx and VOCs are called ozone precursors. Motor vehicle exhaust, industrial emissions, and chemical solvents are the major anthropogenic sources of these chemicals. Another source is windshield washer fluid. Although these precursors often originate in urban areas, winds can carry NOx hundreds of kilometers, causing ozone formation to occur in less populated regions as well. Methane, a VOC whose atmospheric concentration has increased tremendously during the last century, contributes to ozone formation but on a global scale rather than in local or regional photochemical smog episodes. In situations where this exclusion of methane from the VOC group of substances is not obvious, the term Non-Methane VOC (NMVOC) is often used.

The chemical reactions involved in tropospheric ozone formation are a series of complex cycles in which carbon monoxide and VOCs are oxidised to water vapour and carbon dioxide. The reactions involved in this process are illustrated here with CO but similar reactions occur for VOC as well. Oxidation begins with the reaction of CO with the hydroxyl radical. The hydrogen atom formed by this reacts rapidly with oxygen to give a peroxy radical HO₂

OH + CO → H + CO₂

H + O₂ → HO₂

Peroxy radicals then go on to react with NO to give NO₂ which is photolysed to give atomic oxygen and through reaction with oxygen a molecule of ozone:

HO₂ + NO → OH + NO₂

NO₂ + hν → NO + O

O + O₂ → O₃

The net effect of these reactions is:

CO + 2O₂ → CO₂ + O₃

This cycle involving HO_x and NO_x is terminated by the reaction of OH with NO₂ to form nitric acid or by the reaction of peroxy radicals with each other to form peroxides. The chemistry involving VOCs is much more complex but the same reaction of peroxy radicals oxidizing NO to NO₂ is the critical step leading to ozone formation.

Health effects

The following text needs to be harmonized with text in the article Ozone.
(See e.g. Wikipedia:Summary style.)

Ozone is known to have the following health effects at concentrations common in urban air:

Irritation of the respiratory system, causing coughing, throat irritation, and/or an uncomfortable sensation in the chest.
Reduced lung function, making it more difficult to breathe deeply and vigorously. Breathing may become more rapid and more shallow than normal, and a person's ability to engage in vigorous activities may be limited.
Aggravation of asthma. When ozone levels are high, more people with asthma have attacks that require a doctor's attention or use of medication. One reason this happens is that ozone makes people more sensitive to allergens, which in turn trigger asthma attacks.
Increased susceptibility to respiratory infections.
Inflammation and damage the lining of the lungs. Within a few days, the damaged cells are shed and replaced much like the skin peels after a sunburn. Animal studies suggest that if this type of inflammation happens repeatedly over a long time period (months, years, a lifetime), lung tissue may become permanently scarred, resulting in permanent loss of lung function and a lower quality of life.

A statistical study of 95 large urban communities in the United States found significant association between ozone levels and premature death. The study estimated that a one-third reduction in urban ozone concentrations would save roughly 4000 lives per year (Bell et. al, 2004).

Problem areas

The following text needs to be harmonized with text in the article Ozone.
(See e.g. Wikipedia:Summary style.)

The United States Environmental Protection Agency has developed an Air Quality index to help explain air pollution levels to the general public. 8-hour average ozone concentrations of 85 to 104 ppbv are described as "Unhealthy for Sensitive Groups", 105 ppbv to 124 ppbv as "unhealthy" and 125 ppb to 404 ppb as "very unhealthy" [3]. The EPA has designated over 300 counties of the United States, clustered around the most heavily populated areas (especially in California and the Northeast), as failing to comply with the National Ambient Air Quality Standards.

References

Michelle L. Bell; Aidan McDermott; Scott L. Zeger; Jonathan M. Samet; Francesca Dominici (2004). "Ozone and Short-term Mortality in 95 US Urban Communities, 1987-2000". Journal of the American Medical Association. 292, 2372-2378.

Seinfeld, John H.; Pandis, Spyros N (1998). Atmospheric Chemistry and Physics - From Air Pollution to Climate Change. John Wiley and Sons, Inc. ISBN 0-471-17816-0

Wayne, Richard P (2000). Chemistry of Atmospheres (3rd Ed.). Oxford University Press. ISBN 0-19-850375-X

External links

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Contents

Formation

Health effects

Problem areas

See also

References

External links