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Chemical Properties
Nitrogen oxides are a class of compounds generally represented by the chemical abbreviation NOx. The "x" takes into account the number of oxygen atoms present in a particular molecule. Scientists track the abundance of nitrogen dioxide (NO2) in the atmosphere because it readily reacts with many different compounds, including water, and has damaging health and environmental effects.
Production
High-temperature combustion is a leading source of nitrogen oxides. Nitrogen and oxygen do not typically combine at normal temperatures in the environment, and it takes an event like a lightning strike to create nitric oxide (NO) naturally. People rely on combustion to run industries and their vehicles, so nitrogen oxides are an economic necessity.
Effects
The presence of nitrogen oxides in the atmosphere can result in other chemical reactions, creating ozone and nitric acid. High ozone levels can be harmful to both humans and animals, causing respiratory distress, irritating asthmatic conditions and increasing the risk of contracting influenza and other diseases. It can also cause lung damage after prolonged exposure. Nitric acid in the atmosphere is carried back to Earth by water droplets, and this acid rain can cause pollution in bodies of water and significant damage to marble and limestone structures.
Reduction Efforts
Significant acid rain and pollution concerns in the 1980s led to greater emphasis by the government and industries to control nitrogen oxide emissions. Producers are attempting to capture NOx gases prior to their release into the atmosphere and use a process called selective catalytic reduction (SCR) to separate the nitrogen and oxygen. SCR employs ammonia as a catalyst to break NOx bonds, producing an organic end result of nitrogen and water. Cormetech, a specialist in NOx reduction for Mitsubishi Heavy Industries and Corning Inc., indicates 70 to 95 percent of industrial nitrogen oxides can be kept out of the environment by using SCR technology.