Peroxyacetyl nitrate

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Peroxyacetyl nitrate
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Abbreviations PAN
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Template:Longitem C2H3NO5
Molar mass 121.05 g mol−1
log P −0.19
Vapor pressure 29.2 mmHg at 298 K
Template:Longitem 0.000278 m3 atm mol−1 at 298 K
Template:Longitem 10−13 cm3 molecule−1 s−1 at 298 K

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Peroxyacetyl nitrate is a peroxyacyl nitrate. It is a secondary pollutant present in photochemical smog.[1] It is thermally unstable and decomposes into peroxyethanoyl radicals and nitrogen dioxide gas.[2] It is a lachrymatory substance, meaning that it irritates the lungs and eyes.[3]

Peroxyacetyl nitrate, or PAN, is an oxidant that is more stable than ozone. Hence, it is more capable of long-range transport than ozone. It serves as a carrier for oxides of nitrogen (NOx) into rural regions and causes ozone formation in the global troposphere.[1]

Atmospheric chemistry

PAN is produced in the atmosphere via photochemical oxidation of hydrocarbons to peroxyacetic acid radicals, which react reversibly with nitrogen dioxide (Template:Chem2) to form PAN.[4]Template:Rp Night-time reaction of acetaldehyde with nitrogen trioxide is another possible source.[4] Since there are no direct emissions, it is a secondary pollutant. Next to ozone and hydrogen peroxide (H2O2), it is an important component of photochemical smog.

Further peroxyacyl nitrates in the atmosphere are peroxypropionyl nitrate (PPN), peroxybutyryl nitrate (PBN), and peroxybenzoyl nitrate (PBzN). Chlorinated forms have also been observed. PAN is the most important peroxyacyl nitrate. PAN and its homologues reach about 5 to 20 percent of the concentration of ozone in urban areas. At lower temperatures, it is stable and can be transported over long distances, providing nitrogen oxides to otherwise unpolluted areas. At higher temperatures, it decomposes into NO2 and the peroxyacetyl radical.

The decay of PAN in the atmosphere is mainly thermal. Thus, the long-range transport occurs through cold regions of the atmosphere, whereas the decomposition takes place at warmer levels. PAN can also be photolysed by UV radiation. It is a reservoir gas that serves both as a source and a sink of ROx- and NOx radicals.[5] Nitrogen oxides from PAN decomposition enhance ozone production in the lower troposphere.

The natural concentration of PAN in the atmosphere is below 0.1 μg/m3. Measurements in German cities showed values up to 25 μg/m3. Peak values above 200 μg/m3 have been measured in Los Angeles in the second half of the 20th century (1 ppm of PAN corresponds to 4370 μg/m3). Due to the complexity of the measurement setup, only sporadic measurements are available.

PAN is a greenhouse gas.

Synthesis

PAN can be produced in a lipophilic solvent from peroxyacetic acid.[6][7][8][9] For the synthesis, concentrated sulfuric acid is added to degassed n-tridecane and peroxyacetic acid in an ice bath. Next, concentrated nitric acid is added.

As an alternative, PAN can also be synthesized in the gas phase via photolysis of acetone and NO2 with a mercury lamp.[10] Methyl nitrate (CH3ONO2) is created as a by-product.

Toxicity

The toxicity of PAN is higher than that of ozone. Eye irritation from photochemical smog is caused more by PAN and other trace gases than by ozone, which is only sparingly soluble. PAN is a mutagen,[11] and is considered a potential contributor to the development of skin cancer.Script error: No such module "Unsubst".

References

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  5. ↑ J. S. Gaffney et al.: Peroxyacyl Nitrates. In: The Handbook of Environmental Chemistry. Vol. 4, Part B, S. 1–38; Hrsg.: Hutzinger, O., Springer, 1989.
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  9. ↑ J. L. Fry Spectroscopy and kinetics of atmospheric reservoir species: HOONO, CH3C(O)OONO2, CH3OOH and HOCH2OOH. Ph.D. Thesis, 2006
  10. ↑ Script error: No such module "Citation/CS1".
  11. ↑ Script error: No such module "citation/CS1".
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