1c:I[419806,["/_next/static/chunks/bb923814e1f4d2e9.js","/_next/static/chunks/dd3ee9f5b7716ca6.js","/_next/static/chunks/4204a0ae82542ca8.js","/_next/static/chunks/30036bedc5269936.js","/_next/static/chunks/6e1aa89a642f40be.js","/_next/static/chunks/cd5e572bc3e4eb92.js","/_next/static/chunks/8ffd0b71567920d8.js","/_next/static/chunks/67ea6dfd21f16c5f.js","/_next/static/chunks/24eb4379f68013fd.js","/_next/static/chunks/b8cd775ffdf935bd.js","/_next/static/chunks/983103cd9eb7b428.js","/_next/static/chunks/d4ac9dcf27f6ff52.js","/_next/static/chunks/294b9525248c8e5f.js"],"default"] 1d:T483,The generation of hydrogen peroxide (H₂O₂) and the depletion of oxalic acid by photochemical/chemical cycling of Fe(III)/Fe(II)-oxalato complexes in sunlight has been studied under the conditions typical for acidified atmospheric water. H₂O₂ is produced through the reduction of oxygen by intermediates formed from photoreactions of Fe(III)-oxalato complexes. The rate of H₂O₂ formation increases with sunlight intensity, and with oxalate and Fe(III) concentration within the concentration range used. This rate is 3.7 nM s^-1 when 1 μM Fe(III) and 5 μM oxalate at pH 4 is exposed to September noon sunlight. Speciation calculations based on the concentration range of Fe(III) and oxalic acid in atmospheric water indicate that Fe(III)-oxalato complexes are often the predominant species of dissolved Fe(III). The concentrations of Fe(III)-oxalato complexes are sufficiently large to make their photolysis a dominant source of in-cloud H₂O₂, O₂^·-, HO₂, and OH radicals and a major sink for atmospheric oxalic acid.1e:Tb8b,

	Year	Citations

References