Photocatalytic Degradation of Atmospheric Pollutants on the Surface of Metal Oxides

Guesten, H.

doi:10.1007/978-3-642-70627-1_21

Cited by 15 publications

(5 citation statements)

References 51 publications

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“…Subsequently, the reaction is accomplished by interaction between these. It has been proposed that the most probable reason for the catalytic activity of oxides is their basic nature, which helps in accomplishment of the reaction S 4+ and 02 [22]. The observed rate dependence on the catalyst concentration is in accordance with the limiting amount of TCNQ adsorbed.…”

Section: Methodssupporting

confidence: 64%

Electron donor properties and catalytic activity of manganese ferrospinels

Sugunan

John

Renuka

et al. 1999

React Kinet Catal Lett

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The electron donating properties of manganese ferrospinels of various compositions (MnFe204, MnL2 FeLsO4, Mn2FeO4 and Mn2.sFe0.504 ) were studied from the adsorption of electron acceptors of various electron affinity values from acetonitrile as solvent. The limit of electron transfer fTom the oxide surface is from 1.77 to 2.40 eV in terms of the electron atfinity of the electron acceptor. The data have been correlated with the catalytic activity of these oxides towards autoxidation of sulfites. Both weak and strong electron donor sites catalyze the reaction.

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Section: Methodssupporting

confidence: 64%

Electron donor properties and catalytic activity of manganese ferrospinels

Sugunan

John

Renuka

et al. 1999

React Kinet Catal Lett

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“…5). The inorganic material in aerosols alone is considered to have a total surface area of 2 -10 times that of the earth [30] and a residence time of 1 -14 d [31].…”

Section: Natural and Anthropogenic Emissionsmentioning

confidence: 99%

Air, 6. Photochemical Degradation

Simmler

2011

Ullmann's Encyclopedia of Industrial Chemistry

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The article contains sections titled: 1. Introduction 2. Natural and Anthropogenic Emissions 3. Reaction Cycles in the Atmosphere 3.1. The Troposphere 3.2. The Stratosphere 4. Interaction with Surface Layers of Aquatic and Terrestrial Environments 5. Measurement and Computation of Degradability 5.1. Lifetime in the Homogeneous Gas Phase 5.2. Lifetimes of Adsorbates Aerosols 5.3. Assessment and Evaluation

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“…Experiments conducted to measure the photo-degradation of adsorbed PAHs in the laboratory, using natural and artifi cial particles, produced contradictory results [87][88][89][90][91]123]. The experiments showed that the PAHs were degraded by radiation that simulated solar radiation, but the time needed to degrade 50% varied considerably from ca.…”

Section: Degradation On Fly Ash and Sootmentioning

confidence: 99%

Abiotic Degradation in the Atmosphere

Klöpffer¹,

Wagner²

2007

Atmospheric Degradation of Organic Substances

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1)A sink is defi ned here as an irreversible chemical, photochemical or biochemical reaction which removes a molecule from the environment; a perfect sink leads to mineralization. Within this defi nition, the transfer to and the temporary fi xation in another compartment (e.g., soil, vegetation or water) without chemical modifi cation is not considered to be a sink [1].2 Photo-degradation in the Homogenous Gas Phase of the Troposphere Chapter 2: Abiotic Degradation in the Atmosphere 28 k OH (T) = (2.25 + 0.46 -0.39) × 10 -18 T 2 exp{(-910 ± 56)/T} cm 3 molecule -1 s -1 k OH (298 K) = 9.43 × 10 -15 cm 3 molecule -1 s -1More interesting for the average OH lifetime is k OH at the (weighted or effective) average temperature of the troposphere. This temperature has been estimated by Warneck [15] in an analysis of the tropospheric CH 4 + OH reaction as eff = 280 K. According to an earlier estimate, based on the lifetime of chlorinated hydrocarbons [34], this temperature may be as low as 260 K. Using the more recent estimate by Warneck, we obtain k OH (280 K) = 6.84 × 10 -15 cm 3 molecule -1 s -1The average tropospheric OH lifetimes of MCF is calculated to be τ OH = 9.3 a This value is higher than the average residence times calculated for MCF, which are based on long-term measurements of MCF concentrations and estimates of the amounts emitted yearly (see Section 5).MCF is photolysed at wavelengths around 200 nm [28] and can therefore act as a source of chlorine atoms in the stratosphere and contribute to ozone destruction. It has been phased out as a result of the Protocol of Montreal and its follow-up agreements.An up-to-date data collection of OH-reaction rate constants can be found in Chapter 3. Earlier critical data collections are mostly attributable to Roger Atkinson, whose group also measured many substances for the fi rst time

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Photocatalytic Degradation of Atmospheric Pollutants on the Surface of Metal Oxides

Cited by 15 publications

References 51 publications

Electron donor properties and catalytic activity of manganese ferrospinels

Electron donor properties and catalytic activity of manganese ferrospinels

Air, 6. Photochemical Degradation

Abiotic Degradation in the Atmosphere

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