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By McEvoy J.E. (ed.)

ISBN-10: 0841202192

ISBN-13: 9780841202191

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Reduction Reactions . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1 Modeling . . . . . . . . . . . . . . . . General Advective/Dispersive Reactive Transport Equation . . . Model Solutions to the Transport Equation . . . . . . . Analytical . . . . . . . . . . . . . . . . Numerical . . . . . . . . . . . . . . . . Model Codes . . . . . . . . . . . . . . . Case Studies of Model Applications .

With only a few exceptions (for instance, ethylbenzene has not been demonstrated to degrade under sulfatereducing conditions), BTEX oxidation using sulfate, carbon dioxide, ferric iron, 46 M. N. Goltz et al. and Mn(IV) as electron acceptors has also been demonstrated [29, 40]. As would be expected based on energy considerations, anaerobic BTEX oxidation is slower than aerobic oxidation. First-order BTEX oxidation rate constants under anaerobic conditions are reported in Suarez and Rifai [31]. Anaerobic oxidation has also been demonstrated as a pathway for chlorinated ethene degradation.

40 M. N. Goltz et al. Note that kf/kb is equivalent to the Freundlich sorption coefficient (Kf) in Eq. (4) and at equilibrium Eq. (7) simplifies to the Freundlich model, Eq. (4). If we assume a Langmuir isotherm, with sorption kinetics described by a second-order rate constant (kf) that depends on both dissolved contaminant concentration and number of available sorption sites, the following expression results [3, 21]: dS 0 4 = kf C (Q – S) – kbS dt (8) where kf is the second-order sorption rate constant [L3M–1T–1] and kb is the first-order desorption rate constant [T–1].

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Catalysts for the Control of Automotive Pollutants Catalysts for the Control of Automotive Pollutants by McEvoy J.E. (ed.)


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