Kinetics of Aqueous SO2 oxidation at different rate controlling steps

Pasiuk-Bronikowska, W.; Ziajka, J.

doi:10.1016/0009-2509(89)85264-9

Cited by 14 publications

(9 citation statements)

References 8 publications

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“…Values of k\ given in Table 1 are similar to others reported in literature for agitated cells which vary from 1.5 x 10~5 to 6 x 10~5 ms" 1 [16,17,18,19]. Known jfci, another series of phenol ozonation reactions was done with lower values of the ozone partial pressure so the reaction could develop in the fast kinetic regime.…”

Section: Ozonation Of Phenolsupporting

confidence: 79%

Rate constant determination of ozone‐organic fast reactions in water using an agitated cell

Beltrán

Álvarez

1996

Journal of Environmental Science and Health . Part A: Environme

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Rate constants of the direct reaction between ozone and some organic pollutants (phenol and azo dyes) in water have been determined from experiments carried out in an agitated cell of known interfacial area. Kinetic equations derived from the Danckwerts model for gas to liquid absorption have been applied. By varying the ozone partial pressure, the regime of ozone absorption can be changed from instantaneous to fast. In the first case, the volumetric mass transfer coefficient was obtained, while in the second, the rate constant of the ozoneorganic direct reaction studied was determined. The procedure is recommended for ozonation reactions with rate constants in the range 10 2 -10 5 m 3 mol -1 S -1 .

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Section: Ozonation Of Phenolsupporting

confidence: 79%

Rate constant determination of ozone‐organic fast reactions in water using an agitated cell

Beltrán

Álvarez

1996

Journal of Environmental Science and Health . Part A: Environme

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“…Most of the investigations reported in the literature on the mechanism of the aqueous phase oxidation of sulfur dioxide are related to homogeneous catalytic reactions with catalysts such as Cu2+, Mn2+, Co2+ etc. (for example, Hegg and Hobbs, 1978;Altwicker, 1979;Pasiuk-Bronikowska and Ziajka, 1989). These mechanisms are usually based on freeradical chain reactions involving the formation of radicals such as S03and SO5"™.…”

Section: Mechanism and Rate Modelmentioning

confidence: 99%

Oxidation of Sulfur Dioxide in Aqueous Suspensions of Activated Carbon

Govindarao¹,

Gopalakrishna²

1995

Ind. Eng. Chem. Res.

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Sulfur dioxide in aqueous solutions a t low pH levels exists both in molecular SOz(aq) and in hydrolyzed ionic form HSOa-. Experiments indicate that only HS03is the reacting species in the oxidation catalyzed by activated carbon, while SOz(aq) deactivates by competing with HS03for the active sites of the catalyst particles. A mechanism is proposed and a rate model is developed that also accounts for the effect of sulfuric acid (product of the oxidation) on the solubility of sulfur dioxide. It predicts first order in HS03-, half order in dissolved oxygen, and a linear deactivation effect of SOz(aq), which are confirmed by experimental data. The deactivation reaches a constant level corresponding to saturation of the active sites by SOAaq). Activation energy for the oxidation is 93.55 kJ mol-l and for deactivation is 21.4 kJ mol-l.

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“…Although reactions [2][3][4][5] are expressed using sulfite ions and radicals, we are aware that the question of whether sulfite or bisulfite species (or both) are active in the transformations has not yet been finally answered. L"~in eq 2 represents a ligand.…”

Section: Reaction Modelmentioning

confidence: 99%

“…In recent years the attention of investigators working in the area of air pollution control has concentrated on catalytic oxidation of calcium sulfite (CaS03) with molecular oxygen (1)(2)(3)(4)(5). The interest in this reaction is, on the one hand, because of its commercial applicability in flue gas desulfurization systems and, on the other hand, because of the still obscure chemistry and kinetics of the radical chain transformations involved.…”

Section: Introductionmentioning

confidence: 99%

“…Karlsson et al (4) intended to outline the mechanism of calcium sulfite slurry oxidation when the reagent was obtained by spray dryer absorption of sulfur dioxide. The work by Pasiuk-Bronikowska and Ziajka (5) was an attempt to arrange the information on bisulfite autoxidation in order to explain the different kinetics observed under varying reaction conditions. A summary of the literature, including this work, is given in Table I.…”

Section: Introductionmentioning

confidence: 99%

See 1 more Smart Citation

Mechanism and kinetics of autoxidation of calcium sulfite slurries

Pasiuk-Bronikowska¹,

Bronikowski²,

Ulejczyk³

1992

Environ. Sci. Technol.

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The kinetics of Co-catalyzed autoxidation of calcium sulfite was studied to deepen knowledge of the mechanism of this chain reaction. Laboratory experiments were performed under heterogeneous conditions using two different reactors: a stirred tank with a plane gas-liquid (slurry) interface and an impinger. The reaction course was followed by monitoring the conductivity of the reacting solution and by quenching with iodine solution, respectively. Mechanistic judgments were derived from the influence of sulfite and catalyst concentrations, and the solid CaS03 load on the kinetics of oxygen absorption. Appropriate reaction orders and rate constants were determined. Phenomena related to the solubility product law that imposed autoxidation rate limitations were analyzed. A soluble sulfate was shown to be a dual-action additive markedly accelerating the autoxidation due to increased sulfite and catalyst solubilities. The results are useful for designers of air pollution control processes.

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Kinetics of Aqueous SO2 oxidation at different rate controlling steps

Cited by 14 publications

References 8 publications

Rate constant determination of ozone‐organic fast reactions in water using an agitated cell

Rate constant determination of ozone‐organic fast reactions in water using an agitated cell

Oxidation of Sulfur Dioxide in Aqueous Suspensions of Activated Carbon

Mechanism and kinetics of autoxidation of calcium sulfite slurries

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