Oxidation of ferrous sulfate in weakly acidic solution by gas bubbling

Minegishi, Tomoya; Asaki, Zenjiro; Higuchi, Binzo; Kondô, Yoshio

doi:10.1007/bf02654046

Cited by 3 publications

(4 citation statements)

References 6 publications

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“…An attempt has been made to approximate the experimental Fe 2+ ions concentration to the equilibrium value by considering the oxidation of Fe 2+ ions to ferric hydroxide using the integrated kinetic model of Minegishi et al (1983). As noted the corrected experimental and theoretical values are very close for ethyl and propyl xanthate but not for butyl xanthate, which may be due to the adsorption of propyl xanthate on bare surface of pyrite and the surface of dixanthogen.…”

Section: Resultsmentioning

confidence: 93%

On the cathodic reaction coupled with the oxidation of xanthates at the pyrite/aqueous solution interface

Valdivieso

López

Song

2005

International Journal of Mineral Processing

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Section: Resultsmentioning

confidence: 93%

On the cathodic reaction coupled with the oxidation of xanthates at the pyrite/aqueous solution interface

Valdivieso

López

Song

2005

International Journal of Mineral Processing

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“…Despite that ferrous sulfate is a water-soluble chemical and, in theory, its rapid release of dissolved Fe 2+ could be favourable for hydroxyl radical generation through Fenton reaction, it did not exhibit a significantly stronger capacity to decompose the petroleum hydrocarbons, as compared to magnetite. Possibly, oxidation of ferrous iron prior to Fenton-like reaction resulted in a reduction of Fe 2+ availability (Minegishi et al, 1983). The oxidation of Fe 2+ can be accelerated under alkaline conditions (Hove et al, 2007;Daenzer et al, 2015) such as those encountered in desert soils and this could further weaken its availability.…”

Section: Discussionmentioning

confidence: 99%

Decomposition of long-chain petroleum hydrocarbons by Fenton‐like processes: Effects of ferrous iron source, salinity and temperature

Qin¹,

Lin

Al-Mebayedh

et al. 2019

Ecotoxicology and Environmental Safety

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Batch experiments were conducted to examine the effects of ferrous iron source, soil salinity of temperature on degradation of long-chain petroleum hydrocarbons by Fenton-like processes. The results show that over 70%, 50% and 25% of aliphatic C16-C21, C21-C35 and C35-C40, respectively, was eliminated at a H 2 O 2 dose of 1.5%. The decomposition rate of petroleum hydrocarbons was similar to each other for ferrous sulfate and magnetite while the capacity of pyrite to trigger Fenton-driven decomposition of long-chain aliphatic petroleum hydrocarbons was weaker, as compared to ferrous sulfate and magnetite. The decomposition rate of aromatic hydrocarbons decreased with increasing length of carbon chain in the ferrous sulfate and magnetite systems, but the opposite was observed in the pyrite system. The effect of Fenton-like process on degradation of longchain petroleum hydrocarbons was enhanced by increased temperature. At a temperature of 60 o C, the enhancement of Fenton process outweighed the adverse effects from potential loss of H 2 O 2 due to elevated temperature. The use of magnetite as a source of ferrous iron was likely to prevent consumption of Fe 2+ by complexation with chloride ion from occurring and consequently effectively eliminated the inhibitory effect of salinity on Fenton reaction.

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“…Iron(III) compounds are valuable semiproducts used in the production of various ironcontaining substances, pigments, and coatings. However, iron (II) salt oxidation with oxygen proceeds via complicated multistep pathways and depends strongly on the composition of the reaction medium and other process conditions [12][13][14][15][16][17][18][19][20][21]. Conversion of dissolved iron into its highest oxidation state is a necessary step in a variety of commercial hydrometallurgical processes, such as purification of hydrometallurgical solutions and regeneration of Fe(III)-containing solutions that were used as an oxidizer in the processing of complex ores or in the removal of hydrogen sulfide from waste gas [5][6][7][8][9][10][11].…”

mentioning

confidence: 99%

“…Furthermore, they are components of coagulants for water purification [1][2][3][4]. In this case, the oxidation rate may be inversely proportional to the squared concentrations of H + and Fe 2+ [15][16][17][18][19]. Iron(II) is known to be readily oxidizable in air in neutral and alkali media.…”

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confidence: 99%

10.1007/s10975-008-1005-6

2000

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The kinetics of iron(II) sulfate oxidation with molecular oxygen on the 2% Pt/Sibunit catalyst was studied by a volumetric method at atmospheric pressure, T = 303 K, pH 0.33-2.4, [ FeSO 4 ] = 0.06-0.48 mol/l, and [ Fe 2 (SO 4 ) 3 ] = 0-0.36 mol/l in the absence of diffusion limitations. Relationships were established between the reaction rate and the concentrations of Fe 2+ , Fe 3+ , H + , and Clions in the reaction solution. The kinetic isotope effect caused by the replacement of H 2 O with D 2 O and of H + with D + was measured. The dependence of Fe 2+ and Fe 3+ adsorption on the catalyst pretreatment conditions was studied. A reaction scheme is suggested, which includes oxygen adsorption, the formation of a Fe(II) complex with surface oxygen, and the one-electron reduction of oxygen. The last step can proceed via two pathways, namely, electron transfer with H + addition and hydrogen atom transfer from the coordination sphere of the iron(II) aqua complex. A kinetic equation providing a satisfactory fit to experimental data is set up. Numerical values are determined for the rate constants of the individual steps of the scheme suggested.

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Oxidation of ferrous sulfate in weakly acidic solution by gas bubbling

Cited by 3 publications

References 6 publications

On the cathodic reaction coupled with the oxidation of xanthates at the pyrite/aqueous solution interface

On the cathodic reaction coupled with the oxidation of xanthates at the pyrite/aqueous solution interface

Decomposition of long-chain petroleum hydrocarbons by Fenton‐like processes: Effects of ferrous iron source, salinity and temperature

10.1007/s10975-008-1005-6

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