Kinetics of oxidation of Fe(II) ions by gaseous oxygen at high temperatures in an autoclave

Vračar, Rajko Ž.; Cerović, Katarina P

doi:10.1016/s0304-386x(96)00035-7

Cited by 25 publications

(8 citation statements)

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“…Vračar and Cerović studied the oxidation of ferrous ions in a stainless steel autoclave at temperatures ranging from 50 to 200 °C and partial pressures of oxygen ranging from 0.203 to 1.01 MPa. Initial concentrations of H 2 SO 4 and ferrous ions were 0.0–0.51 M and 0.036–0.90 M, respectively.…”

Section: Literature Reviewmentioning

confidence: 99%

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄

Wermink¹,

Versteeg

2017

Ind. Eng. Chem. Res.

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The oxidation of ferrous ions in acidic sulfate solutions at elevated air pressures was investigated. The effect of the Fe2+ concentration, initial H2SO4 concentration and partial oxygen pressure on the reaction rate were determined at three different temperatures, that is, T = 90, 70, and 50 °C. The effect on the reaction rate of the components that H2SO4 dissociates into, that is, HSO4 –, H3O+, and SO4 2–, was established as well. A second order of reaction in Fe2+ and a first order of reaction in O2 were determined. No clear order in either H2SO4 or the components H2SO4 dissociates into, could be established. For the experiments with initial concentrations of H2SO4 of 1 M and higher the oxidation rate was not affected, that is, a zero order of reaction in H2SO4 for these concentrations. Therefore, the kinetic rate expression for the oxidation of Fe2+ at concentrations of H2SO4 of 1 M and higher can be calculated with R Fe2+ = d[Fe2+]/dt = k[Fe2+]2 P O2 , where the activation energy E A was determined to be 60.3 kJ/mol.

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Section: Literature Reviewmentioning

confidence: 99%

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄

Wermink¹,

Versteeg

2017

Ind. Eng. Chem. Res.

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“…The residual concentration of Fe 2+ in the solution after oxidation reaction was determined by chemical titration. It is widely reported that potassium permanganate (KMnO 4 ) can be used as the titrant to determine the concentration of Fe 2+ [18]. KMnO 4 at 0.02 mol/L was prepared.…”

Section: Experimental Methodsmentioning

confidence: 99%

Strengthened Oxygen Oxidation of Ferrous Ions by A Homemade Venturi Jet Microbubble Generator towards Iron Removal in Hydrometallurgy

Niu

Lin³

et al. 2021

Minerals

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Iron normally exists in the form of ferrous ion (Fe2+) in primary ore deposits of valuable metals. To remove iron from hydrometallurgical leaching solution or suspension by precipitation, ferrous ion should be oxidized to ferric ion (Fe3+) first. Due to the low oxidation rate of Fe2+ by the traditional oxygen oxidation method, industry has to use more agitating barrels, steam, and compressed gas, as well as a larger workshop area, which dramatically increases the equipment investment and operation costs. In this study, a strengthened oxygen oxidation method for Fe2+ using a homemade venturi jet microbubble generator is proposed. Microbubbles of air, oxygen, or oxygen-enriched air can be formed in the leaching solution or suspension, which can greatly improve the dissolved oxygen content in the solution and increase the gas-liquid contact area, thereby accelerating the oxygen oxidation rate of Fe2+ to Fe3+ and realizing the rapid iron removal of the leaching solution or suspension. By measuring the residual concentration of Fe2+ in the solution after oxidation reaction, it was found that the pump power, solution temperature, pH, concentration of Cu2+, and solution flow rate had great effects on the oxidation performance of the produced microbubble. By analyzing the images of the microbubbles and measuring the dissolved oxygen content in the solution, it is confirmed that the accelerated oxidation reaction rate of Fe2+ using the new proposed method was mainly due to the increase of the dissolved oxygen amount in the solution. Moreover, this method can significantly increase the purification depth of iron ion, expand production capacity, and decrease energy consumption.

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“…Therefore, even a small amount of dissolved iron in the leaching system can have a significant effect on the rate of reaction, particularly at high temperatures where the rate of ferrous to ferric oxidation by oxygen is a rapid process (Chmielewski and Charewicz, 1984;Lu and Dreisinger, 2013;Vračar and Cerović, 1997). On adding reaction (3) to reactions (4) and (5), the overall reactions (1) and (2) are obtained.…”

Section: Accepted Manuscriptmentioning

confidence: 98%

Kinetics of the pressure leaching of enargite in FeSO4–H2SO4–O2 media

2015

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Kinetics of oxidation of Fe(II) ions by gaseous oxygen at high temperatures in an autoclave

Cited by 25 publications

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The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄

Strengthened Oxygen Oxidation of Ferrous Ions by A Homemade Venturi Jet Microbubble Generator towards Iron Removal in Hydrometallurgy

Kinetics of the pressure leaching of enargite in FeSO4–H2SO4–O2 media

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Kinetics of oxidation of Fe(II) ions by gaseous oxygen at high temperatures in an autoclave

Cited by 25 publications

References 0 publications

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H2SO4

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H2SO4

Strengthened Oxygen Oxidation of Ferrous Ions by A Homemade Venturi Jet Microbubble Generator towards Iron Removal in Hydrometallurgy

Kinetics of the pressure leaching of enargite in FeSO4–H2SO4–O2 media

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The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄

The Oxidation of Fe(II) in Acidic Sulfate Solutions with Air at Elevated Pressures. Part 1. Kinetics above 1 M H₂SO₄