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An electrochemical method of measuring the oxidation rate of ferrous to ferric iron with oxygen in the presence of Thiobacillus ferrooxidans
Author(s) -
Pesic B.,
Oliver D. J.,
Wichlacz P.
Publication year - 1989
Publication title -
biotechnology and bioengineering
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 1.136
H-Index - 189
eISSN - 1097-0290
pISSN - 0006-3592
DOI - 10.1002/bit.260330408
Subject(s) - ferrous , redox , chemistry , oxygen , inorganic chemistry , electrochemistry , pyrite , ferric , platinum , reaction rate , sulfate , electrode , mineralogy , catalysis , biochemistry , organic chemistry
The oxidation of Fe 2+ with oxygen in sulfate solutions was studied in the presence of T. ferrooxidans . To measure the chemical activity of bacteria, and the oxidation rate of iron, the redox potentials of solutions were continuously monitored during the experiments. The redox potentials were simultaneously monitored on the platinum and pyrite indicator electrodes. The redox potential versus time curves were further used to calculate the basic kinetic parameters, such as the reaction orders, the activation energy, and the frequency factor. It was found that under atmospheric conditions, and at Fe 2+ < 0.001 M , T < 25°C, and at pH above 2.2, the oxidation of iron is governed by the following rate expression:\documentclass{article}\pagestyle{empty}\begin{document}$$ - \frac{{d[{\rm Fe}^{2 + }]}}{{dt}} = 1.62 \times 10^{11} C_{{\rm bact}} [{\rm H}^ + ][{\rm Fe}^{2 + }]p{\rm O}_2 e^{ - (58.77/RT)} $$\end{document} Below pH = 2.2, the oxidation rate is independent of H + Concentration.