Ferrate(VI) oxidation of hydrogen sulfide

Virender K. Sharma, Jeremy O. Smith, Frank J. Millero

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119 Scopus citations


The rates of oxidation of hydrogen sulfide with Fe(VI) were made anaerobically as a function of pH (7-12) and temperature (5-15 °C). The reaction was found to be first order for each reactant. The rates decrease with an increase in pH. The energy of activation was found to be 30.1 ± 4.9 kJ mol-1 at pH = 12. When the concentrations of [H2S]T ([H2S] + [HS-]) are in excess, the ratio of [H2S]T consumed to [Fe(VI)] consumed was 1.51 ± 0.14 at pH = 70 and 2.50 ± 0.13 at pH = 9.0 and 11.3. Thiosulfate was the main product at pH = 7.0; sulfite, thiosulfate, and sulfate were identified as the products of the reactions at pH = 9.0 and 11.3. In an excess of [Fe(VI)] over [H2S](T), the hydrogen sulfide is fully oxidized to sulfate. A mechanism in which Fe(VI) oxidizes H2S by a one-electron process is proposed. Experiments were conducted to test the Fe(VI) removal efficiency of sulfide in groundwater and waste-water. The results indicate that Fe(VI) can be used as an effective oxidant to remove hydrogen sulfide from wastewaters.

Original languageEnglish (US)
Pages (from-to)2486-2491
Number of pages6
JournalEnvironmental Science and Technology
Issue number9
StatePublished - Sep 1 1997

ASJC Scopus subject areas

  • Chemistry(all)
  • Environmental Chemistry


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