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Title: The anodic behavior of iron in hydrogen sulfide solutions

Abstract

The anodic behavior of iron in 0.032 mol . L/sup -1/ NaCl/0.003 mol . L/sup -1/ NaHCO/sub 3/ and 1 mol . L/sup -1/ Na/sub 2/SO/sub 4//0.003 mol . L/sup -1/ NaHCO/sub 3/ solutions containing 0.05 mol . L/sup -1/ H/sub 2/S at ambient temperature was studied using cyclic voltammetry and the potentiostatic technique. In both solutions, a nonprotective film of mackinawite (Fe/sub 1+chi/S) was formed on the iron, but the film growth kinetics differ for the two solutions. The film growth in chloride solutions does not appear to follow a conventional type of model for multilayer fils whereas the formation of the film in sulfate solutions can be represented in terms of a pre-resistance model. At more anodic potentials, the mackinawite is oxidized to a higher sulfide, possibly pyrite (FeS/sub 2/), as suggested from a comparison of the anodic and cathodic peak potentials with the equilibrium potential. The formation of the higher sulfide(s) in the chloride solution appears to follow a similar film growth mechanism to that for mackinawite, whereas it is not clear whether this is the case for the sulfate solution.

Authors:
 [1]; ;  [2]
  1. SRI International, Menlo Park, CA (USA)
  2. Auckland Univ. (New Zealand). Dept. of Chemistry
Publication Date:
OSTI Identifier:
5374980
Resource Type:
Journal Article
Journal Name:
Corrosion (Houston); (USA)
Additional Journal Information:
Journal Volume: 45:5; Journal ID: ISSN 0010-9312
Country of Publication:
United States
Language:
English
Subject:
36 MATERIALS SCIENCE; 37 INORGANIC, ORGANIC, PHYSICAL AND ANALYTICAL CHEMISTRY; HYDROGEN SULFIDES; CORROSIVE EFFECTS; IRON; CHEMICAL REACTION KINETICS; IRON SULFIDES; THIN FILMS; SOLUTIONS; ANODES; CHLORIDES; ELECTROCHEMISTRY; POTENTIOSTATS; SODIUM CARBONATES; SODIUM SULFATES; VOLTAMETRY; ALKALI METAL COMPOUNDS; CARBON COMPOUNDS; CARBONATES; CHALCOGENIDES; CHEMISTRY; CHLORINE COMPOUNDS; DISPERSIONS; ELECTRODES; ELEMENTS; FILMS; HALIDES; HALOGEN COMPOUNDS; HYDROGEN COMPOUNDS; IRON COMPOUNDS; KINETICS; MEASURING INSTRUMENTS; METALS; MIXTURES; OXYGEN COMPOUNDS; REACTION KINETICS; SODIUM COMPOUNDS; SULFATES; SULFIDES; SULFUR COMPOUNDS; TRANSITION ELEMENT COMPOUNDS; TRANSITION ELEMENTS; 360105* - Metals & Alloys- Corrosion & Erosion; 400400 - Electrochemistry; 400201 - Chemical & Physicochemical Properties

Citation Formats

Pound, B G, Wright, G A, and Sharp, R M. The anodic behavior of iron in hydrogen sulfide solutions. United States: N. p., 1989. Web. doi:10.5006/1.3582033.
Pound, B G, Wright, G A, & Sharp, R M. The anodic behavior of iron in hydrogen sulfide solutions. United States. https://doi.org/10.5006/1.3582033
Pound, B G, Wright, G A, and Sharp, R M. 1989. "The anodic behavior of iron in hydrogen sulfide solutions". United States. https://doi.org/10.5006/1.3582033.
@article{osti_5374980,
title = {The anodic behavior of iron in hydrogen sulfide solutions},
author = {Pound, B G and Wright, G A and Sharp, R M},
abstractNote = {The anodic behavior of iron in 0.032 mol . L/sup -1/ NaCl/0.003 mol . L/sup -1/ NaHCO/sub 3/ and 1 mol . L/sup -1/ Na/sub 2/SO/sub 4//0.003 mol . L/sup -1/ NaHCO/sub 3/ solutions containing 0.05 mol . L/sup -1/ H/sub 2/S at ambient temperature was studied using cyclic voltammetry and the potentiostatic technique. In both solutions, a nonprotective film of mackinawite (Fe/sub 1+chi/S) was formed on the iron, but the film growth kinetics differ for the two solutions. The film growth in chloride solutions does not appear to follow a conventional type of model for multilayer fils whereas the formation of the film in sulfate solutions can be represented in terms of a pre-resistance model. At more anodic potentials, the mackinawite is oxidized to a higher sulfide, possibly pyrite (FeS/sub 2/), as suggested from a comparison of the anodic and cathodic peak potentials with the equilibrium potential. The formation of the higher sulfide(s) in the chloride solution appears to follow a similar film growth mechanism to that for mackinawite, whereas it is not clear whether this is the case for the sulfate solution.},
doi = {10.5006/1.3582033},
url = {https://www.osti.gov/biblio/5374980}, journal = {Corrosion (Houston); (USA)},
issn = {0010-9312},
number = ,
volume = 45:5,
place = {United States},
year = {Mon May 01 00:00:00 EDT 1989},
month = {Mon May 01 00:00:00 EDT 1989}
}