Influence of anion adsorption on the action of inhibitors on the acid corrosion of iron and cobalt

Iofa, Z.A.; Батраков, В. В.; Cho-Ngok-Ba,

doi:10.1016/0013-4686(64)80091-8

Cited by 140 publications

(69 citation statements)

References 3 publications

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“…Similarly, recent 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 studies on acetic acid corrosion also showed that a direct reduction was not likely [15], also confirming older thoughts [3]. On the other hand, studies on H 2 S corrosion were mainly focused on anodic mechanism or on the formation of FeS scale formation [8,[16][17][18][19]. Electrochemical aspects of H 2 S benefited much less investigations, though it was found to have strong impact on the cathodic current density [1,8,20].…”

Section: Introductionmentioning

confidence: 67%

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Tribollet

Kittel

Meroufel

et al. 2014

Electrochimica Acta

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1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 55 56 57 58 59 60 61 62 63 64 65 Corrosion mechanisms in aqueous solutions containing dissolved H 2 S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode. AbstractIn H 2 S containing solutions, the reduction of protons with a buffer effect contributing to the transport of protons at the steel surface, is not sufficient to explain the cathodic polarization curves obtained on 316L stainless steel. An additional electrochemical reaction was observed and was attributed to a direct H 2 S reduction. A numerical model is presented with these hypotheses and a good agreement is found with the experimental data presented in a previous paper. With this model it is also possible to present the concentration profiles of the different species involved in the cathodic process.

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Section: Introductionmentioning

confidence: 67%

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Tribollet

Kittel

Meroufel

et al. 2014

Electrochimica Acta

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“…FeSHt species has been proposed in electrochemical studies of iron in aqueous H2S solutions (24,25), and by Pohl (26) for the formation of FeS troilite. Sinlilarly NiSH' has been proposed in corrosion studies of nickel in H,S solutions (27).…”

Section: Thern~ocl~cr~iical Quaritities and Difusiorz Coejicientmentioning

confidence: 98%

Dissolution of iron during the initial corrosion of carbon steel in aqueous H₂S solutions

Tewari¹,

Campbell²

1979

Can. J. Chem.

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PARAM H . TEWARI and ALLAY B. CAMPBELL. Can. J. Chem. 57,188 (1979). The dissolution of iron from carbon steel in aqueous H,S solutions has been studied as a function of time and temperature at 0.1 MPa H,S pressure using the rotating disc technique. The iron sulfide film formed on the disc surface has been identified by X-ray diffraction analysis. The solubility and dissolution rate of synthesized mackinawite, FeS,,_,,, have also been determined to help establish the mechanism of release of iron from carbon steel corroding in aqueous H2S solutions.The rate data have been analysed by an equation for a joint chemical and transport controlled process. At 22°C and 0.1 MPa H2S, the maximum rate of release of Fez+, obtained by extrapolating the data to infinite rotation speed, is 7.4 i 0.5 ~m o l / m 2 s. This is similar to the dissolution rate determined for synthesized mackinawite powders, but is 20 times faster than the rate of dissolution for troilite and more than 1000 times faster than the dissolution rates for pyrrhotite and pyrite. Thus, troilite and iron sulfide phases that form subsequently are not major contributors to Fe2+ release during the corrosion of carbon steel.At 22'C the diffusion coefficient for the FeSH+ ion is (1.4 i 0.2) x 1 0 m2/s and the activation energy of the diffusion process is 25 i 7 kJ/mol. The chemical reaction occurring at the surface has a n activation energy of 77 +_ 14 kJ,'mol.It is concluded that the release of iron from corroding carbon steel is governed by the dissolution rate of mackinawite, the initial corrosion product. This dissolution is controlled by the chemical reaction between mackinawite and H + and by the transport of the complexed FeSH' from the interface to the bulk solution.PARAM H . TEWARI et ALLAK B. CAMPBELL. Can. J. Chem. 57, 188 (1979). Faisant appel a la technique du disque rotatif, on a etudie la mise en solution du fer d'aciers au carbone dans des solutions aqueuses de H2S en fonction du temps et de la temperature, a une pression de 0.1 MPa de H,S. Gr2ce a une analyse par diffraction de rayons-)<, on a identifie le film de sulfure de fer qui se forme a la surface du disque. On a aussi determine la solu- jusqu'a une vitesse de rotation infinie est egal a 7.4 + 0.5 ynlol/mz s. Cette valeur est semblable au taux de dissolution determine pour des poudres de mackinawite rnais elle est 20 fois plus rapide que celle determinee pour la dissolution de la troilite et plus de 1000 fois plus grande que les valeurs correspondantes pour la pyrrhotite et la pyrite. Donc les phases du troilite et de sulfure de fer qui se forment subsequemment ne contribuent pas d'une f a~o n importante a la mise en liberte du Fe2+ au cours de la corrosion des aciers au charbon.A 22"C, le coefficient de diffusion de I'ion FeSH+ est (1.4 + 0.2) x m2/s et I'energie d'activation du processus de diffusion est 25 +_ 7 kJ/mol. L'Cnergie d'activation de la reaction chimique se produisant a la surface est 77 i 14 kJ/mol.On en conclut que la mise en liberte du fer par un acier au charbon soumis a u...

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“…Biogenic sulfide may initially stimulate the anodic part of the corrosion reaction by chemisorption and direct reaction with metallic iron (65,109,110). However, once the metallic surface is covered with inorganic corrosion products such as FeS, cathodic reactions become more important drivers of metal oxidation (81).…”

Section: Emic Versus Cmic-emerging Theories In Srb-induced Corrosionmentioning

confidence: 99%

Corrosion of Iron by Sulfate-Reducing Bacteria: New Views of an Old Problem

Enning

Garrelfs

2014

Appl Environ Microbiol

660

414

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About a century ago, researchers first recognized a connection between the activity of environmental microorganisms and cases of anaerobic iron corrosion. Since then, such microbially influenced corrosion (MIC) has gained prominence and its technical and economic implications are now widely recognized. Under anoxic conditions (e.g., in oil and gas pipelines), sulfate-reducing bacteria (SRB) are commonly considered the main culprits of MIC. This perception largely stems from three recurrent observations. First, anoxic sulfate-rich environments (e.g., anoxic seawater) are particularly corrosive. Second, SRB and their characteristic corrosion product iron sulfide are ubiquitously associated with anaerobic corrosion damage, and third, no other physiological group produces comparably severe corrosion damage in laboratory-grown pure cultures. However, there remain many open questions as to the underlying mechanisms and their relative contributions to corrosion. On the one hand, SRB damage iron constructions indirectly through a corrosive chemical agent, hydrogen sulfide, formed by the organisms as a dissimilatory product from sulfate reduction with organic compounds or hydrogen ("chemical microbially influenced corrosion"; CMIC). On the other hand, certain SRB can also attack iron via withdrawal of electrons ("electrical microbially influenced corrosion"; EMIC), viz., directly by metabolic coupling. Corrosion of iron by SRB is typically associated with the formation of iron sulfides (FeS) which, paradoxically, may reduce corrosion in some cases while they increase it in others. This brief review traces the historical twists in the perception of SRB-induced corrosion, considering the presently most plausible explanations as well as possible early misconceptions in the understanding of severe corrosion in anoxic, sulfate-rich environments. E ver since its first production roughly 4,000 years ago, iron has played a central role in human society due to its excellent mechanical properties and the abundance of its ores. Today, iron is used in much larger quantities than any other metallic material (1) and is indispensable in infrastructure, transportation, and manufacturing. A major drawback is the susceptibility of iron to corrosion. Corrosion of iron and other metals causes enormous economic damage. Across all industrial sectors, the inferred costs of metal corrosion have been estimated to range between 2% and 3% of gross domestic product (GDP) in developed countries (2, 3). These costs are to a large extent caused by corrosion of iron, due to its abundant use and particular susceptibility to oxidative damage. Estimates of the costs attributable to biocorrosion of iron lack a computed basis so that they vary widely, and definite numbers cannot be given with certainty. Still, microbially influenced corrosion (MIC) probably accounts for a significant fraction of the total costs (4-7), and, due to its effects on important infrastructure in the energy industry (such as oil and gas pipelines), costs in the range of billions of...

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Influence of anion adsorption on the action of inhibitors on the acid corrosion of iron and cobalt

Cited by 140 publications

References 3 publications

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Dissolution of iron during the initial corrosion of carbon steel in aqueous H₂S solutions

Corrosion of Iron by Sulfate-Reducing Bacteria: New Views of an Old Problem

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Influence of anion adsorption on the action of inhibitors on the acid corrosion of iron and cobalt

Cited by 140 publications

References 3 publications

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Corrosion mechanisms in aqueous solutions containing dissolved H2S. Part 2: Model of the cathodic reactions on a 316L stainless steel rotating disc electrode

Dissolution of iron during the initial corrosion of carbon steel in aqueous H2S solutions

Corrosion of Iron by Sulfate-Reducing Bacteria: New Views of an Old Problem

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Dissolution of iron during the initial corrosion of carbon steel in aqueous H₂S solutions