The spreading of sulphate nests on steel in atmospheric corrosion

Bartoň, K.; Kuchynka, D. J.; Bartoňová, Zuzana; Beránek, E.

doi:10.1016/s0010-938x(71)80038-0

Cited by 22 publications

(7 citation statements)

References 10 publications

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“…Eventually the membrane bursts, spreading its contents to adjacent areas to stimulate corrosion there. Laboratory results appear to be consistent with this scenario (86), and sulfur appears on field samples in a nonuniform pattern (23) and surrounding areas where corrosion is occurring (84). The scenario is only an overview and not a complete mechanistic description, because (i) the mechanism cannot explain the finding (12,73,87) that steel exposed initially during the winter tends to corrode more rapidly than does steel initially exposed in the summer, and (ii) no analytical evidence exists for the constraining hydroxide "membranes."…”

Section: Table II Expected Upper Limits For Ratios Of Metal Complex [...supporting

confidence: 56%

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Graedel

Frankenthal

1990

J. Electrochem. Soc.

141

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Despite extensive study over the years, the chemical processes involved in the atmospheric corrosion of iron and its alloys remain poorly understood. Most conceptual studies have ignored the chemical influence of the trace anions (CI-, NO~ , SO42-, CO2H , etc.) present in the atmosphere and in precipitation. This review, presented from the perspective of atmospheric chemistry and mineralogy, provides an analysis of rust layer formation, evolution, morphology, and composition, together with information on iron-containing minerals and other crystalline structures that are likely to be present. The chemical reactions involved in the formation of these constituents during the corrosion process are then presented. The reactions are not spatially homogeneous, but favor pits, voids, and crevices in the metal surface. It is demonstrated that (i) the pH of the moisture on the surface is crucial to the corrosion process, since it controls the dissolution of the passive oxyhydroxide surface; the pH is largely controlled by atmospheric SO2 and NOx dissolved in the moisture or by fog or rain deposited on the surface; (ii) the extant data suggest that the rate of iron oxyhydroxide formation is slow; hence, the presence of reactive anions generally results in their blending into mixed hydroxy-anion products; (iii) the interactive chemistry of readily available hydrogen peroxide and bisulfite ion in the aqueous surface film can either enhance or impede the rate of corrosion; (iv) photon-driven reactions can promote the corrosion of iron and its alloys. This analysis unifies the analytical information, as well as the data on kinetic processes, and provides the basis for a full understanding of the atmospheric corrosion of iron and low alloy steels.

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Section: Table II Expected Upper Limits For Ratios Of Metal Complex [...supporting

confidence: 56%

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Graedel

Frankenthal

1990

J. Electrochem. Soc.

141

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“…Then from reaction (81, Substituting equations (19), (20) and (16) into equation ( 18), If the unstated assumption is accepted, that the familiar relationship no longer holds, but that a(H20) can vary while a(H+)…”

Section: Step Thenmentioning

confidence: 99%

“…Schwarz explained this as being due t o oxygen exclusion from the surface, preventing oxidation, and enclosure of the FeS04 nest by an FeOOH membrane, which would act as an ion exchange membrane and restrict movement of the SO4 -ions. barto6 et al ( 19) have proposed a mechanism for the action of the nests, based on the existence of such a membrane. In this, they suggest that the membrane cracks periodically due t o osmotic and electrolytic transport into the nest, which cause an increase in internal pressure.…”

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confidence: 99%

Analyses of Some Suggested Mechanisms for Atmospheric Corrosion of Iron in Presence of So₂

Duncan

1974

Materials & Corrosion

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Dealuminization of Aluminium Bronzes. Mod. Castings 45 (1 964) 13. B. Upton; Corrosion Resistance in Sea Water of Medium Strength 14. R. B, Niederberger: Composition and Heat Treatment Effect on 115-128. 15. Z. Tanabe: Effect of Metal Composition and Heat Treatment on De-Aluminification of Cu-A1 Alloys. Corrosion Sci. 4 (1964) 413-423. 16. I ; . Gaillard und A . R . Weill: Etude au potentiostat de la desaluminisation de quelques nuances d'alliages cuproaluminium. Mem. Sci. Rev. Met. 61 (1964) 437-450. 17. S. Goldspiel, J. Kershner und G. Wacker: Heat Treatment, Microstructure and Corrosion Resistance of Aluminium Bronze Castings. Mod. Castings 47 (1965) 818-823. 18. D. Arnaud, R. Paton, S. Wigy und C. Maser&: Contribution 2 l'e'tude de la desaluminisation des cupro-aluminiums moule's. Me' m. Sci. Rev. Me't. 62 (1965) 89-116. verses phaws d un alliage cuivreux; MPmorial de 1 Artillerie Fran-20. F. Gaillurd: Der EinfluD von Nickel auf die Entaluminierung von Kupfer-Aluminium-Legierungen. Cuivre Laitons Alliages 99 3 9. M. Climeau: De'termination du potentiel de dissolution des diCaise 41 (1967) 973-993. (1967) 21-37. 21. P. Sury: Untersuchungen zum Gefugeaufbau und Korrosionsverhalten von Aluminiumbronzen. Dissertation Universitat Ziirich, 1970.

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“…Some of these are given below (Dehri et al , 1994; Nunez et al , 2005; Mendoza et al , 2004; Kılınççeker and Galip, 2008; Kılınççeker, 2008; Babic and Metikoš‐Hukovic, 1993): Equation 5 Equation 6 The sulfate ion formed in equation (4) is changed to sulfuric acid in wet medium. It is also known that brass exposed to an atmosphere containing SO 2 starts corroding with the zinc metal in its structure, and this is selectively removed from the alloy (Tüken et al , 2004, 2005; Özcan and Dehri, 2004; Dehri et al , 2003; Özcan et al , 2002; Doğan and Kılınççeker, 2006; Menekşe and Kılınççeker, 2007; Ackson et al , 2000; Michailovski and Sokolov, 1985; Crundwell, 1993; Abayarathna et al , 1991; Gad‐Allah et al , 1991; Ailor, 1971; Askey et al , 1993; Barton et al , 1971; Tuncay et al , 2005; Baugh and White, 1987a, b; Cabot et al , 1993; Kabasakaloğlu et al , 2002; Aytaç et al , 2005; Cordeiro et al , 1993): Equation 7 Equation 8 Equation 9 In the present study, to determine the corrosion effect on metals quantitatively, SO 2 gas was passed for certain periods of time through an atmospheric corrosion test cell in which the relative humidity (rH) was adjusted to different values (60‐90 percent) by glycerin+water mixtures (Dehri et al , 1994). The corrosion rates in 100 percent rH of the metal samples; iron, copper and brass hanging down in the cell then were measured as weight loss (mdd), galvanic current density (A dm −2 ).…”

Section: Introductionmentioning

confidence: 99%

The effect of sulfur dioxide on iron, copper and brass

Kılınççeker

Taze

Galip

et al. 2011

Anti-Corrosion Methods and Materials

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PurposeThe purpose of this paper is to study, under laboratory conditions, the corrosive effect of sulfur dioxide (SO2) present in the atmosphere of urban and industrial areas on various construction materials.Design/methodology/approachIron, copper and brass metals were exposed to SO2 gas at different relative humidities that were obtained using analytical grade glycerol and water mixtures. The corrosion rates (mdd) of the samples were determined over 120 h using the weight‐loss method under fixed relative humidity (rH) conditions. The change of galvanic current was measured as a function of exposure time over 196 h. Nyquist diagrams were obtained in 10−3 M Na2SO4 solutions with a pH value of 7.2, which was assumed to correspond to 100 percent rH conditions.FindingsThe obtained data showed that the corrosion rate of the studied metals increased with increasing rH. The corrosion rate of the metals decreased with exposure time, due to accumulation of corrosion products over the surface of the metals. However, the surface films of corrosion products on the metal surfaces were not stable and the corrosion rate increased again with time when the surface film disappeared.Research limitations/implicationsThe atmospheric corrosion of the industrial materials is dependent upon the rH and SO2 concentration. The corrosive effect of SO2 present in the atmosphere of urban and industrial areas on various construction materials can be tested under laboratory conditions.Originality/valueThe effects of SO2 and NH3 on the atmospheric corrosion of galvanized iron and the effect of rH on the atmospheric corrosion of defective organic coating materials were reported in literature. In this study, the corrosive effect of SO2 present in the atmosphere of urban and industrial areas on various construction materials (iron, copper and brass) under laboratory conditions was studied.

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The spreading of sulphate nests on steel in atmospheric corrosion

Cited by 22 publications

References 10 publications

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Analyses of Some Suggested Mechanisms for Atmospheric Corrosion of Iron in Presence of So₂

The effect of sulfur dioxide on iron, copper and brass

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The spreading of sulphate nests on steel in atmospheric corrosion

Cited by 22 publications

References 10 publications

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Corrosion Mechanisms for Iron and Low Alloy Steels Exposed to the Atmosphere

Analyses of Some Suggested Mechanisms for Atmospheric Corrosion of Iron in Presence of So2

The effect of sulfur dioxide on iron, copper and brass

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Analyses of Some Suggested Mechanisms for Atmospheric Corrosion of Iron in Presence of So₂