Dissolution of iron sulfide (troilite) in aqueous sulfuric acid

Tewari, P. H.; Campbell, Allan B.

doi:10.1021/j100558a004

Cited by 28 publications

(13 citation statements)

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“…1). T~nmediately before a run, the exposed surface of the disc was ground to within 0.3 mm of the surrounding Teflon surface as described earlier (12). The release of Fe2+ was limited to a well defined area of the exposed surface of the carbon steel disc by painting the sides and part of the surface with polyurethane paint.…”

Section: Appcrrat~rsmentioning

confidence: 99%

“…and by the transport of ~r o n hydrosulfide ion (FeSW'), desorbed from the nlackinawite surface, illto the bulk solution (eq. [7] F~t h e i FeSH -or Fe2 " may be the dlff u s~n g specles (eqs [7] or [12]) In the transport process We prefer eq [ 7 ] , \$lth FeSH' diffusion, over eq. [I21 because of the dlffetence 111 the values of the d i f f u s~o~~ coeffic~e n t of the dlffus~ng specles from that for Fe2+ given in the literature Also, as d~scussed prev~ously, abcorpt~on spectla suggest that FeSH ' 1s the r~nportant species a t pH 4 0 In aqueous H2S solut~ons.…”

Section: R Cl~anismmentioning

confidence: 99%

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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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Section: Appcrrat~rsmentioning

confidence: 99%

Section: R Cl~anismmentioning

confidence: 99%

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

Tewari¹,

Campbell²

1979

Can. J. Chem.

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“…Adsorption of Fe2+ onto goethite at acidic pH values is enhanced as the pH increases (LaKind and Stone, 1989) and may act as an additional barrier to goethite dissolution. Similarly, Tewari and Campbell (1976) have shown that the rate of anoxic dissolution of FeS (troilite) is slower as the pH increases to 6.5. This inhibition of reduction and dissolution of goethite is consistent with increased FeS saturation and therefore diminished tendency of FeS to dissolve at pH greater than 7.0.…”

Section: High Ph Resultsmentioning

confidence: 88%

Geochemical, biogeochemical, and sedimentological studies of the Green River Formation, Wyoming, Utah, and Colorado

Tuttle¹

1991

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“…Presence of hydrogen sulphide in an electrolyte strongly activates the corrosion and hydrogen absorption process in steel [1][2][3][4][5] . It has been reported that the cathodic process of corrosion of metals is depolarized due to the action of HS-or S 2-on the metal surface.…”

Section: Introductionmentioning

confidence: 99%

H2S Corrosion control of steel by using pyridine compounds

Chatterjee

Singh

1991

Anti-Corrosion Methods and Materials

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Pyridine and some of its derivatives have been evaluated as inhibitors for the corrosion of API‐45 steel in NACE sour solution. Amongst the various methyl and halogen substituted pyridine compounds, 2,4,6‐trimethyl pyridine is found to afford maximum protection followed by 2,6‐dimethyl pyridine, >2,4‐dimethyl pyridine, >3‐bromopyridine, >2‐methyl pyridine, 4‐methyl pyridine, 3,5‐dimethyl pyridine, >2 and 3‐chloropyridine>pyridine. These results have been discussed in the light of availability of the electron densities with the nitrogen atom of the pyridine ring. The inhibitive periormance of all the inhibitors is found to deteriorate with increase in temperature from 30 to 60°C and with passage of time. The values of heat of absorption and free energy of absorption indicates that the inhibitors have a chemical type of absorption at the metal/electrolyte interface. Polarization diagrams and shift in open circuit potential in the presence of inhibitors indicate that these compounds retard the cathodic as well as anodic reaction process.

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Dissolution of iron sulfide (troilite) in aqueous sulfuric acid

Cited by 28 publications

References 6 publications

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

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

Geochemical, biogeochemical, and sedimentological studies of the Green River Formation, Wyoming, Utah, and Colorado

H2S Corrosion control of steel by using pyridine compounds

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Dissolution of iron sulfide (troilite) in aqueous sulfuric acid

Cited by 28 publications

References 6 publications

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

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

Geochemical, biogeochemical, and sedimentological studies of the Green River Formation, Wyoming, Utah, and Colorado

H2S Corrosion control of steel by using pyridine compounds

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Product

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

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