Journal of Applied Electrochemistry

, Volume 39, Issue 8, pp 1267–1272 | Cite as

Cathodic reaction kinetics and its implication on flow-assisted corrosion of aluminum alloy in aqueous ethylene glycol solution

Original Paper


The cathodic reaction kinetics and anodic behavior of Al alloy 3003 in aerated ethylene glycol–water solution, under well-controlled hydrodynamic conditions, were investigated by various measurements using a rotating disk electrode (RDE). The transport and electrochemical parameters for cathodic oxygen reduction were fitted and determined. The results demonstrate that the cathodic reaction is a purely diffusion-controlled process within a certain potential region. The experimentally fitted value of diffusion coefficient of oxygen is 3.0 × 10−8 cm2 s−1. The dependence of cathodic current on rotation speed was in quantitative agreement with Levich equation. At potentials more positive than the diffusion controlled region, the cathodic process was controlled by both diffusion and electrochemical kinetics. The electrochemical reaction rate constant, k 0, was determined to be 1.1 × 10−9 cm s−1. There is little effect of electrode rotation on anodic behavior of Al alloy during stable pitting. However, fluid hydrodynamics play a significant role in formation of the oxide film and the Al alloy passivity. An enhanced electrode rotation would increase the mass-transfer rate of solution, and thus the oxygen diffusion towards the electrode surface for reduction reaction. The generated hydroxide ions are favorable to the formation of Al oxide film on electrode surface.


Electrochemical corrosion Aluminum alloy Cathodic process Ethylene glycol Fluid hydrodynamics 



This work was supported by Canada Research Chairs Program, Natural Science and Engineering Research Council of Canada (NSERC) and Dana Canada Corporation.


  1. 1.
    Szklarska-Smialowska Z (1999) Corros Sci 41:1743CrossRefGoogle Scholar
  2. 2.
    Frankel GS (1998) J Electrochem Soc 145:2186CrossRefGoogle Scholar
  3. 3.
    Miller WS, Zhuang L, Bottema J, Wittebrood AJ, De Smet P, Haszler A, Vieregge A (2000) Mater Sci Eng A280:37Google Scholar
  4. 4.
    De Micheli SM (1978) Corros Sci 18:605CrossRefGoogle Scholar
  5. 5.
    Baumgartner M, Haesche H (1990) Corros Sci 31:231CrossRefGoogle Scholar
  6. 6.
    Niu L, Cheng YF (2007) J Mater Sci 42:8613CrossRefGoogle Scholar
  7. 7.
    Niu L, Cheng YF (2008) Wear 265:367CrossRefGoogle Scholar
  8. 8.
    Levich VG (1962) Physicochemical hydrodynamics. Prentice-Hall, Englewood Cliffs, NJGoogle Scholar
  9. 9.
    Bard AJ, Faulkner FR (2004) Electrochemical methods: fundamentals and applications. Kluwer Academic Publishers, NJGoogle Scholar
  10. 10.
    Greef R, Peat R, Peter LM (1985) Instrumental methods in electrochemistry. Ellis Horwood Ltd, Chichester, UKGoogle Scholar
  11. 11.
    King F, Quin MJ, Litke CD (1995) J Electroanal Chem 385:45CrossRefGoogle Scholar
  12. 12.
    Kear G (2007) Electrochim Acta 52:1889CrossRefGoogle Scholar
  13. 13.
    Pourbaix M, Deltombe E, Vanleugenhaghe C (1966) Atlas of electrochemical equilibria in aqueous solutions. Pergamon Press, OxfordGoogle Scholar
  14. 14.
    Macdonald DD (1992) J Electrochem Soc 139:3434CrossRefGoogle Scholar
  15. 15.
    Raja KS, Jones DA (2006) Corros Sci 48:1623CrossRefGoogle Scholar
  16. 16.
    Zhang GA, Xu LY, Cheng YF (2008) Electrochim Acta 53:8245CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media B.V. 2009

Authors and Affiliations

  1. 1.Department of Mechanical & Manufacturing EngineeringUniversity of CalgaryCalgaryCanada

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