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6. Electrochemical reaction kinetics

6.7. Corrosion

In corrosion, two simultaneous reactions are taking place on a metal surface so that the anodic current is equal but opposite in sign to the cathodic current, Ia = |Ic| = Icorr, the corrosion current. Although the net current in corrosion is zero the exchange current can be quite high. Since the anodic and cathodic reactions are not directly connected to one another, their potential dependence and charge transfer coefficients (\( \alpha \)) are mutually independent. The metal surface is settled at a corrosion potential Ecorr where the net current is zero. The corrosion potential does not represent a true thermodynamic equilibrium because reactions are proceeding, and it can also vary during the corrosion process as the surface areas involved in the anodic and cathodic reactions change as corrosion progresses.

The dissolution of a metal can be written as an anodic reaction


M   \(\ce{ -> }\)   Mn+   +   ne- (6.105)


                                                                                              

A cathodic reaction that balances the electric charge depends on the pH of the solution. In a neutral or acidic solution they are

O2   +   4 H+   +   4 e–   \(\ce{ \bond{->} }\) 2 H2O      (neutral)  (6.106a)
2 H+   +   2 e–   \(\ce{ \bond{->} }\)  H2                         (acidic)
 (6.106b)
                                                   

In an alkaline solution, the following reactions are possible:

 O2   +   2 H2O   +   4 e–   \(\ce{ \bond{->} }\)   4 OH–   (6.107a)
2 H2O   +   2 e–   \(\ce{ \bond{->} }\)   H2   +   2 OH– (6.107b)
                                                              

Corrosion is often accompanied by the formation of an oxide film on the metal surface. Such a film is a poor charge carrier (semi-conductor) and passivates the surface, preventing further corrosion. Several metals such as various types of steel, chromium, aluminium, zirkonium, tantalum and titanium form a passivating film, the properties of which determine their corrosion resistance. Copper forms a stable Cu2O film or patina that gives the characteristic beautiful color to copper surfaces.

When the potential of steel is increased, increases corrosion current exponentially until a maximum current reached. Thereafter current drops nearly to zero due to a passivating oxide film.

Figure 6.11. When the potential of steel is increased, this increases corrosion current exponentially until a maximum current reached. Thereafter the current drops to nearly zero due to a passivating oxide film.

Table 6.1. Passivation potential of selected metals, EF0   (potential with the maksimum corrosion current); pH = 0, T = 298 K. (J.O’M. Bockris and A.K.N. Reddy, Modern Electrochemistry, Plenum Press, New York 1970, s. 1317.)

Metal

EF0   / V vs. NHE

Au

+1.36

Pt

+0.91

Fe

+0.58

Ag

+0.40

Ni

+0.36

Cr

-0.22

Ti

-0.24

A great deal of corrosion studies concern iron (steel) due to its immense industrial significance. A qualitative current-voltage curve of steel in Figure 6.11 shows the passivation of the film and the termination of corrosion at potentials which are positive to the Flade potential.

The Flade potential is a linear function of pH and often of the form

\( E_{\text{F}}=E_{\text{F}}^0-\text{pH} \times 0.059{\text{ V}} \) (6.108)

One of the oldest and best known results about the corrosion of iron is that it dissolves readily in diluted nitric acid but not in concentrated nitric acid. Iron dissolution is:

Fe   →   Fe2+   +   2 e-  (6.109)

The cathodic reaction is the reduction of nitrate:

NO3-     +   2 H+   +   2 e-   →   NO2   +   H2O      (6.110)

Looking at reaction (6.110), the reaction rate should increase at a lower pH contrary to Equation (6.108). Obviously the corrosion of iron is determined by kinetics, and a purely thermodynamic analysis based on, for example, Bourbaix diagrams (Chapter 4) does not give the real picture. Based on Figure 6.11, it can be concluded that in very acidic conditions the corrosion potential of iron is on the negative side of the Flade potential and in moderately acidic solutions on its positive side. The impedance analysis of corrosion is discussed in Chapter 9.


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