Corrosion
1 – Corrosion : Definition
1 – The electrochemical’s basis of corrosion An example : the iron
The equation for the corrosion of the Iron •Anode : Fe(s) -> + Fe2+(aq) + 2e• Cathode O2(g) + 2H2O(l) + 4e- -> 4OH-(aq) • The overall cell reaction: Fe2+(aq) + 2OH-(aq) -> Fe(OH)2(s) •Rust reaction: (OH)2(s) + O2(g) -> 2Fe2O3 •H2O(s) + 2H2O(l)
1 – Nerst’s Equation
R: universal gas constant T: Absolute temperature n: number of electrons involved F: Faraday constant E is the standard potential of the metal [Men +] concentration of metal ions in the solution
The Nernst equation is a very important equation in electrochemistry because it relates the potential E of the cells with the standard potential E0 and activity / concentration of the electroactive ion
1-Galvanic Series
1- Kinetic of corrosion: Faraday’s law
W : Weight (g) A : Atomic weight n : number of electron i : electrical intensity (A) t : Time (s) F : Faraday constant → If you replace i by the density of current you can find the thickness which is corroded
1- Tafel’s Straights
Potential Cathode
Ecor
Anode
icor
Log i
1- Curve of polarization for passivables materials
E Transpassive domain
2
1
Passive
3 4
Active estate
Log i
2 – Corrosion of Reinforcement
8
• Anodic reaction : Fe
Fe2+ + 2e2OH-
• Cathodic reaction: ½ O2 +H2O+ 2e• Fe2+ + 2OHFe(OH)2 Rust
2.A - Consequences
9 • Reduction of strength capacity: reduced cross-sectional area of steel • Loss of bond between the steel and the concrete • Rust drip esthetic • Increasing of the volume due to rust cracking, spalling…
2.B – Factors influencing the Corrosion
10 • Presence of chlorides • Deterioration of concrete cover: physical, mecanical and chemical causes • Concrete porosity • CO2 in the atmosphere
2.C – Stages of Corrosion
11
• Initiation: depassivation • Propagation • Concrete cracking
(1) initiation