Chapter 9 - Corrosion | Galvanic Corrosion Flashcards
Describe the process of Galvanic corrosion?
When two metals are connected in a electrolyte solution, electrons will flow from the anode to cathode cause corrosion
What are the 3 main parts of an electrochemical or ‘Galvanic’ Cell?
- Anode
- Cathode
- Electrolyte solution
What is an Anode?
the site where the metal is corroded
What is a Cathode?
Can be the same metal or part of a different one but it is the part of the cell that is protected
What is the electrolyte solution?
This is the corrosive medium which is electrically conductive
where does the reduction reaction occur?
At the cathode
gain of electrons
Where does the oxidation reaction occur?
At the anode
loss of electrons
Which metal is more likely to corrode?
The metal with the more negative electrode potential
What is the standard reduction potential?
If a metal is immersed in a solution of its own
ions there will be a voltage, or potential, at which
equilibrium exists between the metal and solution
Will the more active metal be lower or higher in the standard reduction potential data?
Lower
What happens when you connect dissimilar metals in an electrolyte solution?
The anode will corrode
Whats stages should you go through when designing for galvanic corrosion?
- Material slesction
- Eliminate electrolyte
- Galvanic of anodic protection
- Make anode easily replaceable
