Corrosion

Question 1

Corrosion

Answer 1

• The gradual destruction of metals through chemical reactions with their environment, often involving oxygen and moisture.
• Example: Rusting of iron due to reaction with water and air.

Question 2

Galvanization

Answer 2

• A process of coating metal (usually iron or steel) with a layer of zinc to protect from corrosion. The zinc layer acts as a sacrificial anode, corroding instead of the underlying metal.
• Example: Galvanized steel is used in outdoor structures to prevent rust.

Question 3

Cathodic Protection

Answer 3

• A technique to prevent corrosion by making the metal to be protected act as a cathode in an electrochemical cell. This is achieved by attaching a sacrificial anode or applying external electrical current.
• Example: Used for pipelines and storage tanks, often by attaching a more easily corroded metal (sacrificial anode) or using impressed current systems.

Question 4

Sacrificial Anode

Answer 4

• A more easily corroded metal used to protect a less reactive metal from corrosion.
• It corrodes first and prevents the protected metal from rusting or degrading.
• Examples: Zinc anodes used in galvanization and on ships.