corrosion
Table of content
Introduction.............................................................................pg. 1
Definition of corrosion…………………………….....................pg.2
Chemical change during corrosion…………………………….pg.3
Corrosion in Metals………………………………………………pg.4
Preventing corrosion……………………………………………..pg.4
ABSTRACT
Introduction
Corrosion has been a fundamental problem from the time humans started using metals. Many metallic substances such as steels, cars and ships become subjects to corrosion all the time. Corrosion is a process that happens over a period of time when required properties within a material begin to deteriorate, after a long time exposure to oxygen within its surroundings. Governments spend millions of dollars in budget every year in restoring rusted materials caused by corrosion. Corrosion can take place in many forms as a result of oxidation and rust. Almost any material that comes in contact with oxygen will become at risk of corrosion.
Corrosion in metals
Metal atoms give up electrons and became positively charged ions when exposed to an environment containing water (H2O or air (O2) molecules. Sea water for instance enhances growth of the fatigue crack. The corrosive process of the metal dissolving as ions generates some electrons that are consumed by a secondary process. These two processes have to balance their charges. Salt water or sodium increases the rate of rusting tremendously in solution. Salt is the reason is that many protective paints and sealants don’t defend against rust. Salt water penetrates the protective layers to corrode the metal.
Corrosion in iron
Rust on iron is produced in sea water when iron (Fe) comes in contact with oxygen. The reason for this is because when water interacts with iron it conducts a small amount of current that flows through the iron. Salt increases the amount of ions in water allowing it to become a better conductor. The full chemical equation for this process theoretically is:
Fe + O2
Introduction.............................................................................pg. 1
Definition of corrosion…………………………….....................pg.2
Chemical change during corrosion…………………………….pg.3
Corrosion in Metals………………………………………………pg.4
Preventing corrosion……………………………………………..pg.4
ABSTRACT
Introduction
Corrosion has been a fundamental problem from the time humans started using metals. Many metallic substances such as steels, cars and ships become subjects to corrosion all the time. Corrosion is a process that happens over a period of time when required properties within a material begin to deteriorate, after a long time exposure to oxygen within its surroundings. Governments spend millions of dollars in budget every year in restoring rusted materials caused by corrosion. Corrosion can take place in many forms as a result of oxidation and rust. Almost any material that comes in contact with oxygen will become at risk of corrosion.
Corrosion in metals
Metal atoms give up electrons and became positively charged ions when exposed to an environment containing water (H2O or air (O2) molecules. Sea water for instance enhances growth of the fatigue crack. The corrosive process of the metal dissolving as ions generates some electrons that are consumed by a secondary process. These two processes have to balance their charges. Salt water or sodium increases the rate of rusting tremendously in solution. Salt is the reason is that many protective paints and sealants don’t defend against rust. Salt water penetrates the protective layers to corrode the metal.
Corrosion in iron
Rust on iron is produced in sea water when iron (Fe) comes in contact with oxygen. The reason for this is because when water interacts with iron it conducts a small amount of current that flows through the iron. Salt increases the amount of ions in water allowing it to become a better conductor. The full chemical equation for this process theoretically is:
Fe + O2