Corrosion and Its Prevention CHANGD
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Transcript of Corrosion and Its Prevention CHANGD
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Corrosion and its
prevention
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IntroductionIntroduction
Corrosion is the deterioration of materials by chemical interaction with their Corrosion is the deterioration of materials by chemical interaction with their
environment. The term corrosion is sometimes also applied to theenvironment. The term corrosion is sometimes also applied to the
degradation of plastics, concrete and wood, but generally refers to metals.degradation of plastics, concrete and wood, but generally refers to metals.The most widely used metal is iron (usually as steel) and the followingThe most widely used metal is iron (usually as steel) and the following
discussion is mainly related to its corrosiondiscussion is mainly related to its corrosion..
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Why do metals corrode?Why do metals corrode?
Any spontaneous reaction in the universe is associated with a lowering
in the free energy of the system. All metals except the noble metals
have free energies greater than their compounds. So they tend to
become their compounds through the process of corrosion.
Except noble metal, all metals are unstable to varying degrees in a
terrestrial atmosphere. The most widely used metals, namely, Iron,
aluminium, copper, nickel, silver and alloys of these metals all decay
and lose good mechanical properties.
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Types of corrosionTypes of corrosion
Corrosion may be classified in different waysCorrosion may be classified in different ways
Wet / aqueous CorrosionWet / aqueous Corrosion
Temperature CorrosionTemperature Corrosion
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Wet / aqueous corrosion is the major form of corrosion. Based on the appearance of
the corroded metal, wet corrosion may be classified as
Uniform or General
Galvanic or Two-metal
Crevice
Pitting
Intergranular
Velocity-assisted
Environment-assisted cracking
Type I
Wet / Aqueous corrosion
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UNIFORM CORROSION
Corrosion over the entire exposed surface at a uniform rate. e.g..Atmospheric
corrosion.
Maximum metal loss by this form. Not dangerous, rate can be measured in the laboratory.
GALVA NIC CORROSION
When two dissimilar metals are joined together and exposed, the more active of the two
metals corrode faster and the nobler metal is protected. This excess corrosion is due to the
galvanic current generated at the junction.
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Prevention of galvanic corrosion:
(1) Do not have the area of the more active metal
smaller than the area of the less active metal.
(2) If dissimilar metals are to be used, insulate them.
(3) Use inhibitors in aqueous systems whenever
applicable and eliminate cathodic depolarizers
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Crevice corrosion :
Intensive localized corrosion within crevices &
shielded areas on metal surfaces Small volumes of
stagnant corrosive caused by holes, gaskets, surface
deposits, lap joints
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PITTING
1)A form of extremely localized attack causing holes in the metal
2) Most destructive formAutocatalytic nature
3) Difficult to detect and measure Mechanism
Prevention of pitting corrosion :
(1) Use materials with appropriate alloying elements designed to minimize
pitting susceptibility. e.g. molybdenum in stainless steel.
(2) Provide a uniform surface through proper cleaning, heat treating and surfacefinishing.
(3) Reduce the concentration of aggressive species in the test medium, such as
chlorides, sulfates, etc.
(4) Use inhibitors to minimize the effect of pitting, wherever possible.
(5) Make the surface of the specimen smooth and shiny and do not allow any
impurities to deposit on the surface.
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Intergranular corrosion:
The grain boundaries in metals are more active than the grains because of
segregation of impurities and depletion of protective elements. So preferential
attack along grain boundaries occurs. e.g. weld decay in stainless steels
Method of Prevention
The following are the methods of prevention of austenitic nickel chromium
stainless steels from intergranular corrosion:
(a) Purchase and use stainless steel in the annealed condition in which there is
no harmful precipitate. This only applies when the steel is not to be exposed to
the sensitizing temperature.
(b) Select low carbon grade steel with a maximum of 0.03% C, such as 304 L.
This would prevent the formation of harmful chromium carbide during
fabrication
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Velocity Assisted corrosion :
Fast moving corrosives causea) Erosion-Corrosion,
b) Impingement attack , and
c) Cavitation damage in metals
Cavitation Damage :
Cavitation is a special case of Erosion-corrosion. In high velocity
systems, local pressure reductions create water vapour bubbles which
get attached to the metal surface and burst at increased pressure,
causing metal damage
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EnvironmentAssisted Cracking:When a metal is subjected to a tensile stress and a corrosive medium, it may experience
EnvironmentAssisted Cracking. Three types:
1) Stress Corrosion Cracking
2) Hydrogen Embrittlement3) Liquid Metal Embrittlement
Stress Corrosion Cracking:
Static tensile stress and specific environments produce cracking
Examples:
1) Stainless steels in hot chloride2) Ti alloys in nitrogen tetroxide
3) Brass in ammonia
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Hydrogen Embrittlement:High strength materials stressed in presence of hydrogen crack at reduced stress levels.
(a) Film rupture model
(b) Slip step dissolution modelHydrogen may be dissolved in the metal or present as a gas outside. Only ppm levels of H
needed
liquid metal embrittlement:
Certain metals likeAl and stainless steels undergo brittle failure when stressed in contact
with liquid metals like Hg, Zn, Sn, Pb Cd etc.
Molten metal atoms penetrate the grain boundaries and fracture the metal.Fig. Shows brittle IG fracture inAl alloy by Pb
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Type II
Temperature corrosion:
Generally corrosion rates increase with increases in temperature. This is due to
several interrelated factors:
1. Higher temperatures tend to promote the corrosion reaction kinetics. Therefore
except in cases where oxygen is free to escape, higher temperatures boost the
corrosion rate.
2. Corrosive by products will have a higher diffusion rate at higher temperatures
and thus will be delivered to the corroding surface more efficiently.
(a) High Temperature corrosion
(b)Low temperature corrosion
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High temperature corrosion
High temperature corrosion is a form of corrosion that does notrequire the presence of a liquid electrolyte. Sometimes, this type of
damage is called "dry corrosion" or "scaling".
High temperature metals requires neither moisture nor dissolved
electrolytes (salts, acids) to proceed.
Low temperature corrosion:
Low-temperature corrosion appears in the boiler as well as on other
surfaces where the temperature is under approx. 135°C. It is caused
by condensation of the acidic sulphur and chlorine-containing
gases.
This type of corrosion is temperature-dependent. New plants are
being designed differently in order to avoid low-temperature
corrosion
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Causes of corrosionCauses of corrosionFailures of various kinds and the need for expensive replacements may occur even though the
amount of metal destroyed is quite small.
Some of the major harmful effects of corrosion can be summarized as follows:
1. Reduction of metal thickness leading to loss of mechanical strength and structural failure or
breakdown.
2. Hazards or injuries to people arising from structural failure or breakdown (e.g. bridges,
cars, aircraft).
3. Loss of time in availability of profile-making industrial equipment.
4. Reduced value of goods due to deterioration of appearance.
5. Contamination of fluids in vessels and pipes (e.g. beer goes cloudy when small quantities
of heavy metals are released by corrosion).
6. Perforation of vessels and pipes allowing escape of their contents and possible harm to the
surroundings.
7. Loss of technically important surface properties of a metallic component.
8. Mechanical damage to valves, pumps, etc, or blockage of pipes by solid corrosion products.
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10) Buried gas or water supply pipes can suffer severe corrosion which is not
detected until an actual leakage occurs, by which time considerable damage may be
done.
11) In electronic equipment it is very important that there should be no raised resistance at
low current connections.
12) The lower edge of this aircraft skin panel has suffered corrosion due to leakage and
spillage from a wash basin in the toilet.
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Barrier protection :
Here, a thin barrier is developed between the surface of iron and
atmosphere by one of the following methods:a) Painting of the surface
b) Coating the surface with a thin film of oil or grease
c) Developing a thin layer of some non ±corrosive metal like nickel,
chromium copper etc., by electroplating.
Sacrificial protection:
In this case, the surface of iron is covered with a more electropositive metal like
zinc or aluminum. Since this metal loses electrons more readily than iron, rusting
is prevented. As long as metal is present, iron does not get rusted. This type of
protection is called µsacrificial production¶.
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Cathodic protection (Electrical protection):
This method is especially used for underground iron pipes. Here, the iron
pipe or tank is connected to a more electropositive metal like magnesium or
aluminum. The more electropositive metal acts like anode (supplies electrons) and
iron acts like cathode (receives electrons). Thus, iron is protected by turning it as a
cathode.Hence, the method is called µcathodic protection¶ .
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(b) Alloying the metal
Alloying the metal is to produce a more corrosion resistant alloy, e.g.
stainless steel, in which ordinary steel is alloyed with chromium and nickel.
Stainless steel is protected by an invisibly thin, naturally formed film of chromium
sesquioxide Cr2O3
In general, the corrosion behavior of alloys depends on the interaction of:
1. The alloy of specific chemical composition and metallurgical structure.
2. The film on the alloy surface.
3. The environment, whether it is sufficiently aggressive to break down the
protectiveness of the surface film, thereby initiating localized corrosion.
4. The alloy/environment combination, controlling whether the film self
repairs after breakdown and, if not, the type and rate of corrosion that
propagates after initiation has occurred