unit 3 corrosion & batteries
TRANSCRIPT
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Sept. /06 MA/chem/RCET
Unit 3
Corrosion
And
Batteries
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Sept. /06 MA/chem/RCET
•Lecture 23
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CORROSION
• Any process of deterioration– consequent loss of a solid metallic
material – through an unwanted chemical or
electrochemical attack by its environment , – started at its surface – is called corrosion.
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metal Metal oxide
Corrosion ,oxidation
Metallurgy ,reductionHigher energy
Lower energy
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Example
Rusting of IRON
Fe3O4 , reddish scale
Green film on surface of Cu
CuCO3 + Cu(OH)2 ,
Basic copper carbonate
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Classification
drywet
other
oxidation
By gases
liquid
Evolution of H2 Absorption of O2
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Dry / chemical corrosion
Direct chemical action of environmental gases such
as oxygen ,halogen , hydrogen sulphide , sulphur di oxide , nitrogen or anhydrous liquid
with metal surface in immediate proximity
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Oxidation corrosion
Anode
2M 2ne- + 2Mn+
(Loss of electron ,oxidation process)
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Cathode
n/2 O2 + 2ne- nO2-
(Gain of electron ,reduction process)
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Over all reaction
• 2M + n/2 O2 2Mn+ + nO2-
Metal ion Oxide ion
Metal oxide
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Oxidation corrosion
M Mn+ + ne-
Reaction at metal – metal oxide interface
Atmosphericoxygen
metal
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Chemical reaction
2M 2Mn+ + 2ne-
(loss of electron)
nO2 + 2ne- 2nO2-
(gain of electron)
2M + nO2 2Mn+ + 2nO2-
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TYPES
1. Stable
2. Unstable
3. Volatile
4. porous
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1 .stable• The oxide film on the surface of
• Al , Pb , Sn , Pt, etc
• stable,
• Tightly adhering
• and
• impervious in nature.
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2. Unstable
metal metal metal
Exposed surfaceO2,air
Unstable metal oxide
Film formed
decomposed
+
O2
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3. Volatile
metal metal metal
Exposed surfaceO2,air
volatile metal oxide
Film formed
decomposed
+
O2
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4. Porous
metal metal
Exposed surfaceO2,air
porous metal oxide
Film formed
decomposed
+O2
Further attack through cracks ,pores
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Corrosion by other gases
• SO2
• CO2
• Cl2
• H2S
• F2
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Liquid metal corrosion
• Dissolution of solid metal
• Internal penetration
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• Lect. 24
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Wet corrosion
• Conducting liquid
• In contact with metal
• Dissimilar metal , Alloys
• Immersed , partially immersed
• In solution
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Chemical reaction
Anodic reaction
M Mn+ + ne- (oxidation loss
of e-s)
dissolves in solution
Forms compound such as oxide
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Cathodic reaction
• 1) Evolution of hydrogen
• 2) Absorption of oxygen
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Evolution of hydrogen
In acidic environment
Example
Fe Fe++ ( ferrous)
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Chemical reaction
AnodeFe Fe2+ + 2e-
(oxidation ,loss of electrons)
Cathode
2H+ + 2e- H2
(reduction, gain of electron)
Over all reaction
Fe + 2H+ Fe2+ + H2
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Evolution of hydrogen
M Mn+ + 2e-
Acidic solution ,electrolyte
Small ,cathodic area
Large anodic area
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Absorption of oxygen
• In neutral environment
• Rusting of iron , in presence of NaCl solution
• Fe in presence of 0xygen forms iron oxide
• Anodic area created on surface (smaller)
• Metal part act as cathode (large)
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Absorption of oxygen
Aqueous neutral solution
rust
Large cathodic area
Small anodic area
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Anodic reaction
• Fe Fe2+ + 2e-
• (oxidation, loss of electron)
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Cathodic reaction
• Fe2+ ions (at anode) and OH- ions (at cathode) diffuse
• Ferrous hydroxide is precipitated .
• Fe2+ + 2OH - ----------> Fe2+ + 2e-
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( i )
If enough oxygen is present , ferrous hydroxide is easily oxidized to ferric hydroxide .
4 Fe(OH)2 + O2 + 2H2O---------> 4Fe(OH )3
yellow rust , ( Fe2O3 . H2O)
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( ii )
If the supply of oxygen is limited,
the corrosion product may be even
black anhydrous magnetite, Fe3O4.
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•Lect. - 25
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GALVANIC (OR BIMETALLIC) CORROSION
• When two dissimilar metals
• (e.g., zinc and copper)
• electrically connected and exposed to an electrolyte,
• the metal higher in electrochemical series undergoes corrosion.
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Galvanic / Bimetallic
Zn Cu
Electronic current
Cathode ,protected
Anode , attacked
electrolyte
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Explanation
• zinc (higher in electrochemical series) forms the anode and is attacked and gets dissolved;
• whereas copper (lower in electrochemical series or more noble) acts as cathode.
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Mechanism
• In acidic solution, the corrosion occurs by the hydrogen evolution process;
• while in neutral or slightly alkaline solution, oxygen absorption occurs.
• The electron-current flow from the anodic metal zinc,
• Zn Zn2+ + 2e- (oxidation)
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Examples
• (i) Steel screws in a brass marine hardware;
• (ii) Lead - antimony solder around copper wire;
• (iii) A steel propeller shaft in bronze bearing;
• (iv) Steel pipe connected to copper plumbing.
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CONCENTRATION CELL CORROSION
• corrosion is due to electrochemical attack on the metal surface,
• exposed to an electrolyte of varying concentrations or of varying aeration.
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Concentration cell corrosion
Water line corrosion
Zn rod
Corroding anode
NaCl solution
More oxygenated part
Less oxygenated part
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• This may be the result of local difference in metal - ion concentrations,
• caused by local temperature differences or inadequate agitation or slow diffusion of metal-ions, produced by corrosion.
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• It has been found experimentally that “poor-oxygenated parts are anodic”
• Consequently, a differential aeration of metal causes a flow of current,
• called the differential current.
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• Zinc will dissolve at the anodic areas,
• and oxygen will take up electrons
• at the cathodic areas to form
• hydroxyl ions.•
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Chemical reaction
anodicZn Zn2+ + 2e-
(Oxidation)
cathodic1/2 O2 + H2O + 2e- 2 OH-
(Reduction)
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• The circuit is completed by migration of ions,
• through the electrolyte,
• and flow of electrons,
• through the metal, from anode to cathode.
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• Corrosion is accelerated under accumulation of dirt sand,
• scale or other, contamination
• The result is localized corrosion,
• due to non - uniform corrosion.
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• Metals exposed to aqueous media corrode under blocks of wood or pieces of glass,
• which screen that portion of metal from oxygen access.
•
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• Lect . -25
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PASSIVITY
• . Passivity is the
• “phenomenon in which a metal or an alloy exhibits a much higher corrosion - resistance than expected from its position in the electrochemical series.”
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Passivity falling order
• Tl --------> Al ------> Cr -------> Be -------
• >Mo -------> Mg ------> Ni ------>
• Co -------> Fe ------> Mn ------->Zn -------
• > Cd -------> Sn ------> Pb ------> Cu
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• The action of more concentrated
• solution of HNO3 on active metals (Fe and Al) produces a thin protective oxide film,
• thereby stifling the anodic reaction and making them passive
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8. UNDERGROUND OR SOIL
The corrosiveness of a soil depends upon :
(i) its acidity,
(ii) degree of aeration,
(iii) electrical conductivity,
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(iv) its moisture and salts content,
(v) presence of bacteria and micro-
organisms, and
(vi) soil texture.
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(a)
• Gravelly or sandy solis are very porous and strongly- aerated.
• If a metal pipe is buried in such a soil, corrosive conditions are similar to those under wet condition,
• and the corrosion rate will be governed by amount of moisture content in the soil.
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(b)
• In water-logged soils,
• the amount of free oxygen available is very small,
• but various bacteria and micro- organisms can grow,
• which may lead to micro-biological corrosion.
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corrosion depends
(i) the pH (or acidity) of the soil,
(ii) the presence of salt, and
(iii) the presence of oxygen, etc.
oxygen facilitates the evolution of hydrogen and, hence, accelerates the rate of attack.
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9. PITTING CORROSION
Pitting corrosion is a localized accelerated attack, resulting in the formation of cavities around which the metal is relatively unattached.
pinholes, pits and cavities in the metal.
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• pitting is,
• usually, the result of the breakdown or cracking of the protective film on a metal at specific points.
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Breakdown of the protective film
caused by :
(i) surface roughness or non-uniform finish,
(ii) scratches or cut edge,
(iii) local straining of metal, due to non-uniform stresses,
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(iv) alternating stresses,
(v) sliding under load,
(vi) impingement attack (caused by the turbulent flow of a solution over a metal surface),
(vii) chemical attack.
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1. Differential amount of oxygen in contact with the metal the small part
(underneath the impurity) become the anodic areas
2 . Surrounding large parts become the cathodic areas.
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• Intense corrosion, therefore,
• start just underneath the impurity.
• Once a small pit is formed,
• the rate of corrosion will be increased.
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INTERGRANULAR CORROSION
• along grain boundaries and only where the material, especially sensitive to corrosive attack exists,
• and corrosive liquid possesses a selective character of attacking only at the grain boundaries,
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• but leaving the grain interiors
• untouched or
• only slightly attacked.
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• WATERLINE CORROSION• When water is stored in a steel tank, it is
generally found that the maximum amount of corrosion takes place along a line just beneath the level of the water meniscus. The area above the waterline (highly-oxygenated) acts as the cathodic and is completely unaffected by corrosion. However, if the water is relatively free from acidity, little corrosion takes place.
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• The problem of waterline corrosion is also that concerns marine engineers. In the case of ships, this kind of corrosion is often accelerated by marine plants attaching themselves to the sides of ships. The use of special antifouling paints restrict this to some extent.
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• It is characteerized by a highly localized attack occurring, when overall corrosion is negligible. For stress corrosion to occur : (i) presence of tensile stress, and (ii) a specific corrosive environment are necessary. The corrosive agents are highly specific and selective such are: (a) caustic alkalis and strong nitrate solution for mild steel; (b) traces of ammonia for brass; (c) acid chloride solution for stainless steel.
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• This type of corrosion is seen in fabricated articated articles of certain alloys (like high-zinc brasses and nickel brasses) due to the presence of stresses caused by heavy working like rolling, drawing or insufficent annealing. However, pure metals are relatively immune to stress corrosion.
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• These become so chemically- active that they are attacked, even by a mild corrosive environment, resulting in the formation of a crack, which grows and propagates in a plant (perpendicular to the operating tensile stress), until failure occurs or it may stop, after progressing a finite distance.
• Some typical examples
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• V(1) Seeason cracking in a term applied to stress corrosion of copper allays, mainly brasses. Pure copper is immune to stress corrosion, but presence of small amounts of alloying element (like P,As,Sb, Zn, Al, Si) result in marked sensitivity. For examples, alpha brass (which when highly stressed) undergo intergranular cracking in an atmosphere, containing traces of ammonia or amines. The attack occurs along the grain boundaries, which become more anodic with respect to the grain themselves (probably
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