1 soil & environments 1 st day
DESCRIPTION
cathodic protectionTRANSCRIPT
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What does it look like?What does it look like?
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COST OF CORROSION
Catastrophic failure
Leakage leading to environmental pollution Corroded rotor leading
to equipment failure
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COST OF CORROSION
Soil collapse due corrosion of a municipal water underground steel pipe
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Case HistoriesCase Histories
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SRB Corrosion MechanismSRB Corrosion MechanismElectrochemical ReactionsElectrochemical Reactions
Step oneStep one-:-: Fe Fe → → FeFe++++ + 2 + 2ee-- (Anodic Reaction) (Anodic Reaction)..
4H4H22O O ↔↔ 2H 2H++ + 2OH + 2OH-- (Water Dissociation) (Water Dissociation)..
2H2H++ + 2e + 2e- - →→ HH2 2 (Cathodic Reaction)(Cathodic Reaction)..
2H+H2 2H 2H+
2e-
2e-
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SRB Corrosion MechanismSRB Corrosion MechanismStep twoStep two-:-:
SOSO44---- + 8H + 8H ↔ ↔ SS2-2- + 4H + 4H22O (Bacterial Consumption)O (Bacterial Consumption)..
COPYRIGHT PETROLITE CORP 1993C
S2-
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SRB Corrosion MechanismSRB Corrosion MechanismStep threeStep three-:-:
FeS (Corrosion Product)FeS (Corrosion Product)..Thus the theoretical amount of ferrous sulfide that may be formed from Thus the theoretical amount of ferrous sulfide that may be formed from
a given amount of sulfide isa given amount of sulfide is::
ppm SOppm SO44---- / 96 (MW SO / 96 (MW SO44
---- ) X 88 (MW FeS) = ppm FeS ) X 88 (MW FeS) = ppm FeS
S2- + Fe++ FeS
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COST OF CORROSION
NACE study in 1998 showed that the cost of corrosion in U.S.A. is $ 276 billion / year
Corrosion cost :
Direct cost
materials selection
corrosion control method(s)
manufacturing
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COST OF CORROSION
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MANAGING CORROSION
To reduce risk of equipment failures, corrosion control is to be dealt with by implementing a “ “ Predictive / Proactive Corrosion Predictive / Proactive Corrosion ManagementManagement ProgramProgram “ “ in both :
Design phase
Running/ operative phase
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DESIGN PHASEDESIGN PHASE RUNNING PHASERUNNING PHASE
Materials Selection& Corrosion Control Dept.
Operation Dept.
Inspection Dept.
Corrosion Monitoring
Process flowStream analyses
Service conditions
Past experience, case studies
Codes, standards, specifications, textbooks,
handbooks, vendors recommendations
Predictive Design
Predictive mode Predictive Maintenance
-Effective corrosion control-Extended service life
Reduced CostHigh Profitability
Overall Predictive Management Program
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MANAGING CORROSION
Corrective: unplanned. Most costly
Preventive: planned on a fixed time scale
PredictivePredictive (Proactive): on a (Proactive): on a sliding time scale. Least sliding time scale. Least costlycostly
Relative Cost Of Maintenance
0.25
0.50
0.75
1.00
Corrective Preventive Predictive
Types of Maintenance
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Consequences of Management on Operation & Production
MANAGING CORROSION
Proper ManagementMismanagement
1Pro-activeReactive
2Farsighted - long term planningNo vision- “out of sight, out of mind” attitude
3“Early warning” of corrosion problems
Sudden, unexpected costly failure , i.e. unplanned shutdown
4Increased production capacityDecreased production capacity
5High quality productsLow quality products due to contamination
6Responsible environmental and safety records
Environmental and safety hazards
7“Pay a little now”“Pay a lot later”
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Causes of Corrosion Failures
based leading chemical company investigation outcome
Causes %Freq
APoor design/ wrong material/ bad operation
36
BWrong specification16
CBad inspection10
DHuman error12
EPoor planning14
FOthers4
GUnforeseen8
AA
EE
CC
DD
FF
BB
GG
MANAGING CORROSION
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92% of corrosion failures are PreventablePreventable if the Predictive Corrosion Management Program is strictly implemented during Design and Running phases
Only 8% of unforeseen causes to be dealt with
Results: significant reduction in maintenance Results: significant reduction in maintenance activities and lower cost activities and lower cost
MANAGING CORROSION
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metal Pipemetal Pipe((Gº)Gº) EnvironmentEnvironment
Metal Corrosion Metal Corrosion productproduct
THEORY OF CORROSION
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Engineering MaterialsEngineering Materials
MetallicMetallic
FerrousFerrous Non-FerrousNon-Ferrous
Non- MetallicNon- Metallic
PVCPolyethylene
PolypropyleneTeflon
GRE / GRPCeramics
Copper AlloysNickel Alloys
Aluminum
Cast IronsCarbon Steels
Stainless SteelsLow alloy steel
THEORY OF CORROSION
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CORROSION THEORYCORROSION THEORY
THEORY OF CORROSION
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THEORY of corrosionTHEORY of corrosion
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Chemical PropertiesMetals-
-Usually have 1-3 electrons in their outer shell .-Lose their valence electrons easily .
-Form oxides that are basic .-Are good reducing agents .
-Have lower electro negativities
Nonmetals
-Usually have 4-8 electrons in their outer shell .
-Gain or share valence electrons easily .
-Form oxides that are acidic .
-Are good oxidizing agents .
-Have higher electro negativities
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Non-metals are the elements in groups 14-16 of the periodic table. Non-metals are not able to conduct electricity or heat very well. As opposed to metals, non-metallic elements are very brittle, and cannot be rolled into wires or pounded into sheets. The non-metals exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon). The non-metals have no metallic luster, and do not reflect light. They have
oxidation numbers of ±4, -3, and -2 .The Non-Metal elements are :
HydrogenCarbonNitrogenOxygenPhosphorusSulfurSelenium
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Metals are solids at room temperature with the exception of mercury
and gallium, which are liquids at room temperature.
HardnessAll metals are hard except sodium and potassium, which are soft and can be cut with a knife.
ConductionMetals are good conductors because they have free electrons. Silver and copper are the two best conductors of heat and electricity. Lead is the poorest conductor of heat. Bismuth, mercury and iron are also poor conductors
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Non-Metallic Vessels e.g. Fiber glass
THEORY OF CORROSION
Not concern
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Not concern
Non-Metallic Pipes
PVC pipingAbove-ground GRP piping
Under-ground GRP pipeline
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PVC Piping Connections
1- Heating the sedges 2- Pressing the sedges 3- Fusion Weldment
4- Shaving 3- Fusion Completed
Not concern
Soil & environments
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metal Pipemetal Pipe((Gº)Gº) EnvironmentEnvironment
Metal Corrosion Metal Corrosion productproduct
THEORY OF CORROSION
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Iron Oxide to Steel to Iron Oxide CycleIron Oxide to Steel to Iron Oxide Cycle
Iron OxideIron Oxide
EnergyEnergy(Blast Furnace)(Blast Furnace)
Steel PipeSteel Pipe((Gº)Gº) EarthEarth Iron OxideIron Oxide
BessemerBessemer Pipe MillPipe Mill
THEORY OF CORROSION
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The extracted free metal has a high energy content. i.e. active stateactive state
Blast furnace of reducing iron
ore to iron
Electrolytic reduction of Al oxide to Al
THEORY OF CORROSION
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O/S Separators
FWKO
Biocide Squeeze
Subsea Intrafield P/Ls
•Pigging,Biocide and C.I.
•Some pigging
•Some C.I. injection.
•C.P.
•Manual Cleaning, or P.D.
•C.P. + Coating
Trunk Lines
•Pigging
•Biocide
•Pigging, C.I., Biocide(M-8, M-36)
•C.I., PD (M-1, M-55)
•C.P.
•Manual Cleaning
•Sand Jet
•C.P. + Coating
•Biocide, C.I., P.D.
42”/30”
•Rotation
•Manual Cleaning
GOS CORROSION MITIGATION STATUS
HEMIS
•Fiber Glass Lining
•Chemical Cleaning
36” Suction Header
Biocide, C.I., P.D., Rotation & Replacement.
Mothballing equipment
DESALTERS•C.P.+ Coating
Deposits
ITALIC BOLD: PLANNEDROMAN : COMPLETED Draft : M.H.Eid
Chem. & Corr. Dept.R321\C:\Data\General\CS.ppt
H.EX
2nd Stage
OILTKs
•Fiber Glass Lining
1 st Stage
PROBLEMAREA
PROBLEM AREA
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Soil and environments
Take cure
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Soil and environments Characteristics
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Soil & environments
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Soil and environments
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Piles
Subsea Pipelines
Jackets
Soil and environments
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Sacrificial Anode Cathodic Protection for External Side
of Tank Bottom
Soil and environments
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Sacrificial anodes for vessel internals
Sacrificial Anode
Mist Eliminator
Soil and environments
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Corrosive Formation Water
Crude Oil
Vapor
Air in as Tank Breathes
Sever Corrosion Due to Condensed Aerated Moisture
Protective Coatings
Coatings + CP Sacrificial Anodes
Soil and environments
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metal Pipemetal Pipe((Gº)Gº) EnvironmentEnvironment
Metal Corrosion Metal Corrosion productproduct
THEORY OF CORROSION
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Iron oxidesIron oxides
+
Mining & Extraction
SteelSteel
+
Corrosion
Iron oxidesIron oxides
Oxides, Ore thermodynamically stable
Mining & Extraction
Equipment fabrication, thermodynamically unstable
Corrosion
Corrosion Thermodynamic Cycle
Why Metals Corrode?
THEORY OF CORROSION
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And the
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What is corrosion?
Reaction of a metal with its environment (degradation)** Aqueous corrosion (with water)
** Atmospheric corrosion (with air+water+salts)** High temperature corrosion (with oxygen or other gases)
We will mainly concentrate on Aqueous corrosion
We will focus on metals especially carbon steel and CRAs used on the underground and immersed on the sea water
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* *Corrosion is the return of metals to their Corrosion is the return of metals to their natural states, i.e., the ores from which natural states, i.e., the ores from which they are obtainedthey are obtained..
** Corrosion involves oxidation of the metalCorrosion involves oxidation of the metal
** Corroded metal loses its structural Corroded metal loses its structural integrity and attractivenessintegrity and attractiveness..
** Metals corrode because they oxidize Metals corrode because they oxidize easilyeasily..
What is corrosion?
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Production and Production and degradation of steeldegradation of steel
Plates, pipes,profiles, etc.
Energ
y
Man
ufac
turing
Water /humidity
Oxygen
Raw materialIron ore Rust
Reaction between the material and the surrounding environment takes place
The presence of water / humidity and Oxygen is a pre-requisite for corrosion of steel
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Corrosion is a reaction betweenCorrosion is a reaction between
MaterialMaterial
andand
Surrounding environmentSurrounding environment
under formation of corrosion productsunder formation of corrosion products
What is corrosion?
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Some metals form a protective oxide coating, Some metals form a protective oxide coating, preventing the complete corrosion of the metal.preventing the complete corrosion of the metal.
* * Aluminum is the best example, forming AlAluminum is the best example, forming Al22OO33, , which adheres to, and protects the aluminum.which adheres to, and protects the aluminum.
* Copper forms an external layer of copper * Copper forms an external layer of copper carbonate, known as patina.carbonate, known as patina.
* Silver forms silver tarnish which is silver * Silver forms silver tarnish which is silver sulfide.sulfide.
* Gold does not corrode in air.* Gold does not corrode in air.
What is corrosion products?
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Rusting of steelRusting of steel• corrosion product (rust) is solid but not corrosion product (rust) is solid but not
protectiveprotective Reaction of aluminium with waterReaction of aluminium with water
• corrosion product is insoluble in water, so corrosion product is insoluble in water, so may be protectivemay be protective
Burning of magnesium in airBurning of magnesium in air• high temperature oxidationhigh temperature oxidation
What is corrosion products?
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Corrosion of Iron or Steel by SRB BacteriaCorrosion of Iron or Steel by SRB Bacteria
FeSFeS
224 H O4 H O
FeSFeS
S S ++ 8 H8 H ++ 44SOSO
DesulfovibrioDesulfovibrio
8 H8 H 8 e8 e++ 8 H8 H
SOLUTIONSOLUTION
++++3Fe(OH) 3Fe(OH)
22
4Fe 4Fe 4Fe 4Fe --
--
Corrosion ProductCorrosion Product
Corrosion ProductCorrosion Product
8 OH8 OH ++--
8 H O8 H O22
8 H8 H++SOSO 44 S S ++ 224 H O4 H O
8 H8 H8 e8 e ++8 H8 H
++++
++--
DesulfovibrioDesulfovibrio
++ --8 H O8 H O22
++8 OH8 OH
2-2- 2-2-2-2-2-2-
4Fe 4Fe CathodeCathodeAnodeAnode
4Fe 4Fe
8 e8 e 8 e8 e --
4Fe 4Fe CathodeCathodeCathodeCathode
Cathodic DepolarisationCathodic DepolarisationCathodic DepolarisationCathodic Depolarisation
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Copper, gold, silver, and platinum Copper, gold, silver, and platinum are relatively difficult to oxidize, are relatively difficult to oxidize,
hence the term noble metalshence the term noble metals..
Noble MetalsNoble Metals
What is corrosion products?
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What is corrosion?
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In a chemical reaction :
Reactants Products
∆G = Gprod – Greact
In all corrosion reactions
Gprod < Greact.
Therefore,
∆G is –ve
Hence, the corrosion reaction is :
spontaneous
irreversibleirreversible
Thermodynamics of Corrosion
Reactant
Product
Reactants Products = Corrosion?
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Active free metals tend to react easily to produce compounds, such as salts and oxides.
Metals in the compounded forms have less energy content, i.e. stable state.
Corrosion is governed by the Law of Conservation of Energy :
Energy Gained = Energy LostEnergy Gained = Energy Lost
THEORY OF CORROSION
F
G E
o
cell n
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Corrosion Cell potential is Related to the Change in Gibb’s Free Corrosion Cell potential is Related to the Change in Gibb’s Free EnergyEnergy
where:where:EEcellcell == corrosion cell potential (volts or joules/coulomb)corrosion cell potential (volts or joules/coulomb)
nn == number of charges transferred in the oxidation reaction number of charges transferred in the oxidation reaction
FF == Faraday’s constant – 96,500 coulombs of chargeFaraday’s constant – 96,500 coulombs of charge
GGoo == change in Gibb’s free energy (joules)change in Gibb’s free energy (joules)
F
G E
o
cell n
THEORY OF CORROSION
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Behavior of metals immersed on environments (electrolytes)
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Metal/Aqueous Solution InterfaceMetal/Aqueous Solution Interface
OH_
OH_
OH_
H+
IronIon
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++Electrons
O
O- -H+ H+
O- -H+ H+
O- -H+ H+
O- -H+ H+
- -H+H+
Fe++
IronIon
H+
H+
The Electrode Potential Across a Metal Electrolyte InterfaceThe Electrode Potential Across a Metal Electrolyte Interface
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Corrosion Forming Ferrous HydroxideCorrosion Forming Ferrous Hydroxide
OH_
OH_
OH_
H+
H+
IronIon
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++Electrons
O
O- -H+ H+
O- -H+ H+
O- -H+ H+
O- -H+ H+
- -H+H+
Fe++
H+
H+OH_
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Iron Corrosion CellIron Corrosion Cell
OH_
OH_
OH_H+
H+
H+
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++Fe Fe
O- -H+ H+
O- -H+ H+
O- -H+ H+O- -
H+ H+
O- -H+ H+
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OH_
OH_
OH_H+
H+
H+
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++Fe Fe
O- -H+ H+
O- -H+ H+
O- -H+ H+
O- -H+ H+
O- -H+ H+
Fe(OH)2
H+ H+
H0
H0
AnodeAnode
CathodeCathode
Direction of Conventional CurrentDirection of Conventional Current(positive charge flow)(positive charge flow)
Icorr
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Corrosion Cell ComponentsCorrosion Cell Components
An An anodeanode (where the oxidation reaction occurs) (where the oxidation reaction occurs)
A A cathode cathode (where the reduction reaction occurs)(where the reduction reaction occurs)
An An electronic pathelectronic path that allows electrons to flow from the that allows electrons to flow from the anode to the cathode (inside the metal)anode to the cathode (inside the metal)
An An electrolytic pathelectrolytic path that allows ions to flow between the that allows ions to flow between the anode and cathode (in the electrolyte)anode and cathode (in the electrolyte)
A corrosion cell has the following 4 components:A corrosion cell has the following 4 components:
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Direction of Conventional CurrentDirection of Conventional Current(+ve charges) in a Corrosion Cell(+ve charges) in a Corrosion Cell
OXIDATI
ON
Anode
REDUCTI
ON
C athode
E lectro lyte
Icorr
Icorr
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H+Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++
Fe++
Fe
Fe
Fe
Fe
Fe
OH+ H+
OH
OH+ H+
OH
H+
H+
OH+ H+
OH
OH
EE c,occ,oc
AA
cellcellEE
EE a,oca,oc
Fe
Fe
Fe
Fe
Fe
Fe Fe++
Open Circuit Open Circuit Corrosion CellCorrosion Cell
Cathode
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H+
H+
H+
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe++
AnodeAnode
Fe++
Cathode
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
Fe
FeCathodeCathode
OH+ H+
OH
OH+ H+
OH
H+
H+
OH+ H+
OH
OH
EEc,ccc,cc
AAcorrcorrII +
e
e
Closed Circuit Closed Circuit Corrosion CellCorrosion Cell
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Evans Diagram for a Corrosion Cell Under Cathodic ControlEvans Diagram for a Corrosion Cell Under Cathodic Control
Ea ,cc
E
0 I1 I2 I3 Icorr
C orrosion C urrent
Ec ,cc
Ea ,oc
Ec ,oc
Ep,c
Ep,a
Ecell
E - Polarizationcell
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E
Icorr
Corrosion Current
(a) Anodic Control
E
Icorr
Corrosion Current
(b) Mixed Control
Ea,cc
Ec,cc
Ec,oc
Ea,oc
Ea,cc
Ec,cc
Ec,oc
Ea,oc
Evans Diagram for Corrosion Cells under Anodic and Mixed Evans Diagram for Corrosion Cells under Anodic and Mixed ControlControl
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Fe2+
Fe2+
Fe2+
Atmospheric O2
O2
O2
OH-OH-OH-
e-e-e- e-
Anodic Area Metal Dissolution
Fe(OH)2Cathodic Area
Dissolved Oxygen Reduction
The Corrosion Cell : in Aerated Natural Water
The Corrosion Cell : in Aerated Natural Water
THEORY OF CORROSION
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Corrosion Process
A. Anodic Reaction (metal dissolution)
Fe Fe 2+ + 2e-
B. Cathodic Reaction
1. Oxygen reduction reaction
O2 + 2H2O + 4e- 4 OH- Predominates in aerated
Near-Neutral solutions pH > 5
2. Hydrogen Evolution Reaction
THEORY OF CORROSION
Anodic Area
Cathodic Area
Fe(OH)2
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Very important
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Corrosion Process
Due to the electrochemical nature of corrosion, there shall be electron transfer
Electron transfer requires presence of anode sitesanode sites and cathode sitescathode sites on the metal surface
Due to potential difference ( ∆V ) between anodesanodes and cathodescathodes electrons migrate from anodesanodes to cathodes
Electrons liberated at anodesanodes should be consumed at cathodescathodes
THEORY OF CORROSION
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THEORY OF CORROSIONTHEORY OF CORROSION
Oxidation Is Loss of electrons Reduction Is Gain of electrons
OILRIGOILRIG
Corrosion Process
@@ Anode SitesAnode Sites :
Surface defects
More -ve potentials
Metal atoms have high energy, i.e. unstable & active
Thus, metal atoms ionize by losing their electrons, i.e.
oxidation reactionoxidation reaction : M0 Mn+ + ne-
As a result, metal loss occurs, i.e. metal dissolutionmetal dissolution
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Corrosion Process
@ Cathode Sites@ Cathode Sites :
Intact ( un-defected ) surface areas
More +ve potentials
Metal atoms have low energy, i.e. stable & un-active
Receive electrons to be consumed, i.e. reduction reactionreduction reaction
As a result, no metal loss occurs, i.e. no corrosion
THEORY OF CORROSION
Oxidation Is Loss of electrons Reduction Is Gain of electrons
OILRIGOILRIG
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THEORY OF CORROSION
The corrosion process involves two reactions:
A. Anodic Reaction : occurs @ anode sites
Metal Dissolution : M 0surface M n+
solution + ne-
Oxidation Reaction : involves loss of electrons
B. Cathodic Reaction : occurs @ cathode sites
Reduction Reaction : involve gain of electrons
Oxygen reduction : gain of electrons by dissolved O2
Hydrogen evolution: gain of electrons by H+ ions
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Faraday’s LawFaraday’s Law
corrt I F
M W t
n
where:
Wt = total weight loss at anode or weight of material produced at the cathode (g)
n = number of charges transferred in the oxidation or reduction reaction
Icorr = the corrosion current (A)
F = Faraday’s constant of approximately 96,500 coulombs per equivalent weight of material (where equivalent weight = M )
M = the atomic weight of the metal which is corroding or the substance being produced at the cathode (g)t = the total time in which the corrosion cell has operated (s)
n
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Consumption Rate is Proportional to Consumption Rate is Proportional to Corrosion CurrentCorrosion Current
corrmcorrt IK I
F
M
W
nt
corrt I F
M W t
n multiplied by t
1 then the expression becomes:
Km= constant for each metal
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Theoretical Consumption Rates of Various Theoretical Consumption Rates of Various Metals & Substances on an Ampere-Yr. BasisMetals & Substances on an Ampere-Yr. Basis
Reduced Species
Oxidized Species
Molecular Weight, M
(g)
Electrons Transferred
(n)
Equivalent Weight, M/n
(g)
Theoretical Consumption Rate
(Kg/A-y) Al Al+++ 26.98 3 8.99 2.94 Cd Cd++ 112.4 2 56.2 18.4 Be Be++ 9.01 2 4.51 1.47 Ca Ca++ 40.08 2 20.04 6.55 Cr Cr+++ 52.00 3 17.3 5.65 Cu Cu++ 63.54 2 31.77 10.38 H2 H+ 2.00 2 1.00 0.33 Fe Fe++ 55.85 2 27.93 9.13 Pb Pb++ 207.19 2 103.6 33.9 Mg Mg++ 24.31 2 12.16 3.97 Ni Ni++ 58.71 2 29.36 9.59
OH- O2 32.00 4 8.00 2.61 Zn Zn++ 65.37 2 32.69 10.7
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ExampleExampleUsing the following equation to calculate the weight consumed Using the following equation to calculate the weight consumed
by 1 ampere of stray DC current discharging from an iron by 1 ampere of stray DC current discharging from an iron structure in 1 yearstructure in 1 year..
corrt I nF
M W t
where:where:t = 1 year = 60 s/min x 60 min/h x 8,760 h/y = 31.5 x 106 sM = 55.85 g (from Table)n = 2F = 96,500 coulombs
then:then:
kg 9.12 g9115 coulombs 96,500 2
A1 s10 31.5 g55.85 W
6
t
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substituting the above equation into the Faraday equation substituting the above equation into the Faraday equation yields the following relationshipyields the following relationship::
t
Q I
where: Q ........ charge in coulombs t .......... time in seconds
corrnQ
F
M Wt
Other Corrosion-Related RelationshipsOther Corrosion-Related Relationships
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Similarly, if the Faraday equation is multiplied by the termSimilarly, if the Faraday equation is multiplied by the term::
A = surface area of the anode or cathode t = time in seconds
where:where:
Then the following relationship results:Then the following relationship results:
t A
1
A
I
F
M
A
W corrt nt
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NACE International Ranking for Steel Corrosion
Corrosion Rate (mpy)
Level of corrosion
<1Low
1-5Moderate
5-10Severe
>10Intense
NACE= National Association for Corrosion Engineers
THEORY OF CORROSION
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Energy Metal/alloy Potential Corrosion (volts) *
Least energy required
for refining
High energy required
for refining
GoldSilverTitaniumStainless steel (316, active)Ni-Al- BronzeCopperCarbon steelAluminium (pure)Zinc (anode alloy)Aluminium (anode alloy)Magnesium (anode alloy
+0,500- 0,205- 0,225- 0,235- 0,380- 0,435- 0,600- 0,800- 1,080- 1,140- 1,550
Least corrosive
Very corrosive
* Potential in seawater measured versus a Copper / Copper Sulphate reference electrode
Galvanic Series in Sea WaterGalvanic Series in Sea WaterTHEORY OF CORROSION
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THEORY OF CORROSION
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Before answering
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Thank You and Good Luck
BREAK TIMES