corrosion and corrosion control - c.ymcdn.com · pdf file4/25/2012 4 corrosion is an economic...
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Corrosionand
Corrosion Control
Examples of Corrosion
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Examples of Corrosion
Examples of Corrosion
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Examples of Corrosion
What is Corrosion……….
•Corrosion – The
deterioration of a material,
usually a metal, due to a
reaction in its environment.
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Corrosion is an Economic Issue
e.g. What is the Cost of Corrosion?
Cost of Corrosion
NACE International (National Association of Corrosion Engineers) -- 1972 Estimate?
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Cost of Corrosion
NACE -- 1972Est. @ $10 Billion
Cost of Corrosion
Battelle Columbus -- 1976 Estimate?
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Cost of Corrosion
NACE -- 1972 -- Est. @ $10 Billion
Battelle Columbus -- 1976Est. @ $70 Billion
Cost of Corrosion
U.S. Dept. of Commerce -- 1982 Estimate?
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Cost of Corrosion
NACE -- 1972 -- Est. @ $10 BillionBattelle Columbus -- 1976 -- $70 Billion
U.S. Dept. of Commerce --1982
Est. @ $123.6 Billion
Cost of Corrosion
NACE International (National Association of Corrosion Engineers) -- 1987 Estimate?
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Cost of Corrosion
NACE -- 1987Est. @ $250 Billion
Cost of Corrosion
NACE -- 1972 -- Est. @ $10 BillionBattelle Columbus -- 1976 -- $70 Billion
U.S. Dept. of Commerce - 1982 - $123.6 B
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Cost of Corrosion
What does this tell us
about
the years to come?
Cost of Corrosion - US Annually
0
100
200
300
400
500
600
US Dollars
($Billions)
$10B$70B
$124B
$250B
$500B
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Cost of Corrosion - US annually
�5% of the Gross National Product (GNP)
5%
Cost of Corrosion - US annually
�More than any other disaster presently
occurring in US each year– > Fires– > Floods– > Theft– > Auto Accidents– > Failure of the S&L's
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Cost of Corrosion - US Annually in 1993
�US Population = 250 million
Cost of Corrosion - US Annually in 1993
�US Population = 250 million�Corrosion Cost = $500 billion
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Cost of Corrosion - US Annually in 1993
�US Population = 250 million�Corrosion Cost = $500 billion�Cost per person per year = $2000
Cost of Corrosion - US Annually in 1993
�US Population = 250 million�Corrosion Cost = $500 billion�Cost per person per year = $2000�For a family of four, the family must generate at
least $8000 each year just to pay for the cost of corrosion
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Basic CorrosionPrinciples
Ver. 3.0
Naturally OccurringCorrosion Process
� Metals Corrode in an attempt to achieve a Balance of Energy
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METALS HAVE DIFFERENT ENERGY LEVELS
NOBLE OR PASSIVE (+)
ACTIVE (-)
THE ENERGY HILL
Relative Energy Levels of Various Refined Metals
GOLD
COPPER
STEEL IN CONCRETE WITHOUT Cl
ZINC
MAGNESIUM
ALUMINUM
CARBONSILVER
PLATINUM
STEELSTEEL IN CONCRETE WITH Cl
-
-
NOBLE OR PASSIVE (+)
ACTIVE (-)
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Corrosion of Iron
ELECTROLYTE
METALLICPATH
COPPERCATHODE
IRONANODE
OH-
Fe++
H+ H
Conventional Current Flow
+-
� Metals Corrode in an attempt to achieve a Balance of Energy
Galvanic Corrosion Process
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� Metals Corrode in an attempt to achieve a Balance of Energy
� Anode - Corroding Metal Surface
Galvanic Corrosion Process
� Metals Corrode in an attempt to achieve a Balance of Energy
� Anode - Corroding Metal Surface� Cathode - Non-Corroding Metal Surface
Galvanic Corrosion Process
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� Metals Corrode in an attempt to achieve a Balance of Energy
� Anode - Corroding Metal Surface� Cathode - Non-Corroding Metal Surface� Metal Connection - Path for electrons transfer
Galvanic Corrosion Process
� Metals Corrode in an attempt to achieve a Balance of Energy
� Anode - Corroding Metal Surface� Cathode - Non-Corroding Metal Surface� Metal Connection - Path for electron energy
transfer� Electrolyte Connection - Path for ions transfer
Galvanic Corrosion Process
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FOUR ITEMS REQUIRED FOR CORROSION
ANODE
CATHODE
ELECTROLYTE
METAL CONDUCTOR
Eliminate any one (1) of these elementsand corrosion is stopped!
SOME POSSIBLEANODIC REACTIONS
4 OH O + H O + 4e 22
--
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224 OH O + H O + 4e --
Al Al + 3e+ + + -
SOME POSSIBLEANODIC REACTIONS
Zn Zn + 2e++ -
SOME POSSIBLEANODIC REACTIONS
4 OH O + H O + 4e 22
--
Al Al + 3e+ + + -
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22
Zn Zn + 2e++ -
4 OH O + H O + 4e --
Al Al + 3e+ + + -
Fe Fe + 2e+ -2
SOME POSSIBLEANODIC REACTIONS
SOME POSSIBLECATHODIC REACTIONS
2H + 2e H+ -
2
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SOME POSSIBLE CATHODIC REACTIONS
CI + 2 e 2 CI 2
--
2H + 2e H+ -
2
SOME POSSIBLECATHODIC REACTIONS
2H + 2e H+ -
2
CI + 2 e 2 CI 2
--
O + H O + 4e 4 OH22
--
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H + 1e H+ -
SOME POSSIBLECATHODIC REACTIONS
2H + 2e H+ -
2
CI + 2 e 2 CI 2
--
O + H O + 4e 4 OH22
--
Electro-Chemical Corrosion Cell
ANODE
CURRENT FLOW
CATHODE
STEEL PIPE WALL
ELECTROLYTE
POSITIVE
HHHHHHH
Fe(OH)3
Fe(OH)2
H+ H+ H+
OH-
OH-
OH-
H+
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DISSIMILAR SURFACE CORROSION
ANODIC AREA (corrodes)
CATHODIC AREA (protected)
METAL STRUCTURE ELECTROLYTE
e-
H+
OH-
H + e H+
Fe + 2OH Fe(OH)++
2
-
� CAUSED BY VARIATIONS IN SOIL CHEMISTRY AND PHYSIOLOGY
DISSIMILAR ELECTROLYTE CORROSION
PIPE
HI pH HI pH
HighResistivity
Low Resistivity
LOW pH
HighResistivity
PIPE
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� OCCURS WHEN THE METAL STRUCTURE IS IN CONTACT WITH SOILS HAVING DIFFERENT OXYGEN LEVELS
OXYGEN CONCENTRATION CORROSION
� OCCURS WHEN THE METAL STRUCTURE IS IN CONTACT WITH SOILS HAVING DIFFERENT OXYGEN LEVELS
� THE AREA WITH HIGH OXYGEN CONTENT BECOMES A CATHODE
OXYGEN CONCENTRATION CORROSION
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� OCCURS WHEN THE METAL STRUCTURE IS IN CONTACT WITH SOILS HAVING DIFFERENT OXYGEN LEVELS
� THE AREA WITH HIGH OXYGEN CONTENT BECOMES A CATHODE
� THE AREA WITH LOW OXYGEN CONTENT BECOMES AN ANODE AND CORRODES
OXYGEN CONCENTRATION CORROSION
Oxygen Concentration Corrosion
OXYGEN STARVED COMPACTED CLAY SOIL
PAVEMENT
Corrosion Current caused by difference in Oxygen Concentrations
CORROSION
PIPE
Oxygen RichSand Backfill
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� STONE UP AGAINST PIPE SURFACE WITHIN SAND BACKFILL
OXYGEN CONCENTRATION CORROSION EXAMPLES
� STONE UP AGAINST PIPE SURFACE WITHIN SAND BACKFILL
� CLAY LUMP ON PIPE SURFACE WITH OXYGEN RICH BACKFILL
OXYGEN CONCENTRATION CORROSION EXAMPLES
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� STONE UP AGAINST PIPE SURFACE WITHIN SAND BACKFILL
� CLAY LUMP ON PIPE SURFACE WITH OXYGEN RICH BACKFILL
� DEEPEST POINT IN CREVICE
OXYGEN CONCENTRATION CORROSION EXAMPLES
� STONE UP AGAINST PIPE SURFACE WITHIN SAND BACKFILL
� CLAY LUMP ON PIPE SURFACE WITH OXYGEN RICH BACKFILL
� DEEPEST POINT IN CREVICE– LAPPED PLATES– THREADED COUPLINGS– BOTTOM OF PITS– UNDER BOLT HEADS AND WASHERS
OXYGEN CONCENTRATION CORROSION EXAMPLES
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1. Stray Current
2. Naturally Occurring
THERE ARE ONLY TWO (2) BASIC FORMS OF ELECTROLITIC CORROSION
STRAY CURRENT
�MAN MADE CORROSION
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� MAN MADE CORROSION� AN EXTERNAL SOURCE OF DIRECT CURRENT
(DC) TRAVERSING THROUGH THE SOIL (ELECTROLYTE) STRAYS ONTO THE STRUCTURE
STRAY CURRENT
� MAN MADE CORROSION� AN EXTERNAL SOURCE OF DIRECT CURRENT
(DC) TRAVERSING THROUGH THE SOIL (ELECTROLYTE) STRAYS ONTO THE STRUCTURE
� CATHODIC REACTIONS OCCUR (protection) WHERE THE CURRENT IS PICKED UP BY THE STRUCTURE
STRAY CURRENT
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� MAN MADE CORROSION� AN EXTERNAL SOURCE OF DIRECT CURRENT
(DC) TRAVERSING THROUGH THE SOIL (ELECTROLYTE) STRAYS ONTO THE STRUCTURE
� CATHODIC REACTIONS OCCUR (protection) WHERE THE CURRENT IS PICKED UP BY THE STRUCTURE
� ANODIC REACTIONS OCCUR (corrosion) WHERE THE CURRENT LEAVES THE STRUCTURE
STRAY CURRENT
+
-DC
GENERATOR
TRANSIT POWER LINE
ANODIC AREA
CATHODIC AREA
RAIL
EARTH
Steel Pipe
CORROSION PASSIVATION
STRAY CURRENT
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FARADAY'S LAW: Wt = KIT
WHERE:Wt = Weight Lost
I = Current (amps)T = Time (yrs.)K = Electrochemical
Equivalent #/A/yr.
Fe = 20 #/A/YrCu = 45 #/A/YrPb = 75 #/A/Yr
STRAY CURRENT
� FOR EACH AMPERE OF CURRENT THAT FLOWS OFF THE PIPE SURFACE, MORE THAN 20 POUNDS OF STEEL WILL BE CORRODED EACH YEAR……………….
– For Std wall 2 - inch = 5.48 feet removed– For Std wall 4 - inch = 1.85 feet removed– For Std wall 6 - inch = 1.05 feet removed
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STRAY CURRENT
� FOR EACH AMPERE OF CURRENT THAT FLOWS OFF THE PIPE SURFACE, MORE THAN 20 POUNDS OF STEEL WILL BE CORRODED EACH YEAR
– For Std wall 2 - inch = 5.48 feet removed– For Std wall 4 - inch = 1.85 feet removed– For Std wall 6 - inch = 1.05 feet removed
� TYPICALLY PRODUCES THE HIGHEST CORROSION RATES EXPERIENCED UNDERGROUND
Impressed CurrentCathodic Protection System
18-16
RectifierGround
Bed
+
-Pipeline
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STRAY CURRENT
IF YOU REVERSE THE LEADS OF A RECTIFIER WITH A 10 AMP LOADYOU WILL LOSE:
54.8 FEET OF 2 - INCH MAIN18.5 FEET OF 4 - INCH MAIN10.5 FEET OF 6 - INCH MAIN
NATURALLY OCCURRING CORROSION
� 3 BASIC MECHANISMS
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� 3 BASIC MECHANISMS– DISSIMILAR METAL
NATURALLY OCCURRING CORROSION
� 3 BASIC MECHANISMS– DISSIMILAR METAL– DISSIMILAR ELECTROLYTE
NATURALLY OCCURRING CORROSION
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� 3 BASIC MECHANISMS– DISSIMILAR METAL– DISSIMILAR ELECTROLYTE– OXYGEN CONCENTRATION
NATURALLY OCCURRING CORROSION
Relative Energy Levels of Various Refined Metals
GOLD
COPPER
STEEL IN CONCRETE WITHOUT Cl
ZINC
MAGNESIUM
ALUMINUM
CARBONSILVER
PLATINUM
STEELSTEEL IN CONCRETE WITH Cl
-
-
NOBLE OR PASSIVE (+)
ACTIVE (-)
--
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Relative Energy Levels of Various Refined Metals
-1.7
+1.2GOLD
-0.1COPPER
-0.1STEEL IN CONCRETE WITHOUT Cl
-1.0ALUMINUM
MAGNESIUM
-1.1ZINC
+0.4CARBON
+0.5SILVER
+0.9PLATINUM
-0.6STEEL
-0.5STEEL IN CONCRETE WITH Cl-
-
Energy Level in Volts vs. Cu/CuSO Reference in soil
4
GALVANIC SERIES OF METALENERGY LEVELS
�Measured Potential Depends Upon:– Electrolyte
� Seawater� Fresh Water/Soil� Other
– Temperature
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GALVANIC SERIES OF METALENERGY LEVELS
�There is a Range in Measured Potential Not an Absolute Value
– 316 Passive Stainless - 50 mV to - 200 mV– Copper - 50 mV to - 300 mV– Carbon Steel -400 mV to - 750 mV– Zinc -900 mV to -1100 mV
ENERGY LEVEL DIFFERENCE BETWEEN CARBON AND ZINC
GOLD
COPPER
STEEL IN CONCRETE WITHOUT Cl
ZINC
MAGNESIUM
ALUMINUM
CARBON
SILVER
PLATINUM
STEEL
STEEL IN CONCRETE WITH Cl
-
-
Energy Level in Volts vs. Cu/CuSO Reference4
?
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ENERGY LEVEL DIFFERENCE BETWEEN CARBON AND ZINC
GOLD
COPPER
STEEL IN CONCRETE WITHOUT Cl
ZINC
MAGNESIUM
ALUMINUM
CARBON
SILVER
PLATINUM
STEEL
STEEL IN CONCRETE WITH Cl
-
-
Energy Level in Volts vs. Cu/CuSO Reference4
1.5V
-1.1
+0.4
A COMMON DRY CELL BATTERYIS A GALVANIC CORROSION CELL
CARBON ROD(CATHODE)
ZINC CASE(ANODE)
MOIST PASTE(ELECTROLYTE)
WIRE(CONDUCTOR)
CONVENTIONAL CURRENT
Zn++
H+
OH-
OH-
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CORROSION IS AN ELECTROCHEMICAL PROCESS
� THE CHEMICAL PART IS THE UNWANTED REVERSION OF THE METAL TO IT'S OXIDE FORM
CORROSION IS AN ELECTROCHEMICAL PROCESS
� THE CHEMICAL PART IS THE UNWANTED REVERSION OF THE METAL TO IT'S OXIDE FORM THAT IS INTRODUCED TO THE ELECTROLITE
� THE ELECTRO PART IS THE TRANSFER OF ENERGY (ELECTRONS) WHICH OCCURS DURING THE CORROSION PROCESS FROM ANODE TO THE CATHODE. THE ELECTRONS ARE TRANFERRED INSIDE THE METAL STRUCTURE
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CORROSION IS AN ELECTROCHEMICAL PROCESS
� THE CHEMICAL PART IS THE UNWANTED REVERSION OF THE METAL TO IT'S OXIDE FORM
� THE ELECTRO PART IS THE TRANSFER OF ENERGY WHICH OCCURS DURING THE CORROSION PROCESS
� WHAT WE UNDERSTAND, WE CAN CONTROL
CORROSION IS AN ELECTROCHEMICAL PROCESS
� THE CHEMICAL PART IS THE UNWANTED REVERSION OF THE METAL TO IT'S OXIDE FORM
� THE ELECTRO PART IS THE TRANSFER OF ENERGY WHICH OCCURS DURING THE CORROSION PROCESS
� WHAT WE UNDERSTAND, WE CAN CONTROL� TO UNDERSTAND CORROSION, WE MUST
UNDERSTAND BASIC ELECTRICITY
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CURRENT FLOW
ELECTRONIC IONIC
CAN BE EITHER:
ION
�Charged Atom or Molecule
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ION
�Charged Atom or Molecule
OH -
H + is a Hydrogen Atom without one electronwhich carries a positive charge of +1
is a Hydroxyl Molecule with an excess electronwhich carries a negative charge of -1
Both Electronic and Ionic Current Charge Transfer Occurs in Corrosion Cell
ELECTROLYTE (Solution containingcharged atoms or molecules)
METALLIC
PATH
COPPER
CATHODEIRON
ANODE
OH-
Fe++
H+ H
+-
e-
e-
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CURRENT
� Ampere
CURRENT
� Ampere� Electrical Charge Transfer through Distance per
Unit Time
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CURRENT
� Ampere� Electrical Charge Transfer through Distance per
Unit Time� 1 Coulomb per Second transferred between two
points
CURRENT
� Ampere� Electrical Charge Transfer through Distance per
Unit Time� 1 Coulomb per Second transferred between two
points� 6.24 x 10 electrons per Second transferred
between two points
18
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CURRENT
� Ampere� Electrical Charge Transfer through Distance per
Unit Time� 1 Coulomb per Second transferred between two
points� 6.24 x 10 electrons per Second transferred
between two points� SYMBOL = I
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CURRENT
� Ampere� Electrical Charge Transfer through Distance per
Unit Time� 1 Coulomb per Second transferred between two
points� 6.24 x 10 electrons per Second transferred
between two points� SYMBOL = I
– analogous to gas flow -- e.g. Cubic Feet per Hour
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ELECTRO-MOTIVE FORCE
� VOLT
ELECTRO-MOTIVE FORCE
� VOLT� The Potential (or energy) Difference between
the terminals of a source of electrical energy
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ELECTRO-MOTIVE FORCE
� VOLT� The Potential (or energy) Difference between
the terminals of a source of electrical energy� Basic Unit of Force which causes electric
charge transfer thru distance per unit time
ELECTRO-MOTIVE FORCE
� VOLT� The Potential (or energy) Difference between
the terminals of a source of electrical energy� Basic Unit of Force which causes electric
charge transfer thru distance per unit time� SYMBOL = E or V
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ELECTRO-MOTIVE FORCE
� VOLT� The Potential (or energy) Difference between
the terminals of a source of electrical energy� Basic Unit of Force which causes electric
charge transfer thru distance per unit time� SYMBOL = E or V
– analogous to gas pressure -- e.g. Pounds per Square Inch
RESISTANCE
� OHMS
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RESISTANCE
� OHMS� Impedance to Electric Charge Transfer through
distance per unit time
RESISTANCE
� OHMS� Impedance to Electric Charge Transfer through
distance per unit time� The tendency of a conductor to oppose the flow
of current, causing electrical energy to be changed into heat
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RESISTANCE
� OHMS� Impedance to Electric Charge Transfer through
distance per unit time� The tendency of a conductor to oppose the flow
of current, causing electrical energy to be changed into heat
� The unit of resistance which will limit the current flow to 1 Ampere from an applied EMF of 1 Volt
RESISTANCE
� OHMS� Impedance to Electric Charge Transfer through
distance per unit time� The tendency of a conductor to oppose the flow
of current, causing electrical energy to be changed into heat
� The unit of resistance which will limit the current flow to 1 Ampere from an applied EMF of 1 Volt
� Symbol = R or
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� OHMS� Impedance to Electric Charge Transfer through
distance per unit time� The tendency of a conductor to oppose the flow
of current, causing electrical energy to be changed into heat
� The unit of resistance which will limit the current flow to 1 Ampere from an applied EMF of 1 Volt
� Symbol = R or – analogous to the restriction of gas flow
caused by a given pipe diameter and length
RESISTANCE
Electrical Circuit Calculations
� We will learn how to use Ohm's Law to calculate either the current, volt or resistance factors in both series and parallel circuits.
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OHMS LAW
� The Current Flow in an Electrical Circuit (DC Circuit) is Directly Proportional to the EMF applied to the circuit and Inversely Proportional to the Resistance of the Circuit
I =ER
OHMS LAW
E
RI
I = ER
E = I x R
R = EI
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UNITS OF MEASURE
MILLIVOLT = 0.001 VOLTSVOLT = 1.000 VOLTSKILOVOLT = 1,000.000 VOLTSMEGAVOLT = 1,000,000.000 VOLTS
DO NOT MIX UNITS, i.e., MILLIVOLTS WITH AMPS
OR VOLTS WITH MILLIAMPS
SAMPLE CALCULATION
9 VOLT BATTERYR1 = 1 OHMR2 = 2 OHMS
WHAT ISTHE
CURRENTFLOW?
I = = = 3 AMPSER
__9__ (1 + 2)
RI
E
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• Basic theory of CP
– Galvanic anodes – metallic element that has a higher natural electromotive
force than that element being protected (i.e. – magnesium, zinc, and
aluminum to protect steel)
– Impressed current anodes – External direct current source connected to the
anode (more positive) and structure.
– Level of protection
• Generally -0.85 to -1.15 vdc typical (per NACE standard RP0169-96,
Section 6) for ground to soil (electrolyte) readings.
• If the system exceeds -1.17 volts area starts to be overprotected with -
1.22 volts generation hydrogen gas causing disbondment of the coating
Corrosion and Cathodic Protection
Types of Coatings• Coal Tar Enamels
• Mill-Applied Tape Systems
• Extruded Polyolefin with Butyl Adhesive
• Fusion-Bonded Epoxy
• Multi-layer Epoxy Extruded Polyolefin
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• A technique to reduce the corrosion rate of a metal surface by making it the
cathode of an electrochemical cell.
• 2 types of cathodic protection methods
– Sacrificial or Galvanic Anode
– Impressed Current
Cathodic Protection
Sacrificial or Galvanic Anode CP System
Anodes
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Corrosion Terms
• A/C – Alternating electrical current which flows first in one direction and then the opposite direction in a fixed pattern
• Amps – Basic unit of flow in an electrical or electronic circuit. Usually indicated as “I” in electrical Formulas
• Anode – The part of the corrosion cell that corrodes, or sacrifices itself, to protect the cathode portion of the corrosion cell.
• Battery – A device that stores an electrical charge for later use.
• Bridge – An electronic semi-conductor or electrical device that converts A/C power into D/C power.
• Cathode – The part of the corrosion cell that receives protection from the anode portion of the corrosion cell
• Cathodic Protection – The process of intentionally corroding one material to protect another material.
• Circuit Breaker – Provides overload protection and serves as an on/off switch for equipment.
• Coating – A di-electric material used to isolate a structure from the surrounding environment.
• Collins Meter – Trade name for an instrument used to measure soil resistivity.
• Conductor – Any material capable of carrying an electrical current.
• Copper-Copper Sulfate Reference Electrode – The standard reference used to measure the voltage potential of underground metallic structures. Commonly known as a Half-Cell, CUCUSO4 Reference Cell, or Reference Cell.
• Corrosion – The deterioration of a material, usually a metal, due to a reaction in its environment.
• Criteria – The rules used that indicate when cathodic protection has been achieved.
• Current Interrupter – Portable battery-operated instrument used to turn current producing equipment on and off in defined cycles during field testing procedures.
• D/C – Current which flows only in one direction.
• Diode – An electronic semi-conductor device that allows current to flow only in one direction.
• Electrolyte – The substance in which ions transverse from the anode to the cathode. Normally the earth surrounding a structure
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Corrosion Terms
• Fuse – An electrical device that protects equipment from damage due to an over-current or over-voltage condition.
• Insulator – A fitting or substance that exhibits a high resistance to electrical current flow.
• I-R Drop – A voltage developed due to current flowing through a resistance.
• Ohms – The term used to indicate the amount of resistance to electrical flow. Usually indicated as “R” in electrical formulas.
• Ohms Law – A mathematical statement describing the relationship of volts, amps, and ohms in an electrical circuit. In basic terms, the law states that:
– Volts = Ohms x Amps; or,
– E=I x R
• Resistance – Opposition to current flow. Usually indicated as “R” in electrical formulas.
• Resistivity – Resistance of an electrolyte such as earth. Usually expressed in “ohms per centimeter” or “Ohms/cM”
• Volts – The term used to describe the amount of pressure in an electrical circuit. Usually indicated as “E” in electrical formulas.