1. Understanding the corrosion environment
Teach-in
Understanding the corrosion environment

2. Any method be made more effective…
Different methods for corrosion control
Coupons
Online Monitors
Inhibition programs
Any method be made more effective…

3. …When you understand the effect of the corrosion environment
Corrosion rates vary with process conditions

4. 5.5% NaCl

5. 5.5% NaCl, 5 atm

6. 5.5% NaCl, 85 °C

7. 5.5% NaCl, 10 °C, 15 atm

8. It helps to know the effect of variations in the field
To interpret coupon and monitor data…
It helps to know the effect of variations in the field

9. Wait for a failure…? Rely on past experience?
To locate where to place sensors & coupons…
Wait for a failure…?
Rely on past experience?

10. Tell you what has already happened, not what will happen
Coupons
Online Monitors
Tell you what has already happened, not what will happen

11. OLI tools can help
OLI gets the chemistry right

12. ?
Dew point pH
Phase splits

13. Active Corrosion (dissolution)
Understand what’s happening in your system
Active Corrosion (dissolution) pH
Protective Scale
Passive Film

14. Activation controlled
Determine the rate limiting redox processes
Passive region
Activation controlled
Rate-limiting cathodic process

15. Determine pitting potential and max growth rate
No Pitting
Pitting

16. Pro-active Analysis Test Corrective Actions Determine optimum pH
Screen alloys and inhibitors
Assess process changes
Focus Lab work
Eliminate potential problems before they occur

17. The Corrosion Analyzer
Tool for understanding the corrosion environment
Mechanistically-based software tool
Speciation
Kinetics of uniform corrosion Partial anodic and cathodic processes
Transport properties
Repassivation

18. The Corrosion Analyzer
Based on the OLI Engine
Complete speciation model for complex mixtures
Phase and chemical reaction equilibria
Accurate pH prediction
Redox chemistry
Comprehensive coverage of industrial chemical and petroleum systems

19. The Corrosion Analyzer
Based on the OLI Engine
Thermophysical properties prediction
Phenomenological and unique aqueous process models including kinetics and transport
“Out-of-the-box” solution and technical support

20. The Corrosion Analyzer
What It Does…
Predict metal dissolution regime, passive films, and surface deposits
Predict uniform corrosion rates and the potential for pitting corrosion
Generate real solution stability (Pourbaix) Diagrams
Produce theoretical polarization curves

21. The Corrosion Analyzer
So you can gain insight on …
Corrosion mechanisms
Rate-limiting partial processes for your operating conditions
Effects of process and materials changes
Therefore
Focusing lab time
Reducing risky plant/field testing
Managing design, operation, and maintenance

22. Today’s seminar “Hands-on” and “How-To” Using example problems
Examining plots and diagrams
Understanding the basis of the predictions

23. Today’s Seminar Perform “Single point” calculations
Construct / interpret real solution Pourbaix Diagrams
Calculate corrosion rates
Evaluate the effects of pH, T, comp / flow
Evaluate polarization curves
Gain insight to corrosion mechanisms
See rate limiting steps
Can I read them? Can I trust them?
Determine the likelihood of pitting to occur
For your actual field or lab conditions

24. Simulating Real World Corrosion Problems
Welcome to the
CORROSION TEACH-IN
Simulating Real World Corrosion Problems

25. Gas Condensate Corrosion
Scope
Gas condensates from alkanolamine gas sweetening plants can be highly corrosive.
Purpose
Diethanolamine is used to neutralize (sweeten) a natural gas stream. This removes carbon dioxide and hydrogen sulfide. The off gas from the regeneration is highly acidic and corrosive

26. Gas Condensate Corrosion
Objectives
Determine the dew point of the acid gas
Remove the condensed phase and perform corrosion rate calculations
Mitigate the corrosion

27. Gas Sweetening
Sour Gas Absorber
Acid Gas
Absorber liquor regenerator

28. Acid Gas Concentrations
Species
Concentration (mole %)
H2O
5.42
CO2
77.4 N2
0.02
H2S
16.6
Methane
0.50
Ethane
0.03
Propane
Temperature
38 oC
Pressure
1.2 Atm.
Amount
100 moles

29. Application Time

30. Dew Point
Dew Point = 37.6 oC
pH = 3.93
ORP = V

31. Corrosion Rates: Flow Conditions
Flow conditions have a direct effect on mass-transfer
Static
Pipe flow
Rotating disk
Rotating cylinder
Complete agitation

32. Application Time

33. Carbon Steel Corrosion @ Dew Point
Corrosion Rate = 0.7 mm/yr
Corrosion Potential = V
Repassivation Potential = > 2 V
Current Density = 60.5 A/cm2
H2CO3(aq)= ½ H+ + HCO3- - e
H2S(aq)= ½ H2 + HS- - e
HS-= ½ H2 + S2- - e
H+= ½ H2 - e

34. Mitigation Adjusting solution chemistry Temperature profiling
Alloy screening
Cathodic protection

35. Adjusting the Solution Chemistry
Changing operating pH
Add acid or base

36. Application Time

37. Adjusting solution pH = 8.0

38. Screening Alloys
Select an alloy that has a preferential corrosion rate
13% chromium
304 Stainless

39. Application Time

40. 13 % Cr Steel Corrosion @ Dew Point
Corrosion Rate = 0.06 mm/yr
Corrosion Potential = V
Repassivation Potential = > 2 V
Current Density = 5.7 A/cm2
H2CO3(aq)= ½ H+ + HCO3- - e
HS-= ½ H2 + S2- - e

41. 304 Stainless Steel Corrosion @ Dew Point
Corrosion Rate = mm/yr
Corrosion Potential = V
Repassivation Potential = > 2 V
Current Density = 0.3 A/cm2

42. 304 Stainless Steel Stability @ Dew Point
Passivation is possible due to Cr2O3

43. Explaining common observations using Stability Diagrams
Why Iron Rusts
Explaining common observations using Stability Diagrams

44. Basics
Iron is inherently unstable in water & oxidizes via the following reactions to form rust
Its severity depends on (among others)
Conditions (T/P),
Composition,
pH, and
oxidation potential
These four can be plotted on a single chart called a stability diagram

45. Start example

46. White area is region of iron corrosion
Explaining the EH-pH diagram using Fe, showing solid and dissolved species over range of pH’s and oxidation potentials
H2O is oxidized to O2 and H+
H2O is reduced to H2 and OH-
Elemental iron, Fe(0)o, is stable and will not corrode in this region
H2O is stable and deaerated
H2O is stable and aerated
Fe2O3 reduces and dissolves in water
Fe(II) oxidizes and precipitates as Fe2O3
Elemental iron, Fe(0) oxidizes to Fe(II) in the presence of water
FeO(OH), rust is stable in water at moderate to high pH’s
White area is region of iron corrosion
Water Oxidation Line
Water Reduction Line
Fe3O4 coats the iron surface, protecting it from corrosion
Fe(III)3+ is the
dominant ion
Fe(II)2+ is the
Elemental iron (gray region) corrodes in water to form one of several phases, depending on pH. At ~9 pH and lower, water oxidizes Fe0 to Fe+2 which dissolves in water (white region of the plot). As the oxidation potential increases (high dissolved O2) Fe+2 precipitates as FeOOH, or rust (green region). The lower the pH, the thicker the white region and the greater driving force for corrosion
At higher pH (10-11), Fe0 forms Fe3O4, a stable solid that precipitates on the iron surface, protecting it from further attack.

47. Q: We all know O2 is bad…But how much is bad?
H2O is oxidized to O2 and H+
H2O is stable and aerated
Water Oxidation Line
10 ppm O2
0.1ppm H2
500 ppm O2
80 ppm H2
0.1 ppb H2
3 ppb O2
0.1 ppT H2
0.1 ppT O2
Pure water is here…
No air, no acid, no base
H2O is reduced to H2 and OH-
H2O is stable and deaerated
Water Reduction Line

48. Region of instability Elemental Iron (Feo)
Iron and water react because they are not stable together
Region of instability
The reaction generates 2OH-, which increases the pH
The reaction generates H2, which puts the EH near the bottom line
Elemental Iron (Feo)

49. Start example on Page 36-39

50. The reaction ends within the Fe3O4 region
The reaction ends within the Fe3O4 region. Fe3O4 is a solid that passivates the iron surface protecting it from active corrosion
Initial Conditions
DI water, no Feo
7pH, 0.4V
Final Conditions
1 ppm Feo added
9.38pH, 0.5V
0.9 ppb Feo
7.07pH, -0.27V
0.1 ppm Feo
8.48pH, -0.42V

51. Overlaying the Fe3O4 mass on the diagram – once the pH reached 9, Fe3O4 began to precipitate
1.4 g Fe3O4 ppts from 1 Feo
Fe3O4 precipitates when 0.3 mg/l Feo has reacted
The ppt point lines up with the stability curve

52. Start example on Page 40-41

53. If a constant source of O2 is present, then the EH and pH do not change, and we are stuck in the rust region
The EH and pH does not change as Feo reacts with aerated water

54. Why is Stainless Steel stainless?

55. Cr will oxidizes, but the reaction goes through a tough Cr2O3 protective layer.

56. Ni3Fe2O4 is stable in the corrosion region, and will also protect the surface.

57. Simulating Real World Corrosion Problems
Welcome to the
CORROSION TEACH-IN
Simulating Real World Corrosion Problems

58. Corrosion in Seawater Scope
Metals used for handling sea water face both general and localized corrosion.
Various grades of stainless steels have been used to mitigate the problems.
Stainless steels owe their corrosion resistance to a thin adherent film of oxides on their surface.
Disruption of the films can lead to localized corrosion and premature failure.

59. Corrosion in Seawater Purpose
Chlorine and oxygen in sea water can attack the films used to passivate the steels.
The CorrosionAnalyzer will be used to model the effects of chloride and oxygen on the rates of uniform corrosion and the possibility of pitting on the surface of the metals.

60. Corrosion in Seawater Objectives
Reconcile a sea water sample for electroneutrality
Reconcile a gas analysis
Calculate uniform rates of corrosion for
304 stainless steel
316 stainless steel
S31254 stainless steel

61. Corrosion in Seawater Objectives (continued)
Determine the probability of pitting using the localized corrosion feature.

62. Kinetic Model of General Corrosion: Mass-Transfer
Metal
Surface
Solution
All reactions take place on the metal surface.
Films are a diffusion barrier to corrosive species
Reduce mass-transfer-limited currents.
Mass-transfer from solution is calculated from a concentration- dependent diffusion coefficient.
film

63. Chemistry The rates of corrosion use a subset of the OLI Chemistry
Neutral Species
H­2O, O2, CO2, H­2S, N2 and all inert gases, Cl2, SO2, So and NH3, organic molecules that do not undergo electrochemical reactions
Anions
OH-, Cl-, Br-, I-, HCO3-, CO3-2, HS-, S2-, SO42-, HSO4-, SO32-, NO2-, NO3-, MoO42-, CN-, ClO4-, ClO3-, ClO-, acetate, formate, Cr(VI) anions, As(III) anions, P(V) anions, W(VI) anions, B(III) anions and Si(IV) anions.

64. Chemistry
Cations
H+, alkali metals, alkaline earth metals, Fe(II) cations, Fe(III) cations, Al(III) cations, Cd(II) cations, Sn(II) cations, Zn(II) cations, Cu(II) cations, Pb(II) cations and NH4+.

65. Corrosion of 304 Stainless Steel in Deaerated Sea Water
LabAnalyzer used to reconcile electroneutrality
NaOH/HCl Used to adjust pH
Species
Concentration (mg/L)
Cl-
19000
Na+
10700
Mg+2
1300
Ca+2
400
SO4-2
2750
HCO3-
150 pH
8.0
Temperature
25 oC
Pressure
1 atm.

66. Application Time

67. Screening Considerations
Some alloys do not perform well in seawater
We will evaluate 3 stainless steels
Uniform corrosion rates
Pitting possibility
Considering both deaerated and aerated conditions

68. Corrosion of 304 Stainless Steel in Deaerated Sea Water
300 years to lose 1 mm of metal oC

69. Corrosion of 304 Stainless Steel in Deaerated Sea Water
Large difference means that pits are unlikely to form
Repassivation Potential
Difference = 0.05 V
Corrosion Potential
Or if a pit forms, then it will passivate

70. What’s on a Polarization Curve?
Standard Tafel Behavior
Transition to mass-transfer limited current density

71. What’s on a Polarization Curve?
The curve is only valid in aqueous systems and will be bounded by the decomposition of water.
Intersection indicates location of the corrosion potential
Current density at corrosion potential also read at intersection

72. What’s on a Polarization Curve?
Basic polarization curve with water decomposition and corrosion reaction

73. What’s on a Polarization Curve?
Polarization curve with water decomposition, corrosion reaction and two mass-transfer-limited reactions.

74. What’s on a Polarization Curve?
This is what is measured experimentally
Transpassive region
Passive region
Corrosion Potential and Corrosion current
Active Corrosion

75. What’s on a Polarization Curve?
Transpassive
Passive
Active
Polarization curve demonstrating a galvonostatic sweep. The arrows indicate how the potential is changing as one moves along the line.

76. There are many processes that make up the polarization curve.
Fe = Fe+2 + 2e-
2H2O=O2+4H++4e-
H2O + e- = ½ H2+OH-
H+ + e- = ½ H2

77. The Polarization Curve for 304 SS in Deaerated Water
Oxidation of water to O2
Measurable polarization curve
Breakdown of water to H2
Peak Current density in the pit with the highest corrosion rate
Open circuit potential and current density
Corrosion of 304 ss

78. Kinetic Model of General Corrosion: Phenomena
Partial electrochemical processes in the active state:
Cathodic reactions (e.g., reduction of protons, water molecules, oxygen, etc.)
Anodic reactions (e.g., oxidation of metals)
Adsorption of species on the metal surface
Active-passive transition influenced by
Acid/base properties of passive oxide films
Temperature
Additional species that influence the dissolution kinetics of oxide layers
Synthesis of the partial processes according to the mixed potential theory
May 20, 1997
OLI Systems, Inc,

79. Application Time

80. Corrosion of 316 SS in Deaerated WateroC
1886 years to lose 1 mm of metal
Much better corrosion rate than 304 ss

81. Corrosion of 316 SS in Deaerated Water
Difference = V

82. Application Time

83. Corrosion of 254 SMO in Deaerated Water
Corrosion rate = oC
> 3000 years to lose 1 mm of metal

84. Corrosion of 254 SMO in Deaerated Water
Difference = 2.7 V

85. Summary in Deaerated Water
Stainless
25 oC (mm/yr)
Potential difference (V)
304
0.0033
0.05
316
0.086
254 SMO
2.7

86. Adding Air/Oxygen
The CorrosionAnalyzer allows you to add a gas phase based only on partial pressures
You can set the water/gas ratio
Species
Partial Pressure (atm) N2
0.7897 O2
0.21
CO2
0.0003
WGR
0.01 bbl/scf

87. Application Time

88. 304 SS in Aerated Solutions

89. 304 SS in Aerated Solution
The corrosion potential is greater than the passivation potential = .37 V at max O2
Pitting will occur

90. 304 SS Polarization in Aerated Water
8 ppm O2
Corrosion potential shifted anodically of the repassivation potential.
0 ppm O2
The surface will couple galvanically with the pits to increase their rate of corrosion.

91. Application Time

92. 316 SS Corrosion in Aerated Water
Pitting occurs at higher oxygen concentrations = .21V at max O2

93. Application Time

94. S31254 Corrosion in Deaerated Water
Pitting should not occur

95. Stability Diagram for 316L SS

96. Stability Diagram for 316 L Nickel Only

97. Mitigation Change Alloys Cathodic Protection
S31254 seems the best at 25 oC
S31254 increased potential for pitting at higher temperatures
Cathodic Protection
Shifting of potential to less corrosive potentials via a sacrificial anode.
Analyzers do not model CP
Polarization curves can help determine the change in potential.

98. Simulating Real World Corrosion Problems
Welcome to the
CORROSION TEACH-IN
Simulating Real World Corrosion Problems

99. Dealloying of Copper Nickel Alloys
Scope
A copper-nickel pipe made of Cupronickel 30 has been preferentially dealloyed while in contact with a 26 weight percent calcium chloride brine. It appears that the nickel in the alloy has been preferentially removed.

100. Dealloying of Copper Nickel Alloys
Purpose
The OLI/CorrosionAnalyzer will be used to show the relative stability of nickel and copper in the cupronickel alloy in an aqueous solution. It will show that protective films were not present as originally thought.

101. Dealloying of Copper Nickel Alloys
Objectives
Input information into the software and perform calculations
Use stability diagrams to display information about the alloy and the protective films
Change the diagrams to view different aspects of the stability of the alloy

102. Application: Dealloying of Copper-Nickel Alloys
A cupronickel 30 pipe (30 mass % copper) was used.
26 wt % CaCl2 solution was in contact with the pipe.
Nickel was preferentially removed.
Dealloyed cupronickel pipe.

103. Questions? Why did the nickel dealloy from the pipe?
What could we do to prevent this from occurring?
Which tools are available to understand this phenomenon?

104. Which Tools are Available?
A Pourbaix diagram can help us determine where metals are stable.
CorrosionAnalyzer

105. Creating the First Stability Diagram
We will use the CorrosionAnalyzer  to create a stability diagram for this system.
Features of CorrosionAnalyzer  diagrams
Real-solution activity coefficients
Elevated temperatures
Elevated pressures
Interactions between species and overlay of diagrams.

106. The Pourbaix Diagram

107. Application Time
Time to start working with the OLI Corrosion Analyzer

108. The Pourbaix Diagram
There are quite a few things to look at on this diagram.
Stability field for water
Stability fields for nickel metal and copper metal
Stability fields for nickel and copper oxides
Stability fields for aqueous species.
We will now break down the diagram in to more manageable parts.

109. Stability Diagram Features
Subsystems
A base species in its neutral state and all of its possible oxidation states.
Cuo, Cu+1, Cu+2
Nio, Ni+2
All solids and aqueous species that can be formed from the bulk chemistry for each oxidation state.

110. Stability Diagram Features
For each subsystem
Contact Surface
Base metals
Alloys
Films
Solids
Solid Lines
Aqueous Lines

111. Stability Diagram Features
Natural pH
Prediction based on the bulk fluid concentrations
Displayed as a vertical line
Solids
All solids included by default
The chemistry can be modified to eliminate slow forming solids.

112. Stability Diagram Features
Passivity
Thin, oxidized protective films forming on metal or alloy surfaces.
Transport barrier of corrosive species to metal surface.
Blocks reaction sites

113. Water Stability Water can act as an oxidizing agent
Water is reduced to hydrogen, H2
Water can act as a reducing agent
Water is oxidized to oxygen, O2
To be stable in aqueous solution, a species must not react with water through a redox process.

114. Water Stability

115. Water Stability – Natural Waters
Surface water
Ocean water
Bog water
Organic rich lake water
Organic rich waterlogged soils
Organic rich saline water

116. Copper Pourbaix Diagram
Oxidized Species
E Independent acid and base chemistry
Predominant species
pH dependent redox
pH independent redox
Reduced Species

117. Copper Pourbaix Diagram
Aqueous species
Stability field for passivating film
Equilibrium between species in contact with a solid
Equilibrium between species
Natural pH
Stability field for base metal or alloy

118. Copper Pourbaix Diagram
Stable copper metal in alloy extending into water stability field.
The solution pH is in a region where the copper metal will be stable.
Copper pipes are used for potable water for this reason.

119. Nickel Pourbaix Diagram
No Nickel metal extends into the water stability field
The solution pH is in a region where nickel is expected to corrode

120. Ni Overlaid on Cu We need to know the Oxidation/Reduction potential
CuCl(s) may form to protect the alloy at the solution pH.
Since the nickel is part of a copper-nickel alloy, it is possible that copper could provide a protective film

121. Application Time

122. CorrosionAnalyzer Calculation

123. CorrosionAnalyzer Calculation
The oxidation reduction potential is V

124. Ni Overlaid on Cu
The potential of V lies above the passivating film. Dealloying can occur.

125. Conclusions Why did dealloying occur?
No protective film at the operating pH and oxidation/reduction potential of the process fluid.
Copper lies within the region of water stability
Nickel does not lie within the region of water stability
The presence of Cu+ ions in equilibrium with copper metal promotes replating of copper metal driven by the oxidation of nickel.

126. Chemistry Standard OLI Chemistry
7400 components
9100 individual species
82 Elements of the Periodic Table fully covered
8 additional elements partially covered.
Stability diagrams have access all of this chemistry

127. Chemistry Alloys 6 predefined classes supported User defined alloys
Cu-Ni
Carbon Steels – Fe, Mn, and C
Ferritic Stainless steels – Fe, Cr, Ni, Mo and C
Austenitic stainless steels - Fe, Cr, Ni, Mo and C
Duplex stainless steels FCC phase - Fe, Cr, Ni, Mo, C and N
User defined alloys

128. Limits to the Standard OLI Chemistry
Aqueous Phase
XH2O > 0.65
-50oC < T < 300oC
0 Atm < P < 1500 Atm
0 < I < 30
Non-aqueous Liquid
Currently no Activity Coefficient Model (i.e., no NRTL, Unifaq/Uniqac)
Fugacity Coefficients are determined from the Enhanced SRK

129. Limitations of Pourbaix Diagrams
No information on corrosion kinetics is provided.
Diagram is produced from only thermodynamics.
Diagram is valid only for the calculated temperature and pressure
Oxide stability fields are calculated thermodynamically and may not provide an actual protective film.
Dealloying cannot be predicted from the diagram alone.