16.2 Corrosion Mechanisms, Materials Degradation, and Prevention

16.2 Corrosion Mechanisms, Materials Degradation, and Prevention

Corrosion represents one of the largest single operational costs and safety risks in the chemical process industries (CPI), accounting for billions of dollars annually in premature equipment replacement, unscheduled outages, toxic releases, and fires. Chemical engineers must be able to diagnose corrosion failure modes, calculate metal loss rates, select appropriate alloys, and design cathodic or chemical mitigation systems. On the NCEES PE Chemical Exam, corrosion questions encompass electrochemical thermodynamics, rate kinetics, localized attack phenomena, environmental cracking, and standard industry guidelines (such as NACE/AMPP standards and API Recommended Practices).

---

1. Electrochemical Foundations of Aqueous Corrosion

Anodic and Cathodic Half-Cell Reactions

Aqueous corrosion is an electrochemical process involving the transfer of electrons across a metal-solution interface. The process requires four components: an anode, a cathode, an electrolyte (ionic conductor), and a metallic path (electronic conductor). Removing any one of these four stops the corrosion process completely.

                    Metallic Conductor (Electron Flow: e- --->)
          ===============================================================
                   ANODE (-)                             CATHODE (+)
             M -> M^(n+) + n e-                   2 H+ + 2 e- -> H2 (Acid)
          (Metal Dissolution Loss)            O2 + 2 H2O + 4 e- -> 4 OH- (Base)
          ---------------------------------------------------------------
                             ELECTROLYTE (Ionic Solution)
                             Current Flow: Ions (M^(n+), OH-)

1. Anodic Reaction (Oxidation): Metal atoms lose electrons and dissolve into the electrolyte as cations:

   $$M \longrightarrow M^{n+} + n e^-\qquad (\text{Metal Loss / Dissolution})$$
   • Iron dissolution: $\text{Fe} \longrightarrow \text{Fe}^{2+} + 2e^-$
   • Aluminum dissolution: $\text{Al} \longrightarrow \text{Al}^{3+} + 3e^-$

2. Cathodic Reaction (Reduction): Electrons liberated at the anode travel through the metal to cathodic sites where they are consumed by reducible chemical species in solution. Common cathodic reactions in chemical plants include:

   • Hydrogen Evolution (Deaerated Acids, $\text{pH} < 7$): $$2\text{H}^+ + 2e^- \longrightarrow \text{H}_2 \uparrow$$
   • Oxygen Reduction (Aerated Acidic Solutions): $$\text{O}_2 + 4\text{H}^+ + 4e^- \longrightarrow 2\text{H}_2\text{O}$$
   • Oxygen Reduction (Aerated Neutral or Alkaline Solutions, Cooling Water): $$\text{O}_2 + 2\text{H}_2\text{O} + 4e^- \longrightarrow 4\text{OH}^-$$
   • Water Reduction (Deaerated Neutral or Alkaline Solutions): $$2\text{H}_2\text{O} + 2e^- \longrightarrow \text{H}_2 \uparrow + 2\text{OH}^-$$

The Nernst Equation & Thermodynamics

The reversible electrochemical potential (E) of a half-cell reaction at non-standard conditions is governed by the Nernst Equation:

$$E = E^\circ - \frac{R T}{n F} \ln Q = E^\circ - \frac{2.3026 R T}{n F} \log_{10} Q$$

At standard ambient conditions ($25^\circ\text{C} = 298.15\text{ K}$):

$$E = E^\circ - \frac{0.05916}{n} \log_{10} \left( \frac{[\text{Red}]^b}{[\text{Ox}]^a} \right)$$

Where $E^\circ$ is the standard reduction potential versus the Standard Hydrogen Electrode (SHE), (n) is the number of moles of electrons transferred, (F) is Faraday's constant ($96,485\text{ C/mol } e^-$), and (Q) is the reaction quotient.

Pourbaix ($E\text{-pH}$) Diagrams

A Pourbaix diagram maps the thermodynamically stable phases of a metal-water system as a function of electrochemical potential ((E)) and solution $\text{pH}$:

   Potential E (V vs. SHE)
      ^
 +1.2 |           (Oxygen Evolution Line b: O2 + 4H+ + 4e- = 2H2O)
      |   CORROSION             PASSIVATION
      |    (Fe^3+)                (Fe2O3 Passive Oxide Film)
  0.0 |------------------------------------------------------------
      |    (Fe^2+)            
      |   CORROSION               (Fe3O4 Magnetite Film)
 -0.4 |------------------------+-----------------------------------
      |  (Hydrogen Line a: 2H+ + 2e- = H2)
 -1.0 |                   IMMUNITY
      |                (Elemental Fe Stable, No Dissolution)
      +------------------------+-----------------------------------> pH
      0                        7                                  14

• Immunity Zone: Potential is sufficiently negative that metal dissolution is thermodynamically impossible; the metal remains in its elemental state. This is the operating principle of Cathodic Protection.
• Corrosion Zone: Soluble metal cations (e.g., $\text{Fe}^{2+}, \text{Fe}^{3+}, \text{Al}^{3+}$) are thermodynamically stable, resulting in active metal dissolution and wall loss.
• Passivation Zone: Insoluble, protective oxide or hydroxide films (e.g., $\text{Fe}_2\text{O}_3, \text{Cr}_2\text{O}_3, \text{TiO}_2, \text{Al}_2\text{O}_3$) are thermodynamically stable. These films form a thin ($1 - 5\text{ nm}$), non-porous barrier that stifles ionic diffusion, reducing corrosion current density by orders of magnitude.

---

2. Uniform Corrosion & Corrosion Penetration Rate (CPR)

The CPR Equation

Uniform (general) corrosion is the even, distributed loss of metal across the entire exposed surface. The Corrosion Penetration Rate (CPR) represents the thickness of metal consumed per unit time, derived from mass-loss coupon testing:

$$\text{CPR} = \frac{K \Delta W}{\rho A t}$$

Where:

• $\Delta W$ = mass loss of the test coupon during exposure time (t).
• $\rho$ = metal mass density ($\text{g/cm}^3$; e.g., carbon steel $\rho = 7.85\text{ g/cm}^3$, 316L SS $\rho = 8.00\text{ g/cm}^3$, titanium $\rho = 4.51\text{ g/cm}^3$).
• (A) = total exposed surface area.
• (t) = exposure time in hours.
• (K) = dimensional constant determined by target units:

$$\begin{aligned} \text{For CPR in } \mathbf{mpy} \text{ (mils per year, where } 1\text{ mil} = 0.001\text{ in}): & \quad K = 534 \quad (\Delta W \text{ in } \mathbf{mg}, \rho \text{ in } \mathbf{g/cm}^3, A \text{ in } \mathbf{in}^2, t \text{ in } \mathbf{hr}) \\ \text{For CPR in } \mathbf{mm/yr} \text{ (millimeters per year)}: & \quad K = 87.6 \quad (\Delta W \text{ in } \mathbf{mg}, \rho \text{ in } \mathbf{g/cm}^3, A \text{ in } \mathbf{cm}^2, t \text{ in } \mathbf{hr}) \end{aligned}$$

Unit Conversion:

$$1.0\text{ mm/yr} = 39.37\text{ mpy} \iff 1.0\text{ mpy} = 0.0254\text{ mm/yr} = 25.4\;\mu\text{m/yr}$$

Faraday's Law Link: Current Density to Corrosion Rate

By Faraday's Law, the mass loss rate is directly proportional to the corrosion current ($I_{\text{corr}}$) or corrosion current density ($i_{\text{corr}} = I_{\text{corr}} / A$):

$$\text{CPR} = \frac{C_F \cdot i_{\text{corr}} \cdot \text{EW}}{\rho}$$

Where $i_{\text{corr}}$ is in $\mu\text{A/cm}^2$, $\rho$ is in $\text{g/cm}^3$, $\text{EW}$ is the equivalent weight of the alloy ($\text{EW} = M/n$, in $\text{g/equivalent}$), and $C_F = 0.129$ when $\text{CPR}$ is in mpy (or $C_F = 0.00327$ for mm/yr).

Industrial Acceptability Guidelines

• $< 1.0\text{ mpy} \; (< 0.025\text{ mm/yr})$: Outstanding corrosion resistance. Essential for critical parts, valve trim, instrumentation, and thin heat exchanger tubes.
• $1.0 - 5.0\text{ mpy} \; (0.025 - 0.125\text{ mm/yr})$: Excellent resistance. Standard service for pressure vessels, tanks, and piping with standard corrosion allowances.
• $5.0 - 20.0\text{ mpy} \; (0.125 - 0.50\text{ mm/yr})$: Moderate resistance. Usable for short service lives or non-critical piping with heavy corrosion allowance.
• $> 20.0\text{ mpy} \; (> 0.50\text{ mm/yr})$: Unacceptable. Rapid failure, severe fouling, and product contamination.

---

3. Galvanic Corrosion & The Area Ratio Effect

Mechanism & Galvanic Series

When two electrochemically dissimilar metals are in direct electrical contact within an electrolyte, the potential difference creates a galvanic couple:

• The more active (less noble) metal becomes the anode and suffers accelerated galvanic corrosion.
• The more noble (more positive) metal becomes the cathode and is galvanically protected from corrosion.

The driving force is established by the Galvanic Series in Seawater (more practical than the standard EMF series because it accounts for actual passivity):

$$\begin{aligned} \mathbf{Active \; (Anodic)}: & \quad \text{Magnesium} > \text{Zinc} > \text{Aluminum 7075} > \text{Carbon Steel} > \text{Cast Iron} \\ & \quad > \text{Stainless Steel (Active)} > \text{Lead} > \text{Tin} > \text{Copper} > \text{Monel 400} \\ \mathbf{Noble \; (Cathodic)}: & \quad > \text{Stainless Steel (Passive)} > \text{Inconel 625} > \text{Hastelloy C-276} > \text{Titanium} > \text{Platinum} > \text{Graphite} \end{aligned}$$

The Critical Cathode-to-Anode Area Ratio

Conservation of electric charge dictates that the total anodic current must equal the total cathodic current: $I_A = I_C$. Expressed in current densities ((i = I/A)):

$$\ni_A A_A = i_C A_C \implies i_A = i_C \left( \frac{A_C}{A_A} \right)$$

   CASE 1: DISASTER (Large Cathode / Small Anode)
   +--------------------------------------------------------------+ 
   |  LARGE CATHODE (Stainless Steel Plate, Area Ac = 100)        |  
   +------------------------------+--+----------------------------+ 
                                  |xx| <--- SMALL ANODE (Carbon Steel Rivet, Area Aa = 1)
                                            Penetration Rate = i_c * (100 / 1) = 100x !

   CASE 2: BENIGN (Small Cathode / Large Anode)
   +--------------------------------------------------------------+ 
   |  LARGE ANODE (Carbon Steel Plate, Area Aa = 100)             |  
   +------------------------------+--+----------------------------+ 
                                  |oo| <--- SMALL CATHODE (Stainless Steel Fastener, Area Ac = 1)
                                            Galvanic Acceleration = i_c * (1 / 100) = 0.01x (Negligible)

---

4. Localized Corrosion: Pitting, Crevice, and PREN

Pitting Corrosion & Autocatalytic Acidification

Pitting is an extremely insidious form of localized attack where passive films locally break down in the presence of halides (especially chlorides, $\text{Cl}^-$), forming deep, narrow holes while the surrounding surface remains completely unattacked.

Once a pit initiates, it grows by a self-sustaining autocatalytic mechanism:

                              Bulk Solution (Aerated, Neutral pH ~ 7)
                               O2 + 2 H2O + 4 e- -> 4 OH- (Cathode)
         ====================                       ==================== (Passive Film)
         Metal Surface      \                       /  Metal Surface
                             \    +-------+        /
                              \   | Cl-   |       /
                               \  | Migr. | v    /
                                \ +-------+     / 
                                 |             |
                                 | Anode:      |
                                 | M -> M+ + e-|
                                 +-------------+
                                  Inside Pit: Hydrolysis creates HCl !
                                  M+ + Cl- + H2O -> MOH + H+ + Cl-
                                  Local pH drops to 1 - 2 !

1. Inside the pit, metal rapidly oxidizes: $\text{Fe} \longrightarrow \text{Fe}^{2+} + 2e^-$.
2. Because the pit mouth is narrow, stagnant fluid prevents dissolved oxygen from replenishing inside the pit. Cathodic reduction of oxygen shifts to the exterior surface.
3. The concentrated build-up of positive $\text{Fe}^{2+}$ ions attracts negative chloride ions ($\text{Cl}^-$) from the bulk solution to maintain electroneutrality.
4. Hydrolysis occurs inside the pit: $$\text{Fe}^{2+} + 2\text{H}_2\text{O} + 2\text{Cl}^- \longrightarrow \text{Fe}(\text{OH})_2 \downarrow + 2\text{H}^+ + 2\text{Cl}^-$$
5. Generation of free $\text{H}^+$ and $\text{Cl}^-$ produces concentrated hydrochloric acid ($\text{HCl}$), driving local pit $\text{pH}$ down to (1.0 - 2.0). The acidic chloride environment permanently destroys passivity, drilling rapidly through the vessel wall.

Pitting Resistance Equivalent Number (PREN)

Resistance to localized pitting and crevice attack in chloride environments is quantified by empirical alloy composition:

$$\text{PREN} = \% \text{Cr} + 3.3 (\% \text{Mo}) + 16 (\% \text{N})$$

(In some duplex specifications, the nitrogen factor is 30: $\text{PREN}_{30} = \% \text{Cr} + 3.3\% \text{Mo} + 30\% \text{N}$. The factor 16 is standard in NCEES specifications).

• Type 304 SS (18Cr-8Ni-0Mo): $\text{PREN} \approx 18 - 20$. Prone to pitting in tap water containing $> 200\text{ ppm}$ chlorides.
• Type 316L SS (17Cr-12Ni-2.5Mo): $\text{PREN} \approx 23 - 25$. Resists chlorides up to $1,000\text{ ppm}$ at ambient temperature.
• Duplex 2205 (22Cr-5Ni-3Mo-0.18N): $\text{PREN} \approx 35$. Excellent resistance in brackish water.
• Super Duplex 2507 & 6% Mo Super-Austenitics (AL-6XN, 254 SMO): $\text{PREN} \ge 40 - 45$. Seawater service and warm chlorinated brine require $\text{PREN} \ge 40$ to prevent localized pitting.

Crevice Corrosion

Crevice corrosion occurs in narrow, stagnant geometries ($w < 100\;\mu\text{m}$) such as gasket flange faces, threaded connections, beneath tube-sheet roll expansions, or under sedimentary deposits. The mechanism mirrors pitting: oxygen within the micro-gap is quickly consumed, establishing a differential aeration cell. Chloride migration and subsequent hydrolysis create acidic $\text{HCl}$, causing aggressive localized metal dissolution. The Critical Crevice Temperature (CCT) is typically $20 - 30^\circ\text{C}$ lower than the Critical Pitting Temperature (CPT).

---

5. Environmental Cracking & Metallurgical Degradation

   +-------------------------------------------------------------------------+
   |                  Environmental Cracking Mechanisms                      |
   +-------------------------------------------------------------------------+
   | Stress Corrosion Cracking (SCC) -- Tensile Stress + Specific Chemical   |
   |   - Chloride SCC ---------------- Austenitic SS (304/316) > 60°C (140°F)|
   |   - Caustic Embrittlement ------- Carbon steel in hot NaOH (> 50-80°C)  |
   |   - Amine SCC ------------------- Carbon steel in acid gas treaters     |
   |   - Polythionic Acid SCC -------- Sensitized SS in refinery turnarounds |
   | Intergranular Corrosion (IGC) --- Cr-carbide precipitation (425-850°C)  |
   | Hydrogen Damage:                                                        |
   |   - Hydrogen Embrittlement ------ High strength steels, loss of ductility|
   |   - Hydrogen Blistering --------- H2 gas traps at internal laminations  |
   |   - HTHA (Nelson Curves) -------- Fe3C + 4H -> CH4 fissuring at > 200°C |
   +-------------------------------------------------------------------------+

Stress Corrosion Cracking (SCC)

SCC requires the simultaneous presence of three interdependent factors: (1) tensile stress (residual welding stress or operating pressure), (2) a susceptible alloy metallurgy, and (3) a specific corrosive chemical environment.

1. Chloride Stress Corrosion Cracking (CSCC):
   • Occurs in standard austenitic stainless steels (304, 304L, 316, 316L) exposed to aqueous chlorides.
   • Critical Temperature Threshold: Rarely occurs below $60^\circ\text{C} \; (140^\circ\text{F})$; risk accelerates exponentially with higher temperature.
   • Morphology: Highly branched, transgranular cleavage cracks ("lightning bolt" pattern).
   • Mitigation: Upgrade to Duplex 2205, Super Duplex, or Nickel Alloy 625/825; or eliminate chlorides/reduce temperature.
2. Caustic Embrittlement (Caustic SCC):
   • Occurs in carbon steels exposed to concentrated sodium hydroxide ($\text{NaOH}$) at elevated temperatures ($> 50 - 80^\circ\text{C}$).
   • Morphology: Intergranular cracking along ferrite grain boundaries.
   • Mitigation: Perform mandatory Post-Weld Heat Treatment (PWHT) (stress-relieving at $600 - 650^\circ\text{C}$ per NACE SP0472), or upgrade to Nickel 200/201.
3. Amine Stress Corrosion Cracking:
   • Occurs in carbon steel alkanolamine gas treating units (MEA, DEA, MDEA) used to remove $\text{CO}_2$ and $\text{H}_2\text{S}$.
   • Mitigation: Strict adherence to API RP 945, mandating full PWHT of all welded piping and vessels regardless of wall thickness.
4. Polythionic Acid SCC (PASCC):
   • Occurs during refinery turnarounds in hydroprocessing reactors fabricated from sensitized austenitic stainless steels. When sulfide scale ($\text{FeS}$) contacts oxygen and liquid water during shutdown, it oxidizes to polythionic acids ($\text{H}_2\text{S}_x\text{O}_6$), causing rapid intergranular cracking.
   • Mitigation: Follow NACE SP0170 (purge equipment with dry nitrogen or circulate a 1–2% soda ash [$\text{Na}_2\text{CO}_3$] neutralization wash before admitting air).

Intergranular Corrosion (IGC) & Sensitization

As introduced in Section 16.1, heating standard austenitic stainless steels (e.g., 304, 316) between $425^\circ\text{C}$ and $850^\circ\text{C}$ ($800^\circ\text{F} - 1500^\circ\text{F}$) causes carbon to rapidly diffuse to grain boundaries, where it reacts with chromium to precipitate chromium carbide ($\text{Cr}_{23}\text{C}_6$). Because chromium diffuses vastly slower than carbon, chromium in the grain matrix adjacent to the boundary is depleted below $12\%$. In an acid electrolyte, this chromium-depleted boundary forms a microscopic active anode coupled to the massive cathodic grain interior, resulting in deep, rapid grain dislodgement ("sugaring" or "knife-line attack").

Hydrogen Damage Mechanisms

• Hydrogen Embrittlement (HE): Atomic hydrogen ($\text{H}^0$) generated during acid pickling, electroplating, or sour service ($\text{H}_2\text{S}$) diffuses into high-strength steel lattices, pinning dislocations and causing brittle fracture under tensile stress.
• Hydrogen Blistering: Atomic hydrogen diffuses through steel and encounters microscopic internal voids or manganese sulfide ($\text{MnS}$) inclusions. There, two hydrogen atoms recombine into molecular hydrogen gas ($2\text{H} \longrightarrow \text{H}_2 \uparrow$). Because molecular $\text{H}_2$ is too large to diffuse out, internal gas pressure builds to thousands of atmospheres, plastically deforming the steel into surface blisters.
• High-Temperature Hydrogen Attack (HTHA):
  • Occurs in carbon and low-alloy steels exposed to high hydrogen partial pressure ($P_{\text{H}_2} > 100\text{ psia}$) at elevated temperatures ($T > 200^\circ\text{C} \; [400^\circ\text{F}]$) in hydrocrackers, hydrotreaters, and ammonia converters.
  • Mechanism: Atomic hydrogen diffuses into steel and reacts with cementite (iron carbide): $$\text{Fe}_3\text{C} + 4\text{H} \longrightarrow 3\text{Fe} + \text{CH}_4 \uparrow$$
  • Methane gas ($\text{CH}_4$) cannot diffuse out through the crystal lattice. Extreme methane pressure nucleates micro-fissures along grain boundaries, causing decarburization, loss of tensile strength, and catastrophic rupture.
  • API RP 941 Nelson Curves: Safe operating limits for process equipment are defined by empirical Nelson Curves, which establish maximum safe temperature and $\text{H}_2$ partial pressure limits for carbon steel, $0.5\text{Mo}$, $1.25\text{Cr}-0.5\text{Mo}$, $2.25\text{Cr}-1\text{Mo}$, and $3\text{Cr}-1\text{Mo}$. Adding carbide-stabilizing elements (Cr, Mo, V) binds carbon into stable carbides (e.g., $\text{Cr}_7\text{C}_3, \text{Mo}_2\text{C}$) that resist methane formation.

---

6. Flow-Induced and Biological Degradation

• Erosion-Corrosion: Acceleration in metal dissolution caused by high fluid velocity, turbulence, or impingement mechanically stripping the protective passive film. Most severe at pipe elbows, tees, orifices, and downstream of control valves. Characterized by directional grooves, waves, or "horseshoe" shaped depressions.
• Cavitation: Occurs in high-speed centrifugal pumps and control valves where local pressure drops below vapor pressure, generating vapor bubbles. When these bubbles enter higher-pressure regions, they violently implode, generating localized micro-jets with shock pressures exceeding $1,000\text{ MPa}$. This micro-hammering destroys passive films and mechanically fatigues metal.
• Microbiologically Influenced Corrosion (MIC): Microorganisms establish metabolic colonies (biofilms) on metal surfaces, creating localized anaerobic micro-environments:
  • Sulfate-Reducing Bacteria (SRB, e.g., Desulfovibrio): Under anaerobic conditions (water tanks, stagnant pipelines), SRBs consume cathodic hydrogen and reduce sulfate ions ($\text{SO}_4^{2-}$) to sulfide ($\text{S}^{2-}$), producing highly corrosive hydrogen sulfide ($\text{H}_2\text{S}$) and precipitating black iron sulfide ($\text{FeS}$) scale.
  • Acid-Producing Bacteria (APB): Secrete organic acids (acetic, butyric) that drive local $\text{pH}$ under the biofilm down to (2 - 3).

---

7. Corrosion Prevention & Mitigation Engineering

   +-------------------------------------------------------------------------+
   |                  Corrosion Prevention Strategies                        |
   +-------------------------------------------------------------------------+
   | Cathodic Protection:                                                    |
   |   - Sacrificial Anodes (SACP) --- Zn, Al, Mg (passive, no power)        |
   |   - Impressed Current (ICCP) ---- DC rectifier, MMO/Pt anodes, large A  |
   | Chemical Inhibitors:                                                    |
   |   - Anodic (Passivating) -------- DANGEROUS if underdosed (Pitting!)    |
   |   - Cathodic -------------------- Safe (suppresses reduction rate)      |
   |   - Mixed / Film-Forming -------- Organic amines, hydrophobic film      |
   | Protective Coatings & Linings --- Epoxies, PTFE, rubber, glass          |
   +-------------------------------------------------------------------------+

Cathodic Protection (CP)

Cathodic protection polarizes the metal structure into the thermodynamic Immunity Zone of the Pourbaix diagram (potential $E < -0.850\text{ V}$ versus a Copper/Copper Sulfate Electrode [CSE] for carbon steel in soil/water).

Chemical Corrosion Inhibitors

Chemical inhibitors are substances added in small concentrations ($10 - 500\text{ ppm}$) to process streams to suppress corrosion rates:

1. Anodic Inhibitors (Passivators): Oxidizing anions (nitrites $[\text{NO}_2^-]$, chromates $[\text{CrO}_4^{2-}]$, orthophosphates) that shift the corrosion potential positive into the passive region, strengthening the oxide barrier.

   Warning

   High-Risk PE Exam Trap: Anodic inhibitors are dangerous inhibitors! If an anodic inhibitor is underdosed, passivity is established over most of the surface but fails at small bare spots, creating a small active anode coupled to a massive passivated cathode. This causes severe, accelerated localized pitting that perforates equipment faster than if no inhibitor were added at all!

2. Cathodic Inhibitors: Substances that precipitate insoluble protective films at cathodic sites where alkaline $\text{OH}^-$ ions are generated (e.g., zinc salts $[\text{Zn}^{2+}]$, calcium bicarbonate, polyphosphates). They are safe inhibitors because underdosing never accelerates localized attack; it simply provides partial uniform protection.
3. Mixed / Organic Film-Forming Inhibitors: Long-chain aliphatic amines or imidazolines containing polar nitrogen groups that adsorb onto metal surfaces, with long hydrophobic hydrocarbon tails projecting outward into the fluid to repel water, acids, and ions.

---

8. Summary Comparison Tables

Table 1: Major Degradation Mechanisms, Susceptible Alloys, and Solutions

---

9. Comprehensive Worked Numerical Example

Problem Statement

A refinery sour water stripper overhead condenser experiences accelerated degradation. Solve the following three engineering evaluations:

1. Corrosion Penetration Rate & Pipeline Remaining Life: An ASTM A106 Grade B carbon steel corrosion coupon ($\rho = 7.85\text{ g/cm}^3$) is installed in the overhead vapor line. The coupon has outer dimensions of $2.00\text{ in} \times 1.00\text{ in} \times 0.125\text{ in}$ with a central mounting hole of diameter $d = 0.250\text{ in}$. After $2,160\text{ hours}$ ($90.0\text{ days}$) of steady service, the coupon is removed, cleaned of scale, and reweighed. The initial weight was $W_1 = 31.850\text{ g}$ and the final cleaned weight is $W_2 = 29.425\text{ g}$. Determine the total exposed surface area (A) in $\text{in}^2$, the mass loss $\Delta W$ in $\text{mg}$, the Corrosion Penetration Rate ($\text{CPR}$) in mils per year ($\text{mpy}$), and $\text{CPR}$ in $\text{mm/yr}$. If the overhead carbon steel transfer line has a current ultrasonic measured wall thickness of $0.310\text{ in}$ and an ASME BPVC minimum allowable retirement thickness of $t_{\text{min}} = 0.200\text{ in}$, calculate the remaining operational lifetime of the line in years assuming this corrosion rate continues.
2. Galvanic Area Ratio Acceleration: The condenser features titanium tubes ($A_C = 20.0\text{ ft}^2$) rolled into a carbon steel channel shell. A small carbon steel weld fillet ($A_A = 0.50\text{ ft}^2$, $\rho = 7.85\text{ g/cm}^3$, $\text{EW} = 27.92\text{ g/equivalent}$) is exposed to aerated cooling water. The cathodic oxygen reduction current density on the titanium surface is $i_C = 15.0\;\mu\text{A/cm}^2$. Assuming the couple is under complete cathodic control, calculate the accelerated anodic current density $i_A$ on the carbon steel weld in $\mu\text{A/cm}^2$, and the resulting galvanic penetration rate in $\text{mpy}$ and $\text{mm/yr}$.
3. PREN Evaluation for Cooling Water Alloy Selection: Brackish estuarine cooling water containing $15,000\text{ ppm}$ chlorides at $38^\circ\text{C}$ is used. Compute the PREN for Type 316L SS (17.0% Cr, 2.1% Mo, 0.04% N), Duplex 2205 (22.0% Cr, 3.1% Mo, 0.18% N), and Super Duplex 2507 (25.0% Cr, 4.0% Mo, 0.28% N). Determine which alloy satisfies the marine threshold of $\text{PREN} \ge 40$.

---

Step 1: Corrosion Coupon CPR & Remaining Life

First calculate the exposed surface area (A) of the rectangular coupon with mounting hole:

• Two main rectangular faces: $2 \times (2.00 \times 1.00) = 4.000\text{ in}^2$.
• Two long edge faces: $2 \times (2.00 \times 0.125) = 0.500\text{ in}^2$.
• Two short edge faces: $2 \times (1.00 \times 0.125) = 0.250\text{ in}^2$.
• Mounting hole correction: $$\text{Area subtracted from two faces} = -2 \times \left( \frac{\pi}{4} d^2 \right) = -2 \times \left( \frac{\pi}{4} (0.250)^2 \right) = -0.09817\text{ in}^2$$ $$\text{Cylindrical inside hole area added} = +\pi d t_h = \pi (0.250) (0.125) = +0.09817\text{ in}^2$$ (Notice: The hole face area subtracted exactly equals the cylindrical bore area added!)

Total exposed surface area:

$$A = 4.000 + 0.500 + 0.250 = \mathbf{4.750\text{ in}^2}$$

Compute mass loss:

$$\Delta W = W_1 - W_2 = 31.850\text{ g} - 29.425\text{ g} = 2.425\text{ g} = \mathbf{2,425.0\text{ mg}}$$

Compute Corrosion Penetration Rate in $\text{mpy}$ using (K = 534):

$$\text{CPR} = \frac{K \Delta W}{\rho A t} = \frac{534 \times 2425.0\text{ mg}}{(7.85\text{ g/cm}^3) \times (4.750\text{ in}^2) \times (2160\text{ hr})}$$ $$\text{Numerator} = 534 \times 2425.0 = 1,294,950$$ $$\text{Denominator} = 7.85 \times 4.750 \times 2160 = 80,541$$ $$\text{CPR} = \frac{1,294,950}{80,541} = \mathbf{16.078\text{ mpy}} \approx 16.1\text{ mpy}$$

Convert to $\text{mm/yr}$:

$$\text{CPR} = 16.078\text{ mpy} \times 0.0254\text{ mm/(mpy)} = \mathbf{0.4084\text{ mm/yr}}$$

Compute remaining allowable metal loss before reaching retirement thickness:

$$\Delta t_{\text{allowable}} = t_{\text{actual}} - t_{\text{min}} = 0.310\text{ in} - 0.200\text{ in} = 0.110\text{ in} = 110.0\text{ mils}$$

Calculate remaining service life:

$$\text{Remaining Life} = \frac{\Delta t_{\text{allowable}}}{\text{CPR}} = \frac{110.0\text{ mils}}{16.078\text{ mpy}} = \mathbf{6.84\text{ years}}$$

---

Step 2: Galvanic Acceleration on Carbon Steel Weld

Compute the cathode-to-anode area ratio:

$$\frac{A_C}{A_A} = \frac{20.0\text{ ft}^2}{0.50\text{ ft}^2} = 40.0$$

Calculate accelerated anodic current density on the carbon steel weld:

$$\ni_A = i_C \times \left( \frac{A_C}{A_A} \right) = 15.0\;\mu\text{A/cm}^2 \times 40.0 = \mathbf{600.0\;\mu\text{A/cm}^2}$$

Compute accelerated penetration rate via Faraday's equation:

$$\text{CPR}_A = \frac{0.129 \times i_A \times \text{EW}}{\rho} = \frac{0.129 \times 600.0 \times 27.92}{7.85}$$ $$\text{Numerator} = 0.129 \times 600.0 \times 27.92 = 2,161.01$$ $$\text{CPR}_A = \frac{2,161.01}{7.85} = \mathbf{275.3\text{ mpy}}$$ $$\text{CPR}_A\text{ in mm/yr} = 275.3 \times 0.0254 = \mathbf{6.99\text{ mm/yr}}$$

(Critical finding: The galvanic couple accelerates the corrosion rate from a tolerable $6.9\text{ mpy}$ baseline to a catastrophic $275.3\text{ mpy}$, which would perforate a $0.375\text{ in}$ shell in under $1.4\text{ years}$).

---

Step 3: PREN Evaluation for Warm Estuarine Brine

Calculate PREN using $\text{PREN} = \% \text{Cr} + 3.3(\% \text{Mo}) + 16(\% \text{N})$:

• Type 316L SS: $$\text{PREN} = 17.0 + 3.3(2.1) + 16(0.04) = 17.0 + 6.93 + 0.64 = \mathbf{24.57}$$
• Duplex 2205: $$\text{PREN} = 22.0 + 3.3(3.1) + 16(0.18) = 22.0 + 10.23 + 2.88 = \mathbf{35.11}$$
• Super Duplex 2507: $$\text{PREN} = 25.0 + 3.3(4.0) + 16(0.28) = 25.0 + 13.20 + 4.48 = \mathbf{42.68}$$

Conclusion: Only Super Duplex 2507 ($\text{PREN} = 42.68 \ge 40$) satisfies the threshold required to eliminate pitting and crevice attack in chlorinated $15,000\text{ ppm}$ brackish water at $38^\circ\text{C}$.

---

10. Critical PE Exam Traps & Pitfalls