Presentation on theme: "Chapter 22 – Corrosion and Wear"— Presentation transcript:
1Chapter 22 – Corrosion and Wear The Science and Engineering of Materials, 4th ed Donald R. Askeland – Pradeep P. PhuléChapter 22 – Corrosion and Wear
2Objectives of Chapter 22To introduce the principles and mechanisms by which corrosion and wear occur under different conditions. This includes the aqueous corrosion of metals, the oxidation of metals, the corrosion of ceramics, and the degradation of polymers.To give summary of different technologies that are used to prevent or minimize corrosion and associated problems.
3Chapter Outline 22.1 Chemical Corrosion 22.2 Electrochemical Corrosion 22.3 The Electrode Potential in Electrochemical Cells22.4 The Corrosion Current and Polarization22.5 Types of Electrochemical Corrosion22.6 Protection Against Electrochemical Corrosion22.7 Microbial Degradation and Biodegradable Polymers22.8 Oxidation and Other Gas Reactions22.9 Wear and Erosion
4Section 22.1 Chemical Corrosion Chemical corrosion - Removal of atoms from a material by virtue of the solubility or chemical reaction between the material and the surrounding liquid.Dezincification - A special chemical corrosion process by which both zinc and copper atoms are removed from brass, but the copper is replated back onto the metal.Graphitic corrosion - A special chemical corrosion process by which iron is leached from cast iron, leaving behind a weak, spongy mass of graphite.
7Section 22.2 Electrochemical Corrosion Electrochemical corrosion - Corrosion produced by the development of a current in an electrochemical cell that removes ions from the material.Electrochemical cell - A cell in which electrons and ions can flow by separate paths between two materials, producing a current which, in turn, leads to corrosion or plating.Oxidation reaction - The anode reaction by which electrons are given up to the electrochemical cell.Reduction reaction - The cathode reaction by which electrons are accepted from the electrochemical cell.
10Section 22.3 The Electrode Potential in Electrochemical Cells Electrode potential - Related to the tendency of a material to corrode. The potential is the voltage produced between the material and a standard electrode.emf series - The arrangement of elements according to their electrode potential, or their tendency to corrode.Nernst equation - The relationship that describes the effect of electrolyte concentration on the electrode potential in an electrochemical cell.Faraday’s equation - The relationship that describes the rate at which corrosion or plating occurs in an electrochemical cell.
13Example 22.1 Half-Cell Potential for Copper Suppose 1 g of copper as Cu2+ is dissolved in 1000 g of water to produce an electrolyte. Calculate the electrode potential of the copper half-cell in this electrolyte.Example 22.1 SOLUTIONFrom chemistry, we know that a standard 1-M solution of Cu2+ is obtained when we add 1 mol of Cu2+ (an amount equal to the atomic mass of copper) to 1000 g of water. The atomic mass of copper is g/mol. The concentration of the solution when only 1 g of copper is added must be:From the Nernst equation, with n = 2 and E0 = V:
14Example 22.2 Design of a Copper Plating Process Design a process to electroplate a 0.1-cm-thick layer of copper onto a 1 cm 1 cm cathode surface.Example 22.2 SOLUTIONIn order for us to produce a 0.1-cm-thick layer on a 1 cm2 surface area, the weight of copper must be:From Faraday’s equation, where MCu = 63:54 g/mol and n = 2:
15Example 22.2 SOLUTIONTherefore, we might use several different combinations of current and time to produce the copper plate:Our choice of the exact combination of current and time might be made on the basis of the rate of production and quality of the copper plate.A current of ~ 1 A and a time of ~ 45 minutes are not uncommon in electroplating operations.
16Example 22.3 Corrosion of Iron An iron container 10 cm 10 cm at its base is filled to a height of 20 cm with a corrosive liquid. A current is produced as a result of an electrolytic cell, and after 4 weeks, the container has decreased in weight by 70 g. Calculate (1) the current and (2) the current density involved in the corrosion of the iron.Example 22.3 SOLUTION1. The total exposure time is:From Faraday’s equation, using n = 2 and M = g/mol:
17Example 22.3 SOLUTION2. The total surface area of iron in contact with the corrosive liquid and the current density are:
18Example 22.4 Copper-Zinc Corrosion Cell Suppose that in a corrosion cell composed of copper and zinc, the current density at the copper cathode is 0.05 A/cm2. The area of both the copper and zinc electrodes is 100 cm2. Calculate (1) the corrosion current, (2) the current density at the zinc anode, and (3) the zinc loss per hour.Example 22.4 SOLUTION1. The corrosion current is:2. The current in the cell is the same everywhere. Thus:
19Example 22.4 SOLUTION3. The atomic mass of zinc is g/mol. From Faraday’s equation:
20Section 22.4 The Corrosion Current and Polarization Polarization - Changing the voltage between the anode and cathode to reduce the rate of corrosion.Activation polarization is related to the energy required to cause the anode or cathode reactionConcentration polarization is related to changes in the composition of the electrolyteResistance polarization is related to the electrical resistivity of the electrolyte.
21Section 22.5 Types of Electrochemical Corrosion Intergranular corrosion - Corrosion at grain boundaries because grain boundary segregation or precipitation produces local galvanic cells.Stress corrosion - Deterioration of a material in which an applied stress accelerates the rate of corrosion.Oxygen starvation - In the concentration cell, low-oxygen regions of the electrolyte cause the underlying material to behave as the anode and to corrode.Crevice corrosion - A special concentration cell in which corrosion occurs in crevices because of the low concentration of oxygen.
23Example 22.5 Corrosion of a Soldered Brass Fitting A brass fitting used in a marine application is joined by soldering with lead-tin solder. Will the brass or the solder corrode?Example 22.5 SOLUTIONFrom the galvanic series, we find that all of the copper-based alloys are more cathodic than a 50% Pb-50% Sn solder. Thus, the solder is the anode and corrodes. In a similar manner, the corrosion of solder can contaminate water in freshwater plumbing systems with lead.
27Example 22.6 Corrosion of Cold-Drawn Steel A cold-drawn steel wire is formed into a nail by additional deformation, producing the point at one end and the head at the other. Where will the most severe corrosion of the nail occur?Example 22.6 SOLUTIONSince the head and point have been cold-worked an additional amount compared with the shank of the nail, the head and point serve as anodes and corrode most rapidly.
29Example 22.7 Corrosion of Crimped Steel Two pieces of steel are joined mechanically by crimping the edges. Why would this be a bad idea if the steel is then exposed to water? If the water contains salt, would corrosion be affected?Example 22.7 SOLUTIONBy crimping the steel edges, we produce a crevice. The region in the crevice is exposed to less air and moisture, so it behaves as the anode in a concentration cell. The steel in the crevice corrodes.Salt in the water increases the conductivity of the water, permitting electrical charge to be transferred at a more rapid rate. This causes a higher current density and, thus, faster corrosion due to less resistance polarization.
31Section 22.6 Protection Against Electrochemical Corrosion Inhibitors - Additions to the electrolyte that preferentially migrate to the anode or cathode, cause polarization, and reduce the rate of corrosion.Sacrificial anode - Cathodic protection by which a more anodic material is connected electrically to the material to be protected. The anode corrodes to protect the desired material.Passivation - Producing strong anodic polarization by causing a protective coating to form on the anode surface and to thereby interrupt the electric circuit.
32Example 22.8 Effect of Areas on Corrosion Rate for Copper-Zinc Couple Consider a copper-zinc corrosion couple. If the current density at the copper cathode is 0.05 A/cm2, calculate the weight loss of zinc per hour if (1) the copper cathode area is 100 cm2 and the zinc anode area is 1 cm2 and (2) the copper cathode area is 1 cm2 and the zinc anode area is 100 cm2.
37Figure (a) Intergranular corrosion takes place in austenitic stainless steel. (b) Slow cooling permits chromium carbides to precipitate at grain boundaries. (c) A quench anneal to dissolve the carbides may prevent intergranular corrosion.
38Example 22.9 Design of a Corrosion Protection System Steel troughs are located in a field to provide drinking water for a herd of cattle. The troughs frequently rust through and must be replaced. Design a system to prevent or delay this problem.Example 22.9 SOLUTIONWe might, for example, fabricate the trough using stainless steel or aluminum. Either would provide better corrosion resistance than the plain carbon steel, but both are considerably more expensive than the current material.We might suggest using cathodic protection; a small magnesium anode could be attached to the inside of the trough. The anode corrodes sacrificially and prevents corrosion of the steel.
39Example 22.9 SOLUTION (Continued) Another approach would be to protect the steel trough using a suitable coating. Painting the steel (that is, introducing a protective polymer coating) and, using a tin-plated steel, provides protection as long as the coating is not disrupted.The most likely approach is to use a galvanized steel, taking advantage of the protective coating and the sacrificial behavior of the zinc. Corrosion is very slow due to the large anode area, even if the coating is disrupted. Furthermore, the galvanized steel is relatively inexpensive, readily available, and does not require frequent inspection.
40Example 22.10 Design of a Stainless-Steel Weldment A piping system used to transport a corrosive liquid is fabricated from 304 stainless steel. Welding of the pipes is required to assemble the system. Unfortunately, corrosion occurs and the corrosive liquid leaks from the pipes near the weld. Identify the problem and design a system to prevent corrosion in the future.
43Example SOLUTIONA portion of the pipe in the HAZ heats into the sensitization temperature range, permitting chromium carbides to precipitate. If the cooling rate of the weld is very slow, the fusion zone and other areas of the heat-affected zone may also be affected. Sensitization of the weld area, therefore, is the likely reason for corrosion of the pipe in the region of the weld.We might use a welding process that provides very rapid rates of heat input, causing the weld to heat and cool very quickly.We might heat treat the assembly after the weld is made. By performing a quench anneal, any precipitated carbides are re-dissolved during the anneal and do not re-form during quenching.Perhaps our best design is to use a stainless steel that is not subject to sensitization.
44Section 22.7 Microbial Degradation and Biodegradable Polymers Simple polymers (such as polyethylene, polypropylene, and polystyrene), high-molecular-weight polymers, crystalline polymers, and thermosets are relatively immune to attack.However, certain polymers—including polyesters, polyurethanes, cellulosics, and plasticized polyvinyl chloride (which contains additives that reduce the degree of polymerization)—are particularly vulnerable to microbial degradation.
45Section 22.8 Oxidation and Other Gas Reactions Oxidation - Reaction of a metal with oxygen to produce a metallic oxide. This normally occurs most rapidly at high temperatures.Pilling-Bedworth ratio - Describes the type of oxide film that forms on a metal surface during oxidation.
47Example 22.11 Chromium-Based Steel Alloys Explain why we should not add alloying elements such as chromium to pig iron before the pig iron is converted to steel in a basic oxygen furnace at 1700oC.Example SOLUTIONIn a basic oxygen furnace, we lower the carbon content of the metal from about 4% to much less than 1% by blowing pure oxygen through the molten metal. If chromium were already present before the steel making began, chromium would oxidize before the carbon (Figure 22.16), since chromium oxide has a lower free energy of formation (or is more stable) than carbon dioxide (CO2). Thus, any expensive chromium added would be lost before the carbon was removed from the pig iron.
49Example 22.12 Pilling-Bedworth Ratio The density of aluminum is 2.7 g/cm3 and that of Al2O3 is about 4 g/cm3. Describe the characteristics of the aluminum-oxide film. Compare with the oxide film that forms on tungsten. The density of tungsten is g/cm3 and that of WO3 is 7.3 g/cm3.Example SOLUTIONFor 2Al + 3/2O2 Al2O3, the molecular weight of Al2O3 is and that of aluminum is
50Example SOLUTIONFor tungsten, W+ 3/2O2 WO3. The molecular weight of WO3 is and that of tungsten is :Since P-B ~ 1 for aluminum, the Al2O3 film is nonporous and adherent, providing protection to the underlying aluminum. However, P-B > 2 for tungsten, so the WO3 should be nonadherent and nonprotective.
51Example 22.13 Parabolic Oxidation Curve for Nickel At 1000oC, pure nickel follows a parabolic oxidation curve given by the constant k = 3.9 cm2/s in an oxygen atmosphere. If this relationship is not affected by the thickness of the oxide .lm, calculate the time required for a 0.1-cm nickel sheet to oxidize completely.Example SOLUTIONAssuming that the sheet oxidizes from both sides:
52Section 22.9 Wear and Erosion Adhesive wear - Removal of material from surfaces of moving equipment by momentary local bonding, then bond fracture, at the surfaces.Abrasive wear - Removal of material from surfaces by the cutting action of particles.Cavitation - Erosion of a material surface by the pressures produced when a gas bubble collapses within a moving liquid.Liquid impingement - Erosion of a material caused by the impact of liquid droplets carried by a gas stream.