Introduction to the High Temperature Oxidation of Metals by Neil Birks, Gerald H. Meier, Frederick S. Pettit

By Neil Birks, Gerald H. Meier, Frederick S. Pettit

A simple remedy describing the oxidation methods of metals and alloys at increased temperatures. This 2006 moment variation keeps the basic thought yet accommodates advances made in figuring out degradation phenomena. the 1st part offers an authoritative advent to the elemental ideas, masking thermodynamics and mechanisms of hot temperature corrosion of metals and alloys. The latter part extends the dialogue to oxidation tactics in advanced platforms, from reactions in combined environments to protecting strategies, together with coatings and surroundings keep watch over. The authors offer a logical and professional therapy of the topic, generating a revised variation that would be a complete consultant to fabric scientists and engineers requiring an knowing of this hassle-free method.

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R. Stull and G. C. Sinke, Thermodynamic Properites of the Elements. Advances in Chemistry, Monograph 18, Washington DC, American Chemical Society, 1956. 10. K. C. Mills, Thermodynamic Data for Inorganic Sulphides, Selenides, and Tellurides, London, Butterworth, 1974. 11. M. O. Dayhoff, E. R. Lippincott, R. V. Eck, and G. Nagarajan, Thermodynamic equilibrium in prebiological atmospheres of C, H, O, P, S, and Cl. NASA SP-3040, Washington, DC, 1964. 12. I. Barin, Thermochemical Data of Pure Substances, Weinheim, VCH Verlagsgesellschaft, 1993.

O (ad) = O− (chem) + h. ; (c) ionization: O− (chem) = OO + VN + h. Overall reaction 12 OO + VN + Zh. 15) represents the only mechanism by which the defects form and that these obey Henry’s law: 1/2 Ch2· CVNi = K 15 pO2 . 17) is obtained: 1/6 Ch· = const. pO2 . 17) The electrical conductivity is expected to vary proportionally to the electron-hole concentration and so with the sixth root of the oxygen partial pressure. , in NiO a Ni3+ may be permanently attached to the Ni vacancy. 18): 1 O2 = OO + h· + VNi .

5. The equilibrium oxygen partial pressure may be calculated from either the CO/CO2 or H2 /H2 O equilibria. 0 × 10−18 atm. 1425aC = . 009. The possibility of the formation of other species, such as CH4 , has been ignored in the above calculation because their concentrations would be extremely small. When the gas mixture contains more components, or if formation of additional species must be considered, the calculations become more complex, involving more equilibrium constants and more complicated mass balances.

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