Download CORROSION AND SURFACE CHEMISTRY OF METALS by Dieter Landolt PDF

By Dieter Landolt

Delivering a gently built and entire assessment of the corrosion chemistry of steel fabrics, this ebook covers the valuable tools of corrosion prevention. It encompasses a systematic examine of the actual chemistry of the outside supported via cutting-edge research tools. the writer builds a systematic origin by way of constructing thermodynamics and kinetics of electrode-electrolyte interplay and different floor procedures. this permits him to research and derive the types which are utilized in the examine of corrosion for metals and their alloys, together with electrochemical assault, high-temperature oxidation, passivity, atmospheric corrosion, in addition to the jobs of damage and pressure.

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A well–known example concerns heating systems; copper ions liberated by corrosion of a hot–water heater made of copper react downstream with the wall of a zinc–coated steel pipe. The microscopic deposits of metallic copper form a galvanic cell with the wall and thus accelerate locally the rate of corrosion. 2 Protection potential The Nernst equation describes the equilibrium condition of an electrode. 70) The copper will not dissolve unless the potential of the electrode exceeds this value. In practice, a metal being part of a structure or a machine is rarely in contact with a solution of its own ions, at a uniform and known concentration.

86) using an inert platinum electrode. The value depends on the relative concentration of the Fe3+ and Fe 2+ ions. 13 shows schematically the difference in reaction when iron or platinum electrodes are employed. 86). The potential of a half–cell reaction between dissolved species is called the oxidation–reduction potential or redox potential. It describes the oxidative strength of a solution. 88) sets the redox potential of an aqueous solution containing dissolved oxygen. 23 V The very high standard potential indicates that oxygen is a powerful oxidizing agent.

Kortu¨m, Lehrbuch der Elektrochemie, 5th edition, Verlag Chemie, Weinheim (1972) p. 617. [4] R. A. Robinson, R. H. Stokes, Electrolyte Solutions, 2nd edition, Butterworths, London (1970) pp. 74 and 230. [5] R. A. Robinson, R. H. Stokes, Electrolyte Solutions, 2nd edition, Butterworths, London (1970) pp. 491–503. [6] A. J. Bard, R. Parsons, J. Jordan, Standard Potentials in Aqueous Solution, Marcel Dekker Inc, New York (1985) pp. 1–834. [7] M. Pourbaix, Atlas of Electrochemical Equilibria in Aqueous Solutions, 2nd edition, NACE, Houston Texas (1974) pp.

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