By Allen J. Bard, Martin Stratmann, Gerald S. Frankel
Unrivalled in its breadth and intensity, this 11-volume encyclopedia presents either a simple advent to all themes regarding glossy electrochemistry in addition to a finished evaluate of the topic. all through, the emphasis is in quick access to info, with each subject handled at an introductory, medium and complex point. This first class reference paintings is edited and written by means of well known scientists, protecting every thing from basic learn to parts of software. Alan Bard, skilled editor of the magazine of the yank Chemical Society, is among the most famed specialists in electrochemistry and one of many editors-in-chief.
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Additional resources for Encyclopedia of Electrochemistry, Corrosion and Oxide Films
For small E − Ecorr = dE: exp E − Ecorr b dE ∼ =1+ b (45) For small differences in potential from Ecorr , dE, the measured net currents will be small, di. Substituting into Eq. (41): di = icorr dE 1 1 + ba bc (46) Polarization resistance, RP , can be deﬁned as the slope of the linear polarization curve at the corrosion potential: RP ≡ dE di (47) E=Ecorr Note that the units of RP are cm−2 . Rearranging Eq. 3RP (48) This is the Stern–Geary equation, which shows that the corrosion rate can be determined by a small polarization from the corrosion potential, unlike Tafel extrapolation, which requires large potential changes from the corrosion potential.
34) can be written in terms of current density, i = I /A: ic = 0 (35) + e− → H+ 2 1/2 H M→ M n+ +n e− The total oxidation and reduction current densities will be equal at the point at which the anodic line for the metal dissolution reaction intersects the cathodic line for hydrogen evolution. The potential at which these lines intersect is the corrosion potential. The rate of the anodic reaction at the corrosion potential is the corrosion rate (corrosion current density). The corrosion potential always takes a value between the reversible potentials for the two partial reactions.
8, which is the net current as a function of potential for a metal corroding in an acid accompanied by hydrogen evolution, looks like the one in Fig. 5, which represents the forward and reverse directions of a single reaction. Similarly, an equation similar in form to the Butler–Volmer equation can be derived to describe the curve in Fig. 8. One form of the Tafel equation is: i = i0 exp E − Earev ba (37) |ic | = i0,c exp Ecrev − E |bc | (38) The net current is then given by: inet = ia − |ic | = i0,a exp → M 2 1/ H2 → − M + e M + ne + n+ n e− → + n + 2 1/ H2 → H + − e i0, H2 /H+ i0, M/M+ E rev M/M+ Ecorr E rev H2 /H+ E Relationship of measured polarization curve to the Evans diagram for a corroding active metal in an acid.