Transcription of III. Reaction Kinetics - MIT OpenCourseWare
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III. Reaction Kinetics - MIT OpenCourseWare
III. Reaction Kinetics Lecture 13: Butler-Volmer equation Notes by ChangHoon Lim (and MZB). 1. Interfacial Equilibrium At lecture 11, the Reaction rate R for the general Faradaic half-cell Reaction was derived. where =Reduced state =Oxidized state Here si is the stochiometric coefficient of species i (positive for reduced state and negative for oxidized state), Ri(Oi) is a symbol for chemical formula and Zi is the charge number of species i. where , , = electrode potential- solution potential, and is symmetry factor (transfer coefficient). [Note]. The ratio of anode Reaction rate to cathode Reaction rate does not depend on or any properties of the transition state. In equilibrium, the net Reaction rate R is zero. That is, where This is the Nernst equation. And, is a kinetic definition of the standard potential, related to microscopic Reaction rates. 1. Lecture 13: Butler-Volmer equation (2011) Bazant 2. Activation Overpotential In electrochemistry, it is more common to use (activation) overpotential rather than.
Lecture 13: Butler Volmer equation 10.626 (2011) Bazant 2-Leading order approximation within which current is linear to overpotential, , R act (>0) is the constant resistance of the Faradaic reaction. Activation overpotential is positive at
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