By Joseph Wang(auth.)
Chapter 1 basic ideas (pages 1–27):
Chapter 2 learn of Electrode Reactions (pages 28–59):
Chapter three Controlled?Potential innovations (pages 60–99):
Chapter four functional issues (pages 100–139):
Chapter five Potentiometry (pages 140–170):
Chapter 6 Electrochemical Sensors (pages 171–202):
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Extra info for Analytical Electochemistry, Second Edition
D. Mohilner, Electroanal. , 1, 241 (1966). 9. O'M. A. Devanathan, and K. Muller, Proc. R. , 55, A274 (1963). 10. R. Parsons, J. Electrochem. , 127, 176C (1980). 11. B. Mark, Analyst 115, 667 (1990). 12. M. Bond, I. Heritage, and M. Briggs, Langmuir, 1, 110 (1985). Questions 1. Show or draw the concentration pro®le/gradient near the electrode surface during a linear scan voltammetric experiment in stirred a solution. ) Show also the resulting voltammogram, along with points for each concentration gradient (in a manner analogous to Figure 1-4).
The dotted line in Figure 1-10 displays such a change for the case of a positive E. Under this z condition the barrier for reduction, DGcz , is larger than DGc;0 . A careful study of the new curve reveals that only a fraction (a) of the energy shift f is actually used to increase the activation energy barrier, and hence to accelerate the rate of the reaction. Based on the symmetry of the two potential curves, this fraction (the transfer coef®cient) can range from zero to unity. 8. The term a is thus a measure of the symmetry of the activation energy barrier.
Show or draw the concentration pro®le/gradient near the electrode surface during a linear scan voltammetric experiment in stirred a solution. ) Show also the resulting voltammogram, along with points for each concentration gradient (in a manner analogous to Figure 1-4). 2. Describe and draw clearly the structure of the electrical double layer (with its Questions 27 several distinct parts). 3. Use the activated complex theory for explaining clearly how the applied potential affects the rate constant of an electron-transfer reaction.