1. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.1 An example of a simple electrochemical cell is the lead-acid cell, here shown at rest.

2. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.2 In its galvanic mode the lead-acid cell provides energy to a “load”. The cell voltage is less than its equilibrium value.

3. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.3 In its electrolytic mode the Gibbs energy of the lead-acid cell is increased at the expense of external electrical energy. The cell voltage now exceeds its equilibrium value.

4. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.4 In this polarization curve for a lead-acid cell, the colored segments correspond to operation in the galvanic and electrolytic modes.

5. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.5 (a) a conventional electrochemical cell and (b) the complementary, but impractical, arrangement of conductors.

6. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.6 The Daniell cell incorporates a porous diaphragm.

7. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.7 This concentration cell uses a KC1 salt bridge to prevent the transfer of Cu 2+ ions between the half-cells. The concentration c L of CuCl 2 in the left-hand half-cell exceeds that, c R in the right-hand half-cell.

8. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.8 A bipolar electrode is an alternative to a salt bridge in avoiding transference in a concentration cell.

9. Electrochemical Science and Technology: Fundamentals and Applications, Keith B. Oldham, Jan C. Myland and Alan M. Bond. © 2011 John Wiley & Sons, Ltd. Published 2011 by John Wiley & Sons, Ltd. Figure 3.9 The zirconia-based oxygen-concentration cell responds to the ratio of the partial pressures of oxygen at its two electrodes.