CHEM 122 Lecture Notes - Lecture 20: Galvanic Cell, Nernst Equation, Silver Iodide

• School: Simon Fraser University
• Department: Chemistry
• Course: CHEM 122
• Professor: Garry Mund

Document Summary

Chem 122: general chemistry ii - lecture 20: electrochemistry iii (11. 4 cont"d and 11. 7) The nernst equation can be used to calculate electrode potentials (for individual electrodes) under nonstandard conditions. Calculate the reduction potential of cu2+ in the following half-cell: Cu2+ + 2e- cu where [cu2+] is 3m. = 0. 354 v for cu2+ at 3m concentration. Another use of galvanic cells is to measure low ion concentrations in solutions, concentrations that would otherwise be too difficult to detect using other means. The particular galvanic cell that is used to do this is a concentration cell cells that make use of the same metal electrodes but with different ion concentrations in both anode and cathode compartment. And the measured cell potential is 0. 42 v. Because the ag+ concentration is different in the two compartments, the actual half-cell potentials are different, concentrations are the same. e - flow will occur until the.