Initially, each of the half-cells in Figure 19-21 contained a 100.0-mL sample of solution with an ion concentration of 1.000 M. The cell was operated as an electrolytic cell, with copper as the anode and zinc as the cathode. A current of 0.500 A was used. Assume that the only electrode reactions occurring were those involving Cu/Cu²⁺ and Zn/Zn²⁺. Electrolysis was stopped after 10.00 h, and the cell was allowed to function as a voltaic cell. What was E_cell at that point?

Figure 19-21

Transcribed Image Text:

Iron Fel 2e Fe 2e- Cu Hom Cu Film of water Fe²+ Fe2+ O₂ + 2 H₂O 4 OH (a) Copper-plated iron Iron 4 e Film of water Zn→→→ Zn²+ 2 e www 0₂ + 2 H₂O 4 OH 2e Zn Zn²+ (b) Galvanized iron