Chapter 18 Lecture Problems


Standard Cell Potential

  1. Zn | Zn2+ (1 M) || Fe2+ (1 M) | Fe
    1. Draw cell
    2. Oxidation, Anode
    3. Reduction, Cathode
    4. Use Reduction potentials: Ecell = Ecathode - Eanode
    5. Solutions

  2. Work in groups
    1. Fe | Fe2+ (1 M) || H1+ (1 M), H2 (1 atm) | Pt
    2. Pt | H1+ (1 M), H2 (1 atm) ||Cu2+ (1 M) | Cu
    3. Fe | Fe2+ (1 M) || Cu2+ (1 M) | Cu
    4. Cu | Cu2+ (1 M) || Fe2+ (1 M) | Fe

Cell Potential, not standard conditions

[Zn2+] [Fe2+] Ecell (Volt)
1.00 1.00 0.3538
1.00 2.00 0.3627
2.00 1.00 0.3449
0.100 0.100 0.3538
1.00 0.010 0.2946
0.010 1.00 0.41296

  • Calculate concentration ratio (Q) based upon cell potential for the cell

    Zn|Zn2+ || Fe2+ | Fe

    1. Ecell = 0.3538 V
    2. Ecell = 0.3530 V
    3. Ecell = 0.3400 V
    4. Ecell = 0.3550 V
    5. Ecell = 0.3600 V

  • Solutions
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