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PRE-AP CHEMISTRY ELECTROCHEMISTRY WORKSHEET

1. Using the table of standard reduction potentials, arrange the following substances in decreasing order of ability as reducing agents: Al, Co, Ni, Ag, H2, Na. . Oxidation potentials:Al =1.66, Co = 0.28, Ni = 0.25, Ag = -0.80H2 = 0, Na = 2.71Na, Al, Co, Ni, H2, Ag. 2. Using the table of

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PRE-AP CHEMISTRY ELECTROCHEMISTRY WORKSHEET

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    1. PRE-AP CHEMISTRY ELECTROCHEMISTRY WORKSHEET

    2. 1. Using the table of standard reduction potentials, arrange the following substances in decreasing order of ability as reducing agents: Al, Co, Ni, Ag, H2, Na. Oxidation potentials: Al =1.66, Co = 0.28, Ni = 0.25, Ag = -0.80 H2 = 0, Na = 2.71 Na, Al, Co, Ni, H2, Ag

    3. 2. Using the table of standard reduction potentials, arrange the following substances in order of decreasing ability as oxidizing agents: Fe3+, F2, Pb2+, I2, Sn2+, O2 Reduction potentials: Fe3+ = 0.77, F2 = 2.87, Pb2+ = -0.13, I2 = 0.54, Sn2+ = -0.14, O2 = 1.23 F2, O2, Fe3+, I2 , Pb2+, Sn2+

    4. 3. Calculate Eocell for the following cells using this data: Reaction Eo volts Cd?Cd2+ + 2e- 0.403 H2? 2H+ + 2e- 0.00 Ag?Ag+ + e- -0.799 A. Cadmium and hydrogen 0.403 + 0 = 0.403V B. Silver and hydrogen 0.799 + 0 = 0.799V C. Cadmium and silver 0.403 + 0.799 = 1.202V

    5. 4. For the following redox reaction, write out the two half-reactions and balance the equation, calculate Eo, and determine whether the reaction will occur spontaneously as written. Fe2+ + MnO4- ? Fe3+ + Mn2+ (acidic solution) Fe2+ ?Fe3+ + e- -0.77V MnO4- + 8H+ + 5e- ?Mn2+ + 4H2O +1.51V 5Fe2+ + MnO4- + 8H+ ? 5Fe3+ + Mn2+ + 4H2O E0cell = 0.74V Spontaneous

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