Have each group member select a half-reaction from Table 20.1.

Each member should calculate the standard cell potential of an electrochemical cell formed between each member’s halfreaction and the half-reaction of each of the other group members.

For each pair of half-reactions, write the overall balanced chemical reaction that will be spontaneous.

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TABLE 20.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction High tendency towards reduction F₂(g) + 2 e H₂O₂(aq) + 2 H(aq) + 2 e PbO₂ (s) + 4 H¹(aq) + SO₂² (aq) + 2 e MnO4 (aq) + 4 H (aq) + 3 e MnO4 (aq) +8 H*(aq) + 5 e Au³+ (aq) + 3 e PbO₂ (s) + 4 H(aq) + 2 e Cl₂(g) + 2 e Cr₂O2 (aq) + 14 H+(aq) + 6 e O₂(g) + 4 H(aq) + 4 e MnO₂(s) + 4 H+ (aq) + 2 e 103(aq) + 6 H(aq) + 5 e Br₂() +2 e VO₂ (aq) + 2 H+(aq) + e NO3(aq) + 4 H (aq) + 3 e ClO₂(g) + e Ag (aq) + e 2 F (aq) 2 H₂O(l) PbSO₁(s) + 2 H₂O(1) MnO₂ (s) + 2 H₂O(1) Mn2+ (aq) + 4H₂O(l) Au(s) Pb2+(aq) + 2 H₂O(l) 2 Cl(aq) 2 Cr³+(aq) + 7 H₂0(1) 2 H₂O(1) Mn+ (aq) + 2 H₂O(1) }(aq) + 3 H,O(I) 2 Br (aq) → VO+(aq) + H,O() NO(g) + 2 H₂O(1) CIO₂ (aq) Ag(s) E°(V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.96 0.95 0.80 Low tendency towards oxidation