Dr.Bobb222 please help balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)

(a) NO3−(aq) + Pb(s) → NO(g) + Pb2+(aq)(b) O2(g) + Mn(s) → H2O(l) + Mn2+(aq)
(c) ClO2(g) + Mn2+(aq) → ClO2−(aq) + MnO4−(aq)
(d) F2(g) + IO3−(aq) → F −(aq) + IO4−(aq)

Any solution process that you explain to any one of the redox equations I'm sure will help me to solve the rest. The balancing of the oxidation and reduction equations individually is really grilling me. I appreciate your help, thank you.

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  1. 3Pb + 2NO3- + 8H+ → 3Pb2+ + 2NO + 4H2O
    2Mn + O2 + 4H+ → 2Mn2+ + 2H2O
    Mn2+ + 5ClO2 + 4H2O → MnO4- + 5ClO2- + 8H+
    IO3- + F2 + H2O → IO4- + 2F- + 2H+

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