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Determine whether the following redox reactions are spontaneous as written? (Use the information in the table below. Show the half reactions and the potentials for each half reaction.)

a. 2Ag(s) + Mg2+(aq) → 2Ag+ (aq) + Mg(s) [5 points]

b. 2Al(s) + 3Zn2+(aq) → 2Al3+(aq) + 3Zn(s) [5 points]

Reduction Potentials at 25°C
Electrode Half-Reaction E0(V)
Mg2+/Mg Mg2+ + 2e– → Mg –2.37
Al3+/Al Al3+ + 3e– → Al –1.66
Zn2+/Zn Zn2+ + 2e– → Zn –0.76
Ag2+/Ag Ag+ + e– → Ag +0.80

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  1. 2Ag(s) + Mg2+(aq) → 2Ag+ (aq) + Mg(s) [5 points]
    2Ag(s) ==>2 Ag^+ + e ...........E = -0.80
    Mg^2+ + 2e ==> Mg(s) ......E = -2.87
    --------------------------------------------
    2Ag(s) + Mg^2+ ==> 2Ag^+ +Mg(s) E = -3.67
    E cell is negative. It will not be spontaneous.
    The others are done the same way.

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    DrBob222

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