I will get you started on a and b.
a.
Ni ==> Ni^2+ Eo = ? as an oxiation
Ag^+ +e ==> Ag Eo = ? as a reduction
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Ni + 2Ag^+ ==> Ni^2+ + 2Ag
Ecell = sum E(oxdn) + E(redn) from above.
b is done the same way.
Zn + 2Ag^+ ==> Zn^2+ + 2Ag
Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00 M solutions of their ions. a) If connected as voltaic cells in series, which two metals are plated, and what is the total potential?
a) Ecell for Ag and Ni
b) Ecell for Ag and Zn
c) If 3.30 g of metal is plated in the voltaic cell, how much metal is plated in the electrolytic cell?
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