Study the two half reactions of an electrochemical cell.

Question

Ag(s) → Ag+(aq) + e–
E0 = 0.80 V

Cu(s) → Cu2+(aq) + 2e–
E0 = 0.34 V

Which option correctly gives the standard cell potential of

Ag+(aq) + Cu (s) → 2Ag(s) + Cu2+(aq) reaction?

-1.60
-0.46
1.60
0.46

Answer 1

Something is not right here.
First, the two equations you have written as oxidations have the wrong sign. Second, you don't give any options. Here is the way you get the cell potential for the one reaction you have written.
Ag+(aq) + Cu (s) → 2Ag(s) + Cu2+(aq)

2Ag^+(aq) + 2e ==> 2Ag(s) .......Eo red =+0.80
Cu(s) ==> Cu^2+(aq) + 2e................Eo ox = -0.34
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2Ag^+(aq) + Cu(s) ==> Cu^2+(aq) + 2Ag(s) Ecell = ?
Ecell = Eox + Ered = 0.80 + (-0.34) = ?
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