What is E°_cell for a galvanic cell represented by the combination of the following half-reactions?

Question

Quizplus · Accepted Answer

The cell reaction can be written as:
Cu(s) + 2Ag+(aq) -> Cu2+(aq) + 2Ag(s)
The standard reduction potentials for Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) half-reactions are:
Cu2+(aq) + 2e- -> Cu(s) E° = +0.34 V
Ag+(aq) + e- -> Ag(s) E° = +0.80 V
To calculate the standard cell potential (E°cell), we need to subtract the reduction potential of the anode (Cu2+(aq)/Cu(s)) from the reduction potential of the cathode (Ag+(aq)/Ag(s)):
E°cell = E°cathode - E°anode
E°cell = +0.80 V - (+0.34 V) = +0.46 V
However, the question is asking for the electromotive force of the cell reaction in the opposite direction (i.e., when the anode is the standard electrode), which is the negative of the cell potential:
E°anode = - E°cell = -(+0.46 V) = -0.46 V
Therefore, the answer is D) 1.66 V.

What Is E°cell for a Galvanic Cell Represented by the Combination

What Is E°_cell for a Galvanic Cell Represented by the Combination