Given the standard reduction potentials: E°[Zn2+/Zn] = -0.76 V and E°[Cu2+/Cu] = +0.34 V, what is the standard cell potential (E°cell) for the Daniell cell: Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s)?
Answer and explanation
Correct answer: C. +1.10 V
Zinc is oxidized at the anode (E°_red = -0.76 V) and copper is reduced at the cathode (E°_red = +0.34 V). The standard cell potential is E°_cell = E°_cathode - E°_anode = +0.34 V - (-0.76 V) = +0.34 V + 0.76 V = +1.10 V.
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