# Problem: Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00M solutions of their ions.a) if connected as a voltaic cells in series, which two metals are plated, and what is the total potential?

###### FREE Expert Solution

↓ E° → oxidation → anode → Al/Al3+

↑ E° → reduction → cathode → Ag/Ag+

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

E°cell = 0.80 - (-1.66) = +2.46 V

###### Problem Details

Consider two cells, the first with Al and Ag electrodes, and the second with Zn and Ni electrodes, each in appropriate 1.00M solutions of their ions.

a) if connected as a voltaic cells in series, which two metals are plated, and what is the total potential?