For the following electrochemical cell
Cu(s)|Cu2+(aq,1.00 mol dm-3)||Zn2+ (aq,1.00 mol dm-3)|Zn(s)
choose the correct option in the light of the following standard electrode potentials :
| Half - reaction | E°/V |
| \(\frac{1}{2} \mathrm{Cu}^{2+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \frac{1}{2} \mathrm{Cu}(\mathrm{s})\) | +0.34 |
| \(\frac{1}{2} \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \frac{1}{2} \mathrm{Zn}(\mathrm{s})\) | -0.76 V |
1
The potential of the cell is -1.10 V and the zinc electrode is negative.
2
The potential of the cell is +1.10 V and the zinc electrode is negative.
3
The potential of the cell is -1.10 V and the zinc electrode is positive.
4
The potential of the cell is +1.10 V and the zinc electrode is positive.