Which metal among the following is most sensitive towards oxidation?

Give the symbolic representation of the following half-cells (electrodes):
$(i)$ $2H^{+}_{(aq)} + 2e^- \to H_{2_{(g)}}$
$(ii)$ $Br_{2_{(aq)}} + 2e^- \to 2Br^{-}_{(aq)}$
$(iii)$ $2Br^{-}_{(aq)} \to Br_{2_{(aq)}} + 2e^-$

The $E^0_{cell}$ of the cell $Al(s)|Al^{3+}(1M)||Pb^{2+}(1M)|Pb(s)$ is $1.5 \text{ V}$. If $E^0_{Pb^{2+}/Pb}$ is $-0.14 \text{ V}$, then $E^0_{Al^{3+}/Al}$ will be: (in $\text{ V}$)

Can $E_{cell}^o$ or $\Delta_r G^o$ for a cell reaction ever be equal to zero?

Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the cathode with a suitable example.

Electrode potential of $Zn^{2+}/Zn$ is $-0.76\,V$ and that of $Cu^{2+}/Cu$ is $+0.34\,V$. The $EMF$ of the cell constructed between these two electrodes is ............ $V$.