The $emf$ of a galvanic cell constituted with the electrodes $Zn^{2+} | Zn$ $(-0.76 \ V)$ and $Fe^{2+} | Fe$ $(-0.41 \ V)$ is

The $E^o$ for the reduction of $NO_3^-$ ion in aqueous solution is $+0.96 \, V$. The $E^o$ values for several metal ions are given below:
$V^{2+}_{(aq)} + 2e^{-} \rightarrow V, \, E^o = -1.19 \, V;$
$Fe^{3+}_{(aq)} + 3e^{-} \rightarrow Fe, \, E^o = -0.04 \, V;$
$Au^{3+}_{(aq)} + 3e^{-} \rightarrow Au, \, E^o = +1.40 \, V;$
$Hg^{2+}_{(aq)} + 2e^{-} \rightarrow Hg, \, E^o = +0.86 \, V$
Which of the following pairs of metals is $NOT$ oxidized by $NO_3^-$ in aqueous solution?

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

The $E^o$ values of half-cells are given below. Which combination of two half-cells will form a cell with the maximum potential?
$(i)$ $A + e^- \rightarrow A^- ; E^o = -0.24 \ V$
$(ii)$ $B^- + e^- \rightarrow B^{2-} ; E^o = +1.25 \ V$
$(iii)$ $C^- + 2e^- \rightarrow C^{3-} ; E^o = -1.25 \ V$
$(iv)$ $D + 2e^- \rightarrow D^{2-} ; E^o = +0.68 \ V$

Identify the reaction from the following that occupies the top position in the $EMF$ series (standard reduction potential) at $298 \; K$.

The $E^{0}_{Red}$ values for elements $I, II, III,$ and $IV$ are $-3.04 \, V, -1.90 \, V, 0.00 \, V,$ and $1.90 \, V$ respectively. Which element has the maximum reducing power?