The $E^o$ for half cells $Fe/Fe^{2+}$ and $Cu/Cu^{2+}$ are $-0.44 \, V$ and $+0.32 \, V$ respectively. Then

Which method can be used to determine the strength of a reductant or oxidant in a solution? Explain with an example.

What happens to the Gibbs free energy in a spontaneous electrochemical process?

$A$ normal aluminium electrode coupled with a normal hydrogen electrode gives an $emf$ of $1.66 \ V$. The standard electrode potential of aluminium is ............ $V$.

The reduction potential values are given below. Which is the strongest reducing agent? $Al^{3+}/Al = -1.67 \, V, Mg^{2+}/Mg = -2.34 \, V, Cu^{2+}/Cu = +0.34 \, V, I_2/2I^- = +0.53 \, V$

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?