In which metal container can an aqueous solution of $CuSO_4$ be stored?
$E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$

Given
$E^o_{Cl_2/Cl^-} = 1.36 \ V,$
$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$
$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
Among the following,the strongest reducing agent is:

What is the $e.m.f.$ of the cell in $V$?
$Cr | Cr^{3+} (1.0 \ M) || Co^{2+} (1.0 \ M) | Co$
Given: $E^{o}$ for $Cr^{3+} | Cr = -0.74 \ V$ and $Co^{2+} | Co = -0.28 \ V$

The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is

Given $E^{0}_{Fe^{3+}|Fe} = -0.036 \, V$ and $E^{0}_{Fe^{2+}|Fe} = -0.439 \, V$,the standard electrode potential for the reaction $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ is ........... $V$.

The oxidation potentials of $Zn$,$Cu$,and $Ag$ are $0.76 \ V$,$-0.34 \ V$,and $-0.80 \ V$,respectively. Write down the order of their tendency to lose $e^-$.