The standard reduction potentials (in $V$) of a few metal ion/metal electrodes are given below: $Cr^{3+}/Cr = -0.74$; $Cu^{2+}/Cu = +0.34$; $Pb^{2+}/Pb = -0.13$; $Ag^{+}/Ag = +0.8$. The reducing strength of the metals follows the order:

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 $e^-$.

The $E^{\circ}$ for Daniell cell is $1.1 \ V$. Calculate $\Delta G^{\circ}$ for the following reaction: $Zn_{(s)} + Cu^{2+}_{(aq)} \rightleftharpoons Zn^{2+}_{(aq)} + Cu_{(s)}$

The standard reduction potential for $Fe^{2+}/Fe$ and $Sn^{2+}/Sn$ electrodes are $-0.44 \ V$ and $-0.14 \ V$ respectively. For the given cell reaction $Fe^{2+} + Sn \to Fe + Sn^{2+}$,the standard $EMF$ is ...............$V$.

The reducing ability of the metals $K$,$Au$,$Zn$ and $Pb$ follows the order

Using the standard electrode potentials given below,identify the correct statements from the following.
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
$Cu^{2+} + 2e^{-} \longrightarrow Cu ; E^{\circ} = +0.34 \ V$
$Ag^{+} + e^{-} \longrightarrow Ag ; E^{\circ} = +0.80 \ V$
$(i)$ Copper can displace iron from $FeSO_4$ solution.
$(ii)$ Iron can displace copper from $CuSO_4$ solution.
$(iii)$ Silver can displace copper from $CuSO_4$ solution.
$(iv)$ Iron can displace silver from $AgNO_3$ solution.