If the $emf$ of the cell $Cu(s) | Cu^{2+}(1 \text{ M}) || Ag^+(1 \text{ M}) | Ag(s)$ is $0.463 \text{ V}$ at $25^{\circ} \text{C}$ and the standard electrode potential of the $Cu$ electrode is $0.337 \text{ V}$, find the standard electrode potential of the $Ag$ electrode. (in $\text{ V}$)

Given: $E^{0}_{Mn^{+7} \mid Mn^{+2}} = 1.5 \ V$ and $E^{0}_{Mn^{+4} \mid Mn^{+2}} = 1.2 \ V$,then $E^{0}_{Mn^{+7} \mid Mn^{+4}}$ is (in $V$)

Given the standard electrode potentials: $Fe^{2+}_{(aq)} + 2e^{-} \rightarrow Fe_{(s)}$ $(E^o = -0.44 \ V)$ and $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ $(E^o = 0.77 \ V)$. If $Fe^{2+}$,$Fe^{3+}$,and a piece of $Fe$ are kept together,what happens?

Explain: Reduction reaction is possible with higher $E^{\theta}$ value.

If $E^o_{A^{+2}/A} = -0.30 \ V$ and $E^o_{A^{+3}/A^{+2}} = 0.40 \ V$,the standard $EMF$ of the reaction: $A + 2A^{+3} \to 3A^{+2}$ will be ............ $V$.

Using the standard electrode potential values,which of the following statements $(I, II, III, IV)$ is/are correct?
$Fe^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Fe_{(s)}$ ; $E^o = -0.44 \, V$
$Cu^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Cu_{(s)}$ ; $E^o = +0.34 \, V$
$Ag^{+}_{(aq)} + e^{-} \rightleftharpoons Ag_{(s)}$ ; $E^o = +0.80 \, V$
$I$. Copper displaces iron from $FeSO_4$ solution.
$II$. Iron displaces copper from $CuSO_4$ solution.
$III$. Silver displaces copper from $CuSO_4$ solution.
$IV$. Iron displaces silver from $AgNO_3$ solution.