The standard reduction potential for $Mg^{2+}/Mg$ is $-2.37 \ V$ and for $Cu^{2+}/Cu$ is $0.337 \ V$. The $E^{\circ}_{cell}$ for the following reaction is $Mg + Cu^{2+} \longrightarrow Mg^{2+} + Cu$

For the half-reactions $Zn \rightarrow Zn^{2+} + 2e^{-}$ and $Fe \rightarrow Fe^{2+} + 2e^{-}$,the standard oxidation potentials are given as $E^{0}_{Oxi} = +0.76 \ V$ and $E^{0}_{Oxi} = +0.41 \ V$ respectively. Calculate the cell potential for the reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ in $V$.

Four metals $A$,$B$,$C$,and $D$ have Standard Reduction Potential $(SRP)$ values of $-3.05 \ V$,$-1.66 \ V$,$-0.40 \ V$,and $0.80 \ V$ respectively. Which is the strongest reducing agent?

For the cell reaction,$2Ce^{4+} + Co \to 2Ce^{3+} + Co^{2+}$,$E^\circ_{cell}$ is $1.89 \ V$. If $E^\circ_{Co^{2+}/Co} = -0.28 \ V$,then $E^\circ_{Ce^{4+}/Ce^{3+}}$ is equal to:

Given:
$E^o_{Fe^{3+} /Fe} = -0.036 \ V, E^o_{Fe^{2+} /Fe} = -0.439 \ V$
The value of standard electrode potential for the change,
$Fe^{3+}_{(aq)} + e^- \rightarrow Fe^{2+}_{(aq)}$ will be ........ $V$.

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