Write the equation relating thermodynamics and electrochemistry.

If $E^{\circ}(Fe^{+2}_{(aq)} \mid Fe_{(s)}) = -0.44 \ V$ and $E^{\circ}(Sn^{+2}_{(aq)} \mid Sn_{(s)}) = -0.14 \ V$,what is the standard $emf$ of the cell containing the two electrodes?

Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al, Cu, Fe, Mg$ and $Zn$.

Calculate $E_{cell}^{\circ}$ for the following cell: $Zn_{(s)} | Zn^{2+}_{(1 \ M)} || Pb^{2+}_{(1 \ M)} | Pb_{(s)}$ given that $E^{\circ}_{Zn^{2+}/Zn} = -0.763 \ V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.126 \ V$. (in $V$)

The standard Gibbs energy change for the Daniel cell reaction is $Zn_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$ where $E_{\text{cell}}^{\circ} = 1.1 \ V$.

Reduction of species is dependent on its reduction potential value.