Calculate the $Zn-Cu$ cell (Daniell cell) potential. Given: $E^o_{Zn^{2+}|Zn} = -0.76 \ V$ and $E^o_{Cu^{2+}|Cu} = 0.34 \ V$. (in $V$)

Give the method to determine the potential of any half-cell.

Write the equation relating thermodynamics and electrochemistry.

$A$ standard hydrogen electrode has zero electrode potential because

$A$ cell is constructed by dipping a copper rod in $1\,M\,CuSO_4$ solution and a nickel rod in $1\,M\,NiSO_4$ solution. The standard reduction potentials of copper and nickel electrodes are $+0.34\,V$ and $-0.25\,V$ respectively. Calculate the $EMF$ of the cell. (in $,V$)

Review the $SRP$ (at $25\,\text{°C}$) data in acidic medium:
$Ti^{4+} + e^- \to Ti^{3+}, \, E^o = -x \text{ V}$
$Fe^{3+} + e^- \to Fe^{2+}, \, E^o = -y \text{ V}$
where $x < y$,point out the wrong statement.