What is the standard potential of the cell $Ni|Ni^{2+}_{(1 \ M)} || Cu^{2+}_{(1 \ M)}| Cu$ (in $V$)? Given $E^{\circ}_{Cu^{2+}/Cu} = 0.337 \ V$ and $E^{\circ}_{Ni^{2+}/Ni} = -0.236 \ V$.

If the electrode potential of $Zn^{2+} | Zn$ is $-0.76 \, V$ and the potential of $Cu^{2+} | Cu$ is $0.34 \, V$,what will be the $EMF$ of the cell formed by both electrodes in $V$?

The standard reduction potential $E^{\circ}$ for half reactions are

$Zn \rightarrow Zn^{2+} + 2e^-$	$E^{\circ} = +0.76 \ V$
$Fe \rightarrow Fe^{2+} + 2e^-$	$E^{\circ} = +0.41 \ V$

The $EMF$ of the cell reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ is

Give the cell potential formula for the Daniell cell and the Copper-Silver cell.

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

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$,and $Fe^{2+}/Fe$ are $-0.76 \, V$,$-0.23 \, V$,and $-0.44 \, V$ respectively. For which of the following combinations will the reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ be spontaneous?