Which of the following equations represents the cell potential?

The standard electrode potential for the Daniell cell is $1.1 \ V$. What will be the value of standard Gibbs energy for the reaction?
$Zn_{(s)} + Cu_{(aq)}^{2+} \rightarrow Zn_{(aq)}^{2+} + Cu_{(s)}$
$(1 \ F = 96487 \ C \ mol^{-1})$

For the cell reaction,$2 Al_{(s)} + 3 Cu^{2+}_{(aq)} \rightarrow 2 Al^{3+}_{(aq)} + 3 Cu_{(s)}$. If $\Delta G^{\circ} = -1158 \ kJ$,what is $E^{\circ}_{cell}$ (in $V$)?

Consider the cell given below:
$Ag_{(s)} | Ag^{\oplus} || Cu^{2+} | Cu_{(s)}$
Given:
$Ag^{\oplus} + e^{-} \to Ag; E^{o} = x$
$Cu^{2+} + 2e^{-} \to Cu; E^{o} = y$
The value of $E^{o}_{cell}$ is:

The cell reaction of a cell is $Mg_{(s)} + Cu^{2+}_{(aq)} \to Cu_{(s)} + Mg^{2+}_{(aq)}$. If the standard reduction potentials of $Mg$ and $Cu$ are $-2.37 \ V$ and $+0.34 \ V$ respectively,the $EMF$ of the cell is ................. $V$.

For the following cell,the standard potential of the copper electrode is $0.337 \ V$ and the standard cell potential is $0.463 \ V$ for the reaction $Cu|Cu^{2+}(1 \ M)||Ag^{+}(1 \ M)|Ag$. What is the standard potential of the silver electrode (in $V$)?