In a galvanic cell,the salt bridge

For a hydrogen-oxygen fuel cell at $1 \text{ atm}$ and $298 \text{ K}$, the reaction is $H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_{2}O_{(l)}$; $\Delta G^{\circ} = -240 \text{ kJ}$. The $E^{\circ}$ for the cell is approximately (Given $F = 96,500 \text{ C}$): (in $\text{ V}$)

The position of some metals in the electrochemical series in decreasing electropositive character is given as $Mg > Al > Zn > Cu > Ag$. What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

What happens to the oxidation number of $Mn$ during the operation of a dry cell?

$A^{2+}_{(aq.)} + 2e^- \to A_{(s)}$ ; $E^{\circ} = 0.8 \ V$
$B^{3+}_{(aq.)} + 3e^- \to B_{(s)}$ ; $E^{\circ} = 0.6 \ V$
Using the above information,find the ion which will be deposited first at the cathode if a solution containing $A^{2+}_{(aq.)}$ and $B^{3+}_{(aq.)}$ is electrolysed.

What will occur if a block of copper metal is dropped into a beaker containing a solution of $1 \ M \ ZnSO_4$?