The cells which can be recharged are:

$Cu^{+}_{(aq)}$ is unstable in solution and undergoes simultaneous oxidation and reduction,according to the reaction $2 Cu^{+}_{(aq)} \rightleftharpoons Cu^{2+}_{(aq)} + Cu_{(s)}$. Choose the correct $E^{\circ}$ for the above reaction if $E^{\circ}_{Cu^{2+}/Cu} = 0.34 \ V$ and $E^{\circ}_{Cu^{2+}/Cu^{+}} = 0.15 \ V$.

Consider the figure and answer the following questions.
$(i)$ Cell $'A'$ has $E_{cell} = 2 \ V$ and cell $'B'$ has $E_{cell} = 1.1 \ V$. Which of the two cells,$'A'$ or $'B'$,will act as an electrolytic cell? Which electrode reactions will occur in this cell?
$(ii)$ If cell $'A'$ has $E_{cell} = 0.5 \ V$ and cell $'B'$ has $E_{cell} = 1.1 \ V$,then what will be the reaction at the anode and cathode?

When a lead storage battery is charged,what happens?

$Zn_{(s)} | Zn^{2+}_{(aq)} || Cu^{2+}_{(aq)} | Cu_{(s)}$ is

Standard electrode potentials of $Zn$ and $Fe$ are known to be $(i) -0.76 \ V$ and $(ii) -0.44 \ V$ respectively. How does this explain that galvanization prevents rusting of iron while zinc slowly dissolves away?