In $H_2-O_2$ fuel cell,the reaction occurring at the cathode is:

$A$ galvanic cell has an electrical potential of $1.1 \ V$. If an opposing potential of $1.1 \ V$ is applied to this cell,what will happen to the cell reaction and the current flowing through the cell?

If the standard $emf$ of the cell $Zn_{(s)} | Zn_{(1 \ M)}^{+2} || Ag_{(1 \ M)}^{+1} | Ag_{(s)}$ is $1.55 \ V$, what is the electrical work done under standard conditions (in $kJ$)?

Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)}$ takes place. Further show:
$(i)$ Which of the electrode is negatively charged?
$(ii)$ The carriers of the current in the cell.
$(iii)$ Individual reaction at each electrode.

In which cell is the free energy of a chemical reaction directly converted into electricity?

Can you store copper sulphate solutions in a zinc pot?