$A$ hydrogen gas electrode is made by dipping platinum wire in a solution of $HCl$ of $pH = 10$ and by passing hydrogen gas around the platinum wire at $1 \ atm$ pressure. The oxidation potential of the electrode would be $.......... \ V$.

Cell potential for the following reaction at $298 \ K$ is $0.096 \ V$. Calculate the $pH$ of the $HCl$ solution for the cell: $Sn_{(s)} | Sn^{2+} (0.05 \ M) || H^{+} (x \ M) | H_{2(g)} (1 \ bar) | Pt$ given $E_{Sn^{2+}|Sn}^{\circ} = -0.14 \ V$ and $E_{H^{+}|H_2}^{\circ} = 0.0 \ V$.

The initial $EMF$ of the concentration cell shown in the figure at $298 \ K$ is .............. $V$.

What is the $emf$ series?

Which one of the following has a potential more than zero?

The standard emf for the cell $Cd_{(s)}|Cd^{2+}_{(aq)}(1 \ M)||Cu^{2+}_{(aq)}(1 \ M)|Cu_{(s)}$ is $0.74 \ V$. If the concentration of $Cd^{2+}_{(aq)}$ and $Cu^{2+}_{(aq)}$ both decrease by $10$ times at $298 \ K$,calculate the emf of the cell.