From the following ${E^o}$ values of half cells,what combination of two half cells would result in a cell with the largest potential?
$I$. $A + e^- \to A^{-}$,${E^o} = +0.24 \ V$
$II$. $B^{-} + e^- \to B^{-2}$,${E^o} = +1.25 \ V$
$III$. $C^{-} + 2e^- \to C^{-3}$,${E^o} = +0.15 \ V$
$IV$. $D + 2e^- \to D^{-2}$,${E^o} = +0.68 \ V$

For the reaction $F_2 + 2e^{-} \to 2F^{-}$,$E^{\circ} = 2.8 \, V$. What is the $E^{\circ}$ for the reaction $\frac{1}{2} F_2 + e^{-} \to F^{-}$?

Which of the following metals does not liberate $\text{H}_2$ gas by reacting with $\text{HCl}$?

For the reaction $Cr_2O_7^{2-} + I^- \to I_2 + Cr^{3+}$,if $E_{cell}^o = 0.79 \ V$ and $E_{Cr_2O_7^{2-}}^o = 1.33 \ V$,then $E_{I_2}^o = $ ............. $V$.

In a cell,the following reactions take place:
$Fe^{2+} \rightarrow Fe^{3+} + e^{-}$ $\quad$ $E^{\circ}_{Fe^{3+} / Fe^{2+}} = 0.77 \, V$
$2I^{-} \rightarrow I_{2} + 2e^{-}$ $\quad$ $E^{\circ}_{I_{2} / I^{-}} = 0.54 \, V$
The standard electrode potential for the spontaneous reaction in the cell is $x \times 10^{-2} \, V$ at $298 \, K$. The value of $x$ is .... (Nearest Integer)

The tendency of an electrode to lose electrons is known as