$A$ standard hydrogen electrode has zero electrode potential because

The standard electrode potential $(E^{\circ}_{M^{3+}/M^{2+}})$ for $V$,$Cr$,$Mn$,and $Co$ are $-0.26 \ V$,$-0.41 \ V$,$+1.57 \ V$,and $+1.97 \ V$,respectively. The metal ions which can liberate $H_2$ from a dilute acid are

The standard reduction potentials at $298 \ K$ for the following half reactions are given against each:
$Zn^{2+}(aq.) + 2e^- \rightleftharpoons Zn_{(s)}$; $E^\circ = -0.762 \ V$
$Cr^{3+}(aq.) + 3e^- \rightleftharpoons Cr_{(s)}$; $E^\circ = -0.740 \ V$
$2H^{+}(aq.) + 2e^- \rightleftharpoons H_{2(g)}$; $E^\circ = 0.00 \ V$
$Fe^{3+}(aq.) + e^- \rightleftharpoons Fe^{2+}(aq.)$; $E^\circ = 0.770 \ V$
Which is the strongest reducing agent?

Which of the following metals cannot displace $H_2$ from acids or $H_2O$ from its compounds?

Standard reduction electrode potentials of three metals $A$,$B$,and $C$ are respectively $+0.5 \ V$,$-3.0 \ V$,and $-1.2 \ V$. The reducing powers of these metals are

Two half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be: