The standard electrode potential is measured by

The standard Gibbs energy change for the Daniel cell reaction is $Zn_{(s)} + Cu^{2+}_{(aq)} \longrightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$ where $E_{\text{cell}}^{\circ} = 1.1 \ V$.

$Zn^{2+} + 2e^- \to Zn_{(s)}$; $E^o = -0.76 \ V$
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = +0.77 \ V$
$Cr^{3+} + 3e^- \to Cr_{(s)}$; $E^o = -0.74 \ V$
$H^{+} + e^- \to 1/2 H_2$; $E^o = 0.00 \ V$
Which of the following is the strongest reducing agent?

The standard reduction potential for $Fe^{2+}/Fe$ and $Sn^{2+}/Sn$ electrodes are $-0.44 \ V$ and $-0.14 \ V$ respectively. For the cell reaction,$Fe^{2+} + Sn \longrightarrow Fe + Sn^{2+}$,the standard emf is:

Among the following metals,the strongest reducing agent is

The standard electrode potentials of $Zn^{2+}/Zn$ and $Ag^{+}/Ag$ are $-0.763 \ V$ and $+0.799 \ V$ respectively. The standard potential of the cell is ............ $V$.