Among the following metals,the strongest reducing agent is

The relation between $\Delta G$ and $E$ for a cell is given by $\Delta G = -nFE$. Which of the following conditions must be satisfied for the cell reaction to be spontaneous?

Given electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:

If in a galvanic cell,the hydrogen half-cell is the cathode on the right side,what is the sign of the standard electrode potential of such a galvanic cell? Give an example.

Four metals $A$,$B$,$C$,and $D$ have Standard Reduction Potential $(SRP)$ values of $-3.05 \ V$,$-1.66 \ V$,$-0.40 \ V$,and $0.80 \ V$ respectively. Which is the strongest reducing agent?

The standard reduction potential at $298 \ K$ for the following half-cell reactions is given as:
$Zn^{2+}_{(aq)} + 2e^{-} \rightarrow Zn_{(s)} ; \quad E^{\circ} = -0.762 \ V$
$Cr^{3+}_{(aq)} + 3e^{-} \rightarrow Cr_{(s)} ; \quad E^{\circ} = -0.740 \ V$
$2H^{+}_{(aq)} + 2e^{-} \rightarrow H_{2(g)} ; \quad E^{\circ} = 0.0 \ V$
$F_{2(g)} + 2e^{-} \rightarrow 2F^{-}_{(aq)} ; \quad E^{\circ} = 2.87 \ V$
Which of the following is the strongest reducing agent?