Among the following metals,the strongest reducing agent is

Which of the following metals does not release $H_{2(g)}$ upon reaction with acid?

Which metal among the following has the strongest tendency to undergo oxidation?

Given the standard electrode potentials: $E^o_{Cr^{3+}/Cr} = -0.74 \ V$,$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$,$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V$,and $E^o_{Cl_2/Cl^-} = 1.36 \ V$. Based on this information,which is the strongest oxidizing agent?

Using the standard electrode potential values,which of the following statements $(I, II, III, IV)$ is/are correct?
$Fe^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Fe_{(s)}$ ; $E^o = -0.44 \, V$
$Cu^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Cu_{(s)}$ ; $E^o = +0.34 \, V$
$Ag^{+}_{(aq)} + e^{-} \rightleftharpoons Ag_{(s)}$ ; $E^o = +0.80 \, V$
$I$. Copper displaces iron from $FeSO_4$ solution.
$II$. Iron displaces copper from $CuSO_4$ solution.
$III$. Silver displaces copper from $CuSO_4$ solution.
$IV$. Iron displaces silver from $AgNO_3$ solution.

Consider the half-cell reduction reactions:
$Mn^{2+} + 2e^{-} \rightarrow Mn$,$E^{\circ} = -1.18 \ V$
$Mn^{3+} + e^{-} \rightarrow Mn^{2+}$,$E^{\circ} = +1.51 \ V$
The $E^{\circ}$ for the reaction $3Mn^{2+} \rightarrow Mn + 2Mn^{3+}$,and the possibility of the forward reaction are respectively: