Given:
$E^o_{Fe^{3+} /Fe} = -0.036 \ V, E^o_{Fe^{2+} /Fe} = -0.439 \ V$
The value of standard electrode potential for the change,
$Fe^{3+}_{(aq)} + e^- \rightarrow Fe^{2+}_{(aq)}$ will be ........ $V$.

The $E^{0}_{Red}$ values for elements $I, II, III,$ and $IV$ are $-3.04 \, V, -1.90 \, V, 0.00 \, V,$ and $1.90 \, V$ respectively. Which element has the maximum reducing power?

Which of the following is the weakest reducing agent?

The standard reduction potentials at $25^o \text{C}$ for $Li^{+}/Li$,$Ba^{2+}/Ba$,$Na^{+}/Na$,and $Mg^{2+}/Mg$ are $-3.05 \ V$,$-2.73 \ V$,$-2.71 \ V$,and $-2.37 \ V$ respectively. Which of the following is the strongest oxidizing agent?

$2H^{+} \, (aq) + 2e^- \to H_2 \, (g)$. The standard electrode potential for the above reaction is (in volts):

Standard electrode potential for the cell with cell reaction $Zn_{(s)} + Cu^{2+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + Cu_{(s)}$ is $1.1 \ V$. Calculate the standard Gibbs energy change for the cell reaction. (Given $F = 96487 \ C \ mol^{-1}$)