Given standard electrode potentials:
$Fe^{2+} + 2e^- \to Fe; E^o = -0.440 \ V$
$Fe^{3+} + 3e^- \to Fe; E^o = -0.036 \ V$
The standard electrode potential $(E^o)$ for $Fe^{3+} + e^- \to Fe^{2+}$ is .............. $V$.

For the spontaneity of a cell,which of the following is correct?

The standard reduction potential values of the three metallic cations $x, y, z$ are $0.52 \ V, -3.03 \ V$ and $-1.18 \ V$ respectively. The order of reducing power of their corresponding metals will be

For the half-reactions $Zn \rightarrow Zn^{2+} + 2e^{-}$ and $Fe \rightarrow Fe^{2+} + 2e^{-}$,the standard oxidation potentials are given as $E^{0}_{Oxi} = +0.76 \ V$ and $E^{0}_{Oxi} = +0.41 \ V$ respectively. Calculate the cell potential for the reaction $Fe^{2+} + Zn \rightarrow Zn^{2+} + Fe$ in $V$.

The standard electrode potentials of the half-cells are given below:
$Zn^{2+} + 2e^- \to Zn$; $E^{\circ} = -0.76 \, V$
$Fe^{2+} + 2e^- \to Fe$; $E^{\circ} = -0.44 \, V$
The $EMF$ of the cell $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

Give the anode reaction for an electrode of any metal $M \,|\, M^{n+}$.