The standard oxidation potentials for the half-reactions are given as $Zn \to Zn^{2+} + 2e^{-}; E^o = +0.76 \ V$ and $Fe \to Fe^{2+} + 2e^{-}; E^o = +0.41 \ V$. The $EMF$ for the cell reaction $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.

The standard electrode potentials of $Ag^{+}/Ag$,$Hg_2^{2+}/2Hg$,$Cu^{2+}/Cu$,and $Mg^{2+}/Mg$ are $0.80 \ V$,$0.79 \ V$,$0.34 \ V$,and $-2.37 \ V$,respectively. An aqueous solution containing $1 \ M$ concentration of each of these metal salts is electrolyzed. With increasing voltage,what is the correct sequence of deposition of the metals at the cathode?

In a cell,the following reactions take place:
$Fe^{2+} \rightarrow Fe^{3+} + e^{-}$ $\quad$ $E^{\circ}_{Fe^{3+} / Fe^{2+}} = 0.77 \, V$
$2I^{-} \rightarrow I_{2} + 2e^{-}$ $\quad$ $E^{\circ}_{I_{2} / I^{-}} = 0.54 \, V$
The standard electrode potential for the spontaneous reaction in the cell is $x \times 10^{-2} \, V$ at $298 \, K$. The value of $x$ is .... (Nearest Integer)

Two half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:

Which expression represents the cell potential $(E_{cell})$?

Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]