$A$ galvanic cell with electrode potential of $A = + 2.23 \ V$ and $B = - 1.43 \ V$. The value of $E^o_{cell}$ is .............. $V$.

What is the standard potential of the cell $Ni|Ni^{2+}_{(1 \ M)} || Cu^{2+}_{(1 \ M)}| Cu$ (in $V$)? Given $E^{\circ}_{Cu^{2+}/Cu} = 0.337 \ V$ and $E^{\circ}_{Ni^{2+}/Ni} = -0.236 \ V$.

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$ and $Fe^{2+}/Fe$ are $-0.76 \ V$,$-0.23 \ V$ and $-0.44 \ V$ respectively.
The reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ will be spontaneous when:

If the $\Delta G$ of a cell reaction $AgCl + e^- \to Ag + Cl^{-}$ is $-21.20 \ kJ$,the standard e.m.f. of the cell is ............ $V$.

Which method can be used to determine the strength of a reductant or oxidant in a solution? Explain with an example.

Which is the increasing order of reducing power of the following metals on the basis of standard electrode potential? $Ag^{+}/Ag = 0.80 \ V$,$Mg^{2+}/Mg = -2.37 \ V$,$Hg^{2+}/Hg = 0.79 \ V$,$Cr^{3+}/Cr = -0.74 \ V$