Under standard conditions, what will be the potential of cell based on the reaction given below and predict whether, it can occur spontaneously or not.

${\mathrm{Pb}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{Fe}}^{+2}\to 2{\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+\mathrm{Pb}\left(\mathrm{s}\right)$

Given data:

${\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right); {\mathrm{E}}^{\mathrm{o}}=+0.771 \mathrm{V}$

${\mathrm{Pb}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\to \mathrm{Pb}\left(\mathrm{s}\right); {\mathrm{E}}^{\mathrm{o}}=-0.126 \mathrm{V}$

The standard reduction potential for ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$ is $+\mathrm{0.34 }\mathrm{V}.$ Calculate the reduction potential at $\mathrm{pH}=14$ for the above couple.

$\left({\mathrm{K}}_{\mathrm{sp}} \mathrm{of} \mathrm{Cu}{\left(\mathrm{OH}\right)}_2=1\times {10}^{-19}\right)$

In which metal container, the aqueous solution of ${\mathrm{CuSO}}_4$ can be stored?

${\mathrm{E}}_{{\mathrm{Cu}}^{3+}/\mathrm{Cu}}^0=0.34 \mathrm{V}$

$E_{Fe/F{e}^{2+}}^0=0.44V,E_{Al/A^{3+}}^0=1.66V$

$E_{Ni/N^{2+}}^0=0.25V,E_{A{g}^{+}/Ag}^0=0.80V$

Calculate the standard cell potential (in V) of the cell in which the following reaction takes place:

${\mathrm{F}\mathrm{e}}^{2+}\mathrm{ }\left(\mathrm{a}\mathrm{q}\right)+\mathrm{A}{\mathrm{g}}^{+}\left(\mathrm{a}\mathrm{q}\right)\to \mathrm{F}{\mathrm{e}}^{3+}\left(\mathrm{a}\mathrm{q}\right)+\mathrm{A}\mathrm{g}\left(\mathrm{s}\right)$

Given that
${\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{A}\mathrm{g}}^{\mathrm{o}}=\mathrm{x}\mathrm{ }\mathrm{V}$
${\mathrm{E}}_{{\mathrm{F}\mathrm{e}}^{2+}/\mathrm{F}\mathrm{e}}^{\mathrm{o}}=\mathrm{y}\mathrm{ }\mathrm{V}$
${\mathrm{E}}_{{\mathrm{F}\mathrm{e}}^{3+}/\mathrm{F}\mathrm{e}}^{\mathrm{o}}=\mathrm{z}\mathrm{ }\mathrm{V}$

Given the standard half-cell potentials $\left(\mathrm{E}°\right)$ of the following as

$\mathrm{Zn}⟶{\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}; \mathrm{E}°=+0.76 \mathrm{V}$

$\mathrm{Fe}⟶{\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}; \mathrm{E}°=+0.41 \mathrm{V}$

Then the standard e.m.f. of the cell with the reaction ${\mathrm{Fe}}^{2+}+\mathrm{Zn}⟶{\mathrm{Zn}}^{2+}+\mathrm{Fe}$ is

What will be the oxidation potential for the following hydrogen half cell at $1$bar pressure and $25º\mathrm{C}$ temperature?

$\mathrm{Pt}\left|\underset{ 1\mathrm{bar} }{{\mathrm{H}}_{2\left(g\right)}}\right|{\mathrm{HCl}}_{\left(\mathrm{aq}\right)}\mathrm{pH}=3$