Calculate the E.M.F. of the following cell at $298 \mathrm{K}:$

$\mathrm{Mg}\left|{\mathrm{Mg}}^{2+}\left(0.130\mathrm{M}\right)\right|\left|{\mathrm{Ag}}^{+}\left(1.0\times {10}^{-4}\mathrm{M}\right)\right|\mathrm{Ag}$

Given that ${\mathrm{E}}_{\left({\mathrm{Mg}}^{2+}\mid \mathrm{Mg}\right)}^{\mathrm{\Theta }}=-2.37 \mathrm{V}, {\mathrm{E}}_{\left({\mathrm{Ag}}^{+}\mid \mathrm{Ag}\right)}^{\mathrm{\Theta }}=0.80 \mathrm{V}$

Calculate the equilibrium constant $\mathrm{K}$ for the reaction at $298 \mathrm{K}:$

$\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right)$ [Given ${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{°}=-0.76 \mathrm{V}; {\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{°}=0.34 \mathrm{V}$]

Calculate the equilibrium constant for the following cell reaction.

$\frac{1}{2}{\mathrm{Cl}}_2\left(\mathrm{g}\right)+{\mathrm{Br}}^{-}⟶\frac{1}{2}{\mathrm{Br}}_2\left(\mathrm{l}\right)+{\mathrm{Cl}}^{-}; {\mathrm{E}}^{°}=0.30 \mathrm{V}$

Calculate the value of $\mathrm{\Delta G}$ and ${\mathrm{E}}_{\mathrm{cell}}$ at $298 \mathrm{K}$ for the following cell.

$\mathrm{Al}\left|{\mathrm{AI}}_{(0.01\mathrm{M})}^{3+}\right|\left|{\mathrm{Fe}}_{(0.02\mathrm{M})}^{2+}\right|\mathrm{Fe}$

Given that ${\mathrm{E}}_{{\mathrm{Al}}^{3+}/\mathrm{Al}}^{\mathrm{\Theta }}=-1.66 \mathrm{V}$ and ${\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{\mathrm{\Theta }}=0.80 \mathrm{V}$

Calculate the maximum work that can be obtained from the following cell

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\right|\left|{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\right|\mathrm{Ag}$

Given that ${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{°}=-0.76 \mathrm{V}$ and ${\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{°}=0.80 \mathrm{V}$

The standard electrode potential for Daniel cell is $1.1 \mathrm{V}.$ Calculate the standard Gibbs energy for the reaction:

$\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)⟶{\mathrm{Zn}}^{2+}+\mathrm{Cu}\left(\mathrm{s}\right)$

Calculate ${\mathrm{\Delta G}}^{\mathrm{\Theta }}$ and the equilibrium constant for the cell reaction:

${\mathrm{Cl}}_2+2{\mathrm{I}}^{-}⟶2{\mathrm{Cl}}^{-}+{\mathrm{I}}_2$

Given that ${\mathrm{E}}^{\mathrm{\Theta }}\left({\mathrm{Cl}}_2, {\mathrm{Cl}}^{-}\right)=1.36 \mathrm{V}; {\mathrm{E}}^{\mathrm{\Theta }}\left({\mathrm{I}}_2, {\mathrm{I}}^{-}\right)=0.536 \mathrm{V}$