The cell reaction is spontaneous or feasible when emf of the cell is:

Calculate the mass of silver deposited at cathode when a current of $2$ amperes is passed through a solution of ${\mathrm{AgNO}}_3$ for $15$ minutes. (atomic mass: $\mathrm{Ag}=108, 1 \mathrm{F}=96,500 \mathrm{C}$).

Calculate the emf and $∆\mathrm{G}$ for the cell reaction at $298 \mathrm{K}$·

The resistance of a conductivity cell containing $0.001 \mathrm{M} \mathrm{KCl}$ solution at $298 \mathrm{K}$ is $1500 \mathrm{ohm}$. What is the cell constant and molar conductivity of $0.001 \mathrm{M} \mathrm{KCl}$ solution, if the conductivity of this solution is $0.146\times {10}^{-3} {\mathrm{ohm}}^{-1}{\mathrm{cm}}^{-1}$ at $298 \mathrm{K}$?

Calculate the emf and $\mathrm{\Delta G}$ for the given cell at $25 °\mathrm{C}$: $\mathrm{Cr}\left(\mathrm{s}\right)/{\mathrm{Cr}}^{3+}\left(0.1 \mathrm{M}\right)//{\mathrm{Fe}}^{2+}\left(0.01 \mathrm{M}\right)/\mathrm{Fe}\left(\mathrm{s}\right).$

Given: ${\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^{°}=-0.74 \mathrm{V}; {\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{°}=-0.44 \mathrm{V}; [1\mathrm{F}=96500 \mathrm{C}; \mathrm{R}=8.314 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}]$.

Calculate the degree of dissociation $(\propto )$ of acetic acid, if its molar conductivity $\left({\mathrm{Ʌ}}_{\mathrm{m}}\right)$ is $39.05 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$. 

Given: $\mathrm{\lambda }{°}_{\left({\mathrm{H}}^{+}\right)}=349.6 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$ and $\mathrm{\lambda }{°}_{\left({\mathrm{CH}}_3{\mathrm{COO}}^{-}\right)}=40.9 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$.