Calculate ${\wedge }^0$ for ${\mathrm{CaCl}}_2$ and ${\mathrm{MgSO}}_4$ from the following data:

${\mathrm{\lambda }}_{{\mathrm{Ca}}^{2+}}^0=119.0 \mathrm{S}{ \mathrm{cm}}^2{ \mathrm{mol}}^{-1}; {\mathrm{\lambda }}_{{\mathrm{Mg}}^{2+}}^0=106 \mathrm{S} {\mathrm{cm}}^2{ \mathrm{mol}}^{-1}$

${\mathrm{\lambda }}_{{\mathrm{Cl}}^{-}}^0=76.3 \mathrm{S}{ \mathrm{cm}}^2{ \mathrm{mol}}^{-1}; {\mathrm{\lambda }}_{{\mathrm{SO}}_4^{2-}}^0=160.0 \mathrm{S}{ \mathrm{cm}}^2{ \mathrm{mol}}^{-1}$

For how long a current of $1.5$ amperes, has to be passed through the electrolyte in order to deposit $1.5 \mathrm{g}$ of $\mathrm{Al}$ , when the electrode reaction is

${\mathrm{Al}}^{3+}+3{\mathrm{e}}^{-}⟶\mathrm{Al}$   (Atomic mass of $\mathrm{Al}=27$)

How much charge is required for the following reduction of:

$1 \mathrm{mol}$ of ${\mathrm{Al}}^{3+}$ to $\mathrm{Al}$

How much charge is required for the following reduction of:$1 \mathrm{mol}$ of ${\mathrm{Cu}}^{2+}$ to $\mathrm{Cu}$?