Can you store copper sulphate solutions in a zinc pot?

The standard free energy change $(\Delta G^{\circ})$ for the following reaction (in $kJ$) at $25^{\circ} C$ is $3 Ca_{(s)} + 2 Au^{3+}(aq, 1 M) \rightarrow 3 Ca^{2+}(aq, 1 M) + 2 Au_{(s)}$ (given: $E^{\circ}_{Au^{3+}/Au} = +1.50 \ V, E^{\circ}_{Ca^{2+}/Ca} = -2.87 \ V, 1 \ F = 96500 \ C \ mol^{-1}$)

The following limiting molar conductivities are given as:
$\lambda_{m(H_{2}SO_{4})}^{0} = x \ S \ cm^{2} mol^{-1}$
$\lambda_{m(K_{2}SO_{4})}^{0} = y \ S \ cm^{2} mol^{-1}$
$\lambda_{m(CH_{3}COOK)}^{0} = z \ S \ cm^{2} mol^{-1}$
The $\lambda_{m}^{0} \ (\text{in } S \ cm^{2} mol^{-1})$ for $CH_{3}COOH$ will be:

Calculate $\Delta G^{\circ}$ for the reaction $Mg_{(s)} + Sn_{(aq)}^{2+} \longrightarrow Mg_{(aq)}^{2+} + Sn_{(s)}$ if $E_{cell}^{\circ}$ is $2.23 \ V$. (in $kJ$)

Given $\lambda^{\circ}_{Mg^{2+}} = 106 \ S \ cm^2 \ mole^{-1}$ and $\lambda^{\circ}_{SO_4^{2-}} = 160 \ S \ cm^2 \ mole^{-1}$. The value of $\lambda^{\circ}_{MgSO_4}$ (in $S \ cm^2 \ mole^{-1}$) is

Arrange the following metals in the order in which they displace each other from the solution of their salts: $Al$,$Cu$,$Fe$,$Mg$,and $Zn$.