Use the tabulated half$-$cell potentials to calculate $G$ for the following redox reaction.

$2Al(s)+3M{g}^{2+}(aq)2A{l}^{3+}(aq)+3Mg(s)$

$M{g}^{2+}(aq)+2e^{-}Mg(s),E=-2\mathrm{.}37V$

$A{l}^{3+}(aq)+3e^{-}Al(s),E=-1\mathrm{.}66V$

$+2\mathrm{.}1{10}^{2}kJ$

$-7\mathrm{.}8{10}^{2}kJ$

$+1\mathrm{.}4{10}^{2}kJ$

$+4\mathrm{.}1{10}^{2}kJ$

$+2\mathrm{.}3{10}^{3}kJ$

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