Calculate ΔG° for the following redox reaction. 2 Al (s) + 3 Mg2+ (aq) → 2 Al3+ (aq) + 3 Mg (s)?

Refer to: https://www.drjez.com/uco/ChemTools/Standard%20Thermodynamic%20Values.pdf
G°[Al(s)] = 0 kJ/mol
G°[Mg²⁺(aq)] = -454.801 kJ/mol
G°[Al³⁺(aq)] = -485.344 kJ/mol
G°[Mg(s)] = 0 kJ/mol
(G° values from different sources may be slightly different.)

2Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3Mg(s)     ΔG°

ΔG° of the reaction
= 2G°[Al³⁺(aq)] + 3G°[Mg(s)] - 2G°[Al(s)] - 3G°[Mg²⁺(aq)]
= [2(-485.344) + 3(0) - 2(0) -3(-454.801)] kJ/mol
= +393.715 kJ/mol