Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

+6.8 x 102 kJ
-7.8 x 102 kJ
+4.1 x 102 kJ
+1.4 x 102 kJ
-2.3 x 102 kJ
Answer is 4.1-10^2 kJ

Please explain every details

When I did it, I got the potential energy -2.37+(-1.66)=-4.03

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: