What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? al(s) | al3+(aq) || fe2+(aq) | fe(s) what is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? al(s) | al3+(aq) || fe2+(aq) | fe(s) 3 fe(s) + 2 al3+(aq) → 3 fe2+(aq) + 2 al(s) 2 fe(s) + 3 al3+(aq) → 2 fe2+(aq) + 3 al(s) 3 al(s) + 2 fe2+(aq) → 3 al3+(aq) + 2 fe(s) 2 al(s) + 3 fe2+(aq) → 2 al3+(aq) + 3 fe(s)

2Al(s) + 3Fe⁺²(Aq) → 2Al⁺³(aq) + 3Fe(s)

Explanation:

The shorthand notation first places the oxidation reaction and then the reduction reaction. So, the half-reactions are:

Al(s) → Al⁺³(aq) + 3e⁻     (Al must lose 3 electrons)

Fe⁺²(Aq) + 2e⁻ → Fe (s)  (Fe⁺² must gain 2 electrons)

The total amount of electrons must be equal, so the first equation must be multiplied by 2, and the second by 3:

2Al(s) → 2Al⁺³(aq) + 6e⁻

3Fe⁺²(Aq) + 6e⁻ → 3Fe (s)

And now they must be summed, which will be the balanced chemical equation:

2Al(s) + 3Fe⁺²(Aq) → 2Al⁺³(aq) + 3Fe(s)

i do not get it   at all