Consider a galvanic cell in which Al 3 + Al3+ is reduced to elemental aluminum and magnesium metal is oxidized to Mg 2 + Mg2+ . Write the balanced half-cell reactions that take place at the cathode and at the anode.

Anode:

3Mg(s) > 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e > 2Al(s)

Explanation:

Anode:

3Mg(s) > 3Mg2+(aq) + 6e

Cathode:

2Al3+(aq) +6e > 2Al(s)

Magnesium is more electro positive than aluminum hence it functions as the anode. Six electrons are lost/gained in the redox process as shown in the oxidation and reduction half reaction equations above. Magnesium is oxidized to magnesium ion while aluminum is reduced to elemental aluminum.

answer; i believe that the correct answer is (a) potassium(k)