Write a balanced chemical equation describing the oxidation of cl2 gas by cu3+ to form chlorate ion (clo3-) and cu2+ in an acidic aqueous solution. use the smallest whole-number coefficients possible and indicate states of matter in your balanced reaction.

Cl2(g) + 10 Cu3+(aq) + 6H2O(l) → 2 ClO3(aq) + 10 Cu2+(aq) + 12 H+(aq)

Explanation:

Step 1: The half reactions

Cl2(g) + 6H20(l) ⇆ 2ClO3-(aq) +12H+(aq) +10e-

Cu3+(aq) +e- ⇆ Cu2+(aq)

Step 2: Balance the reactions

To balance the electron transfers, we have to multiply the second equation by 10

Cl2(g) + 6H20(l) ⇆ 2ClO3-(aq) +12H+(aq) +10e-

10 Cu3+(aq) +10e- ⇆ 10 Cu2+(aq)

Step 3: The netto reaction

Cl2(g) + 10 Cu3+(aq) + 6H2O(l) → 2 ClO3(aq) + 10 Cu2+(aq) + 12 H+(aq)