Question

Balance each of the following redox reactions occurring in basic solution.

a)H2O2(aq)+ClO2(aq)→ClO−2(aq)+O2(g)

Express your answer as a chemical equation. Identify all of the phases in your answer.

b) Al(s)+MnO−4(aq)→MnO2(s)+Al(OH)−4(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. c) Cl2(g)→Cl−(aq)+ClO−(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

(a) H₂O₂(aq)+ClO₂(aq)→ ClO−2(aq)+ O₂(g)

Cl is going from +4 oxidation state to +3 oxidation state (Reduction)

Oxygen in H2O2 is going from -1 oxidation state to zero oxidation state (Oxidation)

Reduction half cell: ClO2 + e- ClO2-

Oxidation half cell: H2O2 O2 + 2e-

Multiply reduction half cell by 2 to cancel electrons in overall reaction, we get 2 ClO2 + 2 e- 2 ClO2-

Now add the oxidation and reductions reactions:

H2O2 + 2ClO2 2ClO2- + O2

Since the solution is basic , we use OH- and H₂O to balance

H2O2 (aq) + 2 ClO2 (aq) + 2 OH- (aq) 2 ClO2- (aq) + O2 (g) + 2 H2O (l)