Balance each redox reaction occurring in basic aqueous solution. c. Cl₂(g) → Cl^–(aq) + ClO^–(aq)

Verified step by step guidance

1. Identify the oxidation and reduction half-reactions. In this case, Cl2 is being reduced to Cl- and oxidized to ClO-. Write the half-reactions: Cl2 → Cl- and Cl2 → ClO-.
2. Balance the atoms other than oxygen and hydrogen in each half-reaction. For the reduction half-reaction, Cl2 → 2Cl-. For the oxidation half-reaction, Cl2 → ClO-.
3. Balance the oxygen atoms by adding H2O molecules. For the oxidation half-reaction, add one H2O to the right side: Cl2 → ClO- + H2O.
4. Balance the hydrogen atoms by adding OH- ions. For the oxidation half-reaction, add two OH- to the left side: Cl2 + 2OH- → ClO- + H2O.
5. Balance the charges by adding electrons. For the reduction half-reaction, add two electrons to the right side: Cl2 + 2e- → 2Cl-. For the oxidation half-reaction, add two electrons to the left side: Cl2 + 2OH- + 2e- → ClO- + H2O.