Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. b. KCl(aq) c. CuBr₂(aq)

Verified step by step guidance

1. Step 1: Identify the ions present in the aqueous solution of KCl. In KCl(aq), the ions are K⁺ and Cl⁻. Water (H₂O) is also present and can participate in the electrolysis reactions.
2. Step 2: Determine the possible half-reactions at the anode for KCl(aq). At the anode, oxidation occurs. The possible reactions are the oxidation of Cl⁻ to Cl₂ gas and the oxidation of water to oxygen gas.
3. Step 3: Write the half-reaction for the oxidation of Cl⁻ at the anode: 2Cl⁻(aq) → Cl₂(g) + 2e⁻. This reaction is more favorable than the oxidation of water under standard conditions.
4. Step 4: Identify the ions present in the aqueous solution of CuBr₂. In CuBr₂(aq), the ions are Cu²⁺ and Br⁻. Water is also present.
5. Step 5: Determine the possible half-reactions at the cathode for CuBr₂(aq). At the cathode, reduction occurs. The possible reactions are the reduction of Cu²⁺ to Cu(s) and the reduction of water to hydrogen gas. Write the half-reaction for the reduction of Cu²⁺ at the cathode: Cu²⁺(aq) + 2e⁻ → Cu(s). This reaction is more favorable than the reduction of water under standard conditions.