1. **Stating the problem:** Balance the chemical equation and identify which species undergo reduction, oxidation, or act as spectator ions. 2. **Equation 1:** $$\_\_\_\_ \text{AgCl} + \_\_\_\_ \text{Na} \rightarrow \_\_\_\_ \text{Ag} + \_\_\_\_ \text{NaCl}$$ 3. **Balancing Equation 1:** - Silver (Ag) and chlorine (Cl) appear once on each side. - Sodium (Na) appears only on reactants and products. - Balanced form: $$\text{AgCl} + \text{Na} \rightarrow \text{Ag} + \text{NaCl}$$ (coefficients all 1) 4. **Identify oxidation states:** - Ag in AgCl is +1, Cl is -1. - Na is 0 (elemental), Na in NaCl is +1. - Ag in elemental form is 0. 5. **Determine oxidation/reduction:** - Ag: +1 to 0 (gain of electrons) → Reduction. - Na: 0 to +1 (loss of electrons) → Oxidation. - Cl: -1 remains -1 → Spectator ion. 6. **Equation 2:** $$\_\_\_\_ \text{Cl}_2 + \_\_\_\_ \text{KI} \rightarrow \_\_\_\_ \text{KCl} + \_\_\_\_ \text{I}_2$$ 7. **Balancing Equation 2:** - Cl atoms: 2 on left, 1 on right → coefficient 2 for KCl. - I atoms: 1 in KI, 2 in I2 → coefficient 2 for KI. - Balanced form: $$\text{Cl}_2 + 2\text{KI} \rightarrow 2\text{KCl} + \text{I}_2$$ 8. **Identify oxidation states:** - Cl in Cl2 is 0, in KCl is -1. - I in KI is -1, in I2 is 0. 9. **Determine oxidation/reduction:** - Cl: 0 to -1 → Reduction. - I: -1 to 0 → Oxidation. - K: +1 remains +1 → Spectator ion. **Final answers:** Equation 1 coefficients: AgCl=1, Na=1, Ag=1, NaCl=1 - AgCl: Spectator ion (Cl), Ag: Reduction, Na: Oxidation Equation 2 coefficients: Cl2=1, KI=2, KCl=2, I2=1 - Cl2: Reduction, KI: Oxidation (I), K: Spectator ion