TASK 1Justify the reaction: 2Cu₂O (s) + Cu₂S (s) · → 6Cu (s) + SO2 (g) is a redox reaction. Cuprous oxide + cuprous sulfide = Copper + sulfur dioxide Identify the species oxidized, and reduced, which acts as an oxidant and which acts as a reductant. TASK 1.2 Identify which of the following is an oxidizing agent or reducing agent. 1. CIO₁- → CIO₂2. SO 2 →S23.Mn2+ → MnO₂ 4. Zn → ZnCl₂ 5. 2Na+ Cl2 → 2NaCl TASK 2Identify which is the oxidized and reduced species and also the oxidizing and reducing agents in each chemical equation. 1. 4AI+30. = 2AIO. Aluminum + oxygen = Aluminum oxide 2. HSCIS + 2HCI . Hydrogen sulfide + Chlorine = Sulfur + Hydrochloric acid 3. 2CUSO. + 4KI = 2Cul + I + 2K.SO. • Copper sulfate + Potassium iodide = Copper iodide + lodine + Potassium sulfate 4. 3PbO+2NH. N. + 3HO + 3Pb • Lead oxide + Ammonia = Nitrogen + Water + Lead 5. MnO2+4HCI = MnCl2 + Cl2 + 2H,O Manganese oxide + Hydrochloric acid = Manganese chloride + Chlorine + water(I need help with this one again po!)
Answer (1)
Answer:TASK 1 Justification: The reaction 2Cu₂O (s) + Cu₂S (s) → 6Cu (s) + SO₂ (g) is a redox reaction because it involves the transfer of electrons between the reactants. Identification: - Oxidized species: Cu₂S (s) - Sulfur in Cu₂S is oxidized from a -2 oxidation state to +4 in SO₂.- Reduced species: Cu₂O (s) - Copper in Cu₂O is reduced from +1 oxidation state to 0 in Cu.- Oxidant: Cu₂O (s) - It accepts electrons and causes the oxidation of Cu₂S.- Reductant: Cu₂S (s) - It donates electrons and causes the reduction of Cu₂O. TASK 1.2 1. CIO₁- → CIO₂ - Oxidizing agent: CIO₁- - Chlorine in CIO₁- is reduced from +7 oxidation state to +4 in CIO₂. 2. SO₂ → S²⁻ - Reducing agent: SO₂ - Sulfur in SO₂ is reduced from +4 oxidation state to -2 in S²⁻. 3. Mn²⁺ → MnO₂ - Oxidizing agent: Mn²⁺ - Manganese in Mn²⁺ is oxidized from +2 oxidation state to +4 in MnO₂. 4. Zn → ZnCl₂ - Reducing agent: Zn - Zinc in Zn is oxidized from 0 oxidation state to +2 in ZnCl₂. 5. 2Na + Cl₂ → 2NaCl - Oxidizing agent: Cl₂ - Chlorine in Cl₂ is reduced from 0 oxidation state to -1 in NaCl.- Reducing agent: Na - Sodium in Na is oxidized from 0 oxidation state to +1 in NaCl. TASK 2 1. 4Al + 3O₂ = 2Al₂O₃ - Oxidized species: Al - Aluminum is oxidized from 0 to +3.- Reduced species: O₂ - Oxygen is reduced from 0 to -2.- Oxidizing agent: O₂ - Oxygen accepts electrons.- Reducing agent: Al - Aluminum donates electrons. 2. H₂S + 2Cl₂ = S + 2HCl - Oxidized species: H₂S - Sulfur is oxidized from -2 to 0.- Reduced species: Cl₂ - Chlorine is reduced from 0 to -1.- Oxidizing agent: Cl₂ - Chlorine accepts electrons.- Reducing agent: H₂S - Hydrogen sulfide donates electrons. 3. 2CuSO₄ + 4KI = 2CuI + I₂ + 2K₂SO₄ - Oxidized species: I⁻ - Iodide is oxidized from -1 to 0.- Reduced species: Cu²⁺ - Copper is reduced from +2 to +1.- Oxidizing agent: CuSO₄ - Copper sulfate accepts electrons.- Reducing agent: KI - Potassium iodide donates electrons. 4. 3PbO + 2NH₃ = N₂ + 3H₂O + 3Pb - Oxidized species: N in NH₃ - Nitrogen is oxidized from -3 to 0.- Reduced species: PbO - Lead is reduced from +2 to 0.- Oxidizing agent: PbO - Lead oxide accepts electrons.- Reducing agent: NH₃ - Ammonia donates electrons. 5. MnO₂ + 4HCl = MnCl₂ + Cl₂ + 2H₂O - Oxidized species: Cl⁻ in HCl - Chlorine is oxidized from -1 to 0.- Reduced species: MnO₂ - Manganese is reduced from +4 to +2.- Oxidizing agent: MnO₂ - Manganese oxide accepts electrons.- Reducing agent: HCl - Hydrochloric acid donates electrons.
