Oxidation-Reduction Practice Problems

The following questions are designed to practice rudimentary oxidation-reduction. They start with balancing chemical reactions and move on to determining oxidation states of individual compounds. They then go on to determining which element is being oxidized and reduced in a chemical reaction.

  1. Balance the following equations:
    1. __ Fe + __ Cl2 → __ FeCl3
    2. __ KMnO4 + __ HCl → __ KCl + __ MnCl2 + __ H2O + __ Cl2
    3. __ K4Fe(CN)6 + __ H2SO4 + __ H2O → __ K2SO4 + __ FeSO4 + __ (NH4)2SO4 + __ CO
    4. __ C6H5COOH + __ O2 → __ CO2 + __ H2O
    5. __ K4Fe(CN)6 + __ KMnO4 + __ H2SO4 → __ KHSO4 + __ Fe2(SO4)3 + __ MnSO4 + __ HNO3 + __ CO2 + __ H2O
  1. Determine the oxidation state of each of the elements in the following compounds below:
    1. H2O
    2. O2
    3. NaCl
    4. Fe3O4
    5. N2O
    6. AsCl3
    7. NaNO3
    8. Zn(OH)­42-
  2. Determine which element is being oxidized and which element is being reduced:
    1. Al + NO2 → Al(OH)4 + NH3
    2. Sn + NO2 → SnO2 + NO
    3. Fe2O3 + 3CO → 2Fe + 3CO2
    4. ClO3 + Cl → Cl2 + ClO2
    5. Fe2O3 + 3CO → 2Fe + 3CO2
    6. MnO4 + HSO3 → MnO42- + SO42-
    7. Mn2+ + BiO3 → MnO4 + Bi3+
    8. MnO4 + HSO3 → MnO42- + SO42-

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