Practice Problems: Redox Reactions


  1. Determine the oxidation number of the elements in each of the following compounds:

    a. H2CO3

    b. N2

    c. Zn(OH)42-

    d. NO2-

    e. LiH

    f. Fe3O4

    Hint


  2. Identify the species being oxidized and reduced in each of the following reactions:

    a. 2 Cr+ + Sn4+ Cr3+ + Sn2+

    b. 3 Hg2+ + 2 Fe (s) 3 Hg2 + 2 Fe3+

    c. 2 As (s) + 3 Cl2 (g) 2 AsCl3

    Hint


  3. Would you use an oxidizing agent or reducing agent in order for the following reactions to occur?

    a. ClO3- ClO2

    b. SO42- S2-

    c. Mn2+ MnO2

    d. Zn ZnCl2

    Hint


  4. Write balance equations for the following redox reactions:

    a. NaBr + Cl2 NaCl + Br2

    b. Fe2O3 + CO Fe + CO2 in acidic solution

    c. CO + I2O5 CO2 + I2 in basic solution

    Hint


  5. Write balanced equations for the following reactions: Hint

    a. Cr(OH)3 + Br2 CrO42- + Br- in basic solution

    b. O2 + Sb H2O2 + SbO2- in basic solution Hint

    c. HCOOH + MnO4- CO2 + Mn2+ in acidic solution

    d. ClO2- ClO2 + Cl- in acidic solution Hint



  6. Write the balanced half reactions of the following reactions:

    a. NiO2 + 2 H2O + Fe Ni(OH)2 + Fe(OH)2 in basic solution

    b. CO2 + 2 NH2OH CO + N2 + 3 H2O in basic solution

    c. 2 H+ + H2O2 + 2 Fe2+ 2 Fe3+ + 2 H2O in acidic solution

    d. H+ + 2 H2O + 2 MnO4- + 5 SO2 2 Mn2+ + 5 HSO4- in acidic solution

    Hint



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