Redox Reactions 3
Balance the following Redox reactions by the method of ½-reactions. Assume all
species are aqueous unless otherwise noted. Assume all are in acidic solution.
1. MnO4- + Cl-  Mn2+ + Cl2(g) in acidic solution.
2. Cr2O72- + I2  IO3- + Cr3+ in acidic solution.
3. SO2 + ClO4-  SO42- + Cl- in acidic solution.
4. Cr2O72- + C2O32-  Cr3+ + CO2 in acidic solution.
5. CH3OH(aq) + Cr2O72– (aq)  CH2O(aq) + Cr3+(aq) in acidic solution.
6.
S2(aq) + I2(aq)  SO42(aq) + I(aq) in basic solution.
7. CO + I2O5  I2 + CO2 in acidic solution.
8. HNO3 + KBr  NO(g) + Br2 + KNO3 in acidic solution.
9. Mn2+(aq) + NaBiO3(s)  Bi3+(aq) + MnO4(aq) + Na+ in acidic solution.
10.Br2(aq) + SO2(aq)  Br(aq) + SO42(aq) in basic solution.
11. S8(s) + H2SO4(aq)  SO2(g) (Consider, is this acidic or basic solution?)
12. CrI3(s) + Cl2(g)  CrO42(aq) + IO4(aq) + Cl(aq) in acidic solution.