In: Chemistry
Balance the following redox reaction in acidic solution. Br? (aq) + MnO2 (s) ? Br2 (l) + Mn+2 (aq)
Unbalanced equation
Br- + MnO2 Br2 + Mn2+
Separate the redox reaction into half-reactions.
Oxidation
Br- Br2
Reduction
MnO2 Mn2+
Balance all other atoms except hydrogen and oxygen
Oxidation
2Br- Br2
Reduction
MnO2 Mn2+
Balance the oxygen atoms.
Oxidation
2Br- Br2
Reduction
MnO2 Mn2+ + 2H2O
Balance the hydrogen atoms.
Oxidation
2Br- Br2
Reduction
MnO2 + 4H+ Mn2+ + 2H2O
Balance the charge.
Oxidation
2Br- Br2 + 2e-
Reduction
MnO2 + 4H+ + 2e- Mn2+ + 2H2O
Make electron gain equivalent to electron lost.
Oxidation
2Br- Br2 + 2e-
Reduction
MnO2 + 4H+ + 2e- Mn2+ + 2H2O
Add the half-reactions together.
2Br- + MnO2 + 4H+ +
2e-
Br2 + Mn2+ + 2e- +
2H2O
Simplify the
equation.
2Br-(aq) + MnO2(s) + 4H+(aq) Br2(l) + Mn2+(aq) + 2H2O(l)