Determine the number of water molecules necessary to balance the reduction half reaction of
___ MnO4-(aq) → ___ MnO2(s) that occurs in a basic solution.
Mn in MnO4- has oxidation state of +7
Mn in MnO2 has oxidation state of +4
So, Mn in MnO4- is reduced to MnO2
MnO4- + 3e- --> MnO2
Balance Oxygen by adding water
MnO4- + 3e---> MnO2 + 2 H2O
Balance Hydrogen by adding H+
MnO4- + 4 H+ + 3e- --> MnO2 + 2 H2O
Add equal number of OH- on both sides as the number of H+
MnO4- + 4 H+ + 4 OH- + 3e- --> MnO2 + 2 H2O + 4 OH-
Combine H+ and OH- to form water
MnO4- + 4 H2O + 3e- --> MnO2 + 2 H2O + 4 OH-
Remove common H2O from both sides
Balanced Eqn is
MnO4- + 2 H2O + 3e- --> MnO2 + 4 OH-
This is balanced chemical equation in basic medium
Answer:
MnO4- + 2 H2O + 3e- --> MnO2 + 4 OH-
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