Br in BrO- has oxidation state of +1
Br in Br- has oxidation state of -1
So, Br in BrO- is reduced to Br-
This means BrO- is oxidising agent
Fe in Fe has oxidation state of 0
Fe in Fe+3 has oxidation state of +3
So, Fe in Fe is oxidised to Fe+3
This means Fe is reducing agent
Reduction half cell:
BrO- + 2e- --> Br-
Oxidation half cell:
Fe --> Fe+3 + 3e-
Balance number of electrons to be same in both half reactions
Reduction half cell:
3 BrO- + 6e- --> 3 Br-
Oxidation half cell:
2 Fe --> 2 Fe+3 + 6e-
Lets combine both the reactions.
3 BrO- + 2 Fe --> 3 Br- + 2 Fe+3
Balance Oxygen by adding water
3 BrO- + 2 Fe --> 3 Br- + 2 Fe+3 + 3 H2O
Balance Hydrogen by adding H+
3 BrO- + 2 Fe + 6 H+ --> 3 Br- + 2 Fe+3 + 3 H2O
Add equal number of OH- on both sides as the number of H+
3 BrO- + 2 Fe + 6 H+ + 6 OH- --> 3 Br- + 2 Fe+3 + 3 H2O + 6 OH-
Combine H+ and OH- to form water
3 BrO- + 2 Fe + 6 H2O --> 3 Br- + 2 Fe+3 + 3 H2O + 6 OH-
Remove common H2O from both sides
Balanced Eqn is
3 BrO- + 2 Fe + 3 H2O --> 3 Br- + 2 Fe+3 + 6 OH-
This is balanced chemical equation in basic medium
Answer:
3 BrO-(aq) + 2 Fe(s) + 3 H2O(l) -> 3 Br-(aq) + 2 Fe3+(aq) + 6 OH-(aq)
BrO- is oxidising agent
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show work
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