Balance the follo

The oxidation number of Cl decreases from + 7 in Cl₂O₇ to + 3 in and the oxidation number of ClO₂^- increases from – 1 in H₂O₂ to zero in O₂. Hence, in this reaction, Cl₂O₇ is the oxidizing agent and H₂O₂ is the reducing agent as could be clearly seen in the figure below: -

Solving by ion–electron method:

The oxidation half equation is:-

The oxidation number is balanced by adding 2 electrons as:-

The charge is balanced by adding 2OH^- ions as:-

The oxygen atoms are balanced by adding 2H₂O as:-

The reduction half equation is:-

The Cl atoms are balanced as:-

The oxidation number is balanced by adding 8 electrons as:-

The charge is balanced by adding 6OH^- as:-

The oxygen atoms are balanced by adding 3H₂O as:-

Multiplying the oxidation half reaction by 4 and then adding it to the reduction half reaction, we get the net balanced reaction equation as:-

Solving by oxidation number method:

Total decrease in oxidation number of Cl₂O₇= 4 × 2 = 8 Total increase in oxidation number of H₂O₂ = 2 × 1 = 2 .Now multiplying H₂O₂ and O₂ with 4 to balance the increase and decrease in the oxidation number, we get:

The Cl atoms are balanced as:-

The O atoms are balanced by adding 3H₂O as:-

The H atoms are balanced by adding 2OH^- and 2H₂O to get the desired balance equation :-