The correct option is
B Cr2O2−7+3H2O2+8H+⟶2Cr3++3O2+7H2OH2O2(aq) reduces
Cr2O2−7(aq) to green coloured
Cr3+(aq) in acidic medium.
The unbalanced redox equation is as follows:
Cr2O2−7+H2O2⟶Cr3++O2
Balance all atoms other than H and O.
Cr2O2−7+H2O2⟶2Cr3++O2
The oxidation number of Cr changes from 6 to 3. The change in the oxidation number per Cr atom is 3. For 2 Cr atoms, the change in the oxidation number is 6.
The oxidation number of O changes from -1 to 0. The change in the oxidation number per O atom is 1. For 2 O atoms, the change in the oxidation number is 2.
To balance the increase in the oxidation number with a decrease in the oxidation number multiply H2O2 and O2 with 3.
Cr2O2−7+3H2O2⟶2Cr3++3O2
To balance O atoms, add 7 water molecules on RHS.
Cr2O2−7+3H2O2⟶2Cr3++3O2
To balance H atoms, add 8 H+ on LHS.
Cr2O2−7+3H2O2+8H+⟶2Cr3++3O2+7H2O
This is the balanced chemical equation.