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Question

Write balanced redox reactions of the following:

H2O2(aq) reduces Cr2O27(aq) to green coloured Cr3+(aq) in acidic medium.

A
Cr2O27+3H2O2+8H+2Cr3++3O2+7H2O
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B
Cr2O29+3H2O2+4H+2Cr3++3O2+7H2O
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C
Cr2O27+3H2O2+8H+2Cr3++3O2+9H2O
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D
None of these
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Solution

The correct option is B Cr2O27+3H2O2+8H+2Cr3++3O2+7H2O
H2O2(aq) reduces Cr2O27(aq) to green coloured Cr3+(aq) in acidic medium.

The unbalanced redox equation is as follows:
Cr2O27+H2O2Cr3++O2

Balance all atoms other than H and O.
Cr2O27+H2O22Cr3++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.

Cr2O27+3H2O22Cr3++3O2

To balance O atoms, add 7 water molecules on RHS.

Cr2O27+3H2O22Cr3++3O2

To balance H atoms, add 8 H+ on LHS.

Cr2O27+3H2O2+8H+2Cr3++3O2+7H2O

This is the balanced chemical equation.

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