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Question

Balance the following redox reaction:

MnO4+H++H2O2Mn2++O2

A
2MnO4+6H++5H2O22Mn2++5O2+8H2O
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B
2MnO4+6H++3H2O22Mn2++6O2+8H2O
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C
4MnO4+6H++5H2O22Mn2++5O2+8H2O
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D
None of these
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Solution

The correct option is A 2MnO4+6H++5H2O22Mn2++5O2+8H2O
The unbalanced redox equation is as follows:

MnO4+H++H2O2Mn2++O2

All atoms other than H and O are balanced.
The oxidation number of Mn changes from 7 to 2. The change in the oxidation number of Mn is 5.

The oxidation number of O changes from -1 to -2. The change in the oxidation number per O atom is 1. Total change in the oxidation number for 2 O atoms is 2.

The increase in the oxidation number is balanced with a decrease in the oxidation number by multiplying MnO4 and Mn2+ with 2 and by multiplying H2O2 and O2 with 5.

2MnO4+H++5H2O22Mn2++5O2

O atoms are balanced by adding 8 water molecules on RHS.
2MnO4+H++5H2O22Mn2++5O2+8H2O

To balance H atoms, add 6 H+ on RHS.
2MnO4+5H2O2+6H+2Mn2++5O2+8H2O

This is the balanced chemical equation.

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