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B
2MnO−4+6H++3H2O2⟶2Mn2++6O2+8H2O
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C
4MnO−4+6H++5H2O2⟶2Mn2++5O2+8H2O
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D
None of these
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Solution
The correct option is A2MnO−4+6H++5H2O2⟶2Mn2++5O2+8H2O The unbalanced redox equation is as follows:
MnO−4+H++H2O2⟶Mn2++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 MnO−4 and Mn2+ with 2 and by multiplying H2O2 and O2 with 5.
2MnO−4+H++5H2O2⟶2Mn2++5O2
O atoms are balanced by adding 8 water molecules on RHS. 2MnO−4+H++5H2O2⟶2Mn2++5O2+8H2O
To balance H atoms, add 6 H+ on RHS. 2MnO−4+5H2O2+6H+⟶2Mn2++5O2+8H2O