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Question

Balance the following equation :
PbS+H2O2PbSO4+H2O

A
2PbS+4H2O22PbSO4+4H2O
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B
PbS+4H2O2PbSO4+4H2O
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C
PbS+2H2O2PbSO4+2H2O
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D
2PbS+2H2O22PbSO4+4H2O
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Solution

The correct option is B PbS+4H2O2PbSO4+4H2O
Writing oxidation numbers of all the atoms,
+2 2PbS++11H2O2+2 +6 2PbSO4++12H2O
The oxidation number of S has increased and O has decreased.
2PbS+6PbSO4 ...(i)
1H2O2 2H2O ...(ii)
Increase in oxidation number of S = 8 units per PbS molecule
Decrease in oxidation number of O=1 unit per 12H2O2 molecule
=2 units per H2O2 molecule
Multiplying eq. (ii) by 4 as to make increase and decrease equal.
PbS+4H2O2PbSO4+4H2O

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