Balance the following equation -PbS-H2O2- PbSO4-H2O

Writing oxidation numbers of all the atoms, +2 2PbS++1 1H_2O_2→+2 +6 2PbSO_4++1 2H_2O The oxidation number of S has increased and O has decreased. 2PbS→+6 ...

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Byju's Answer

Standard XIII

Chemistry

Ion Electron Method

Balance the f...

Question

Balance the following equation :
$P b S + H_{2} O_{2} \to P b S O_{4} + H_{2} O$

2 P b S + 4 H_{2} O_{2} \to 2 P b S O_{4} + 4 H_{2} O

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P b S + 4 H_{2} O_{2} \to P b S O_{4} + 4 H_{2} O

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P b S + 2 H_{2} O_{2} \to P b S O_{4} + 2 H_{2} O

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2 P b S + 2 H_{2} O_{2} \to 2 P b S O_{4} + 4 H_{2} O

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Solution

The correct option is B $P b S + 4 H_{2} O_{2} \to P b S O_{4} + 4 H_{2} O$
Writing oxidation numbers of all the atoms,
$+ 2 - 2 P b S + + 1 - 1 H_{2} O_{2} \to + 2 + 6 - 2 P b S O_{4} + + 1 - 2 H_{2} O$
The oxidation number of $S$ has increased and $O$ has decreased.
$- 2 P b S \to + 6 P b S O_{4}$ ...(i)
$- 1 H_{2} O_{2} \to - 2 H_{2} O$ ...(ii)
Increase in oxidation number of $S$ = $8 u n i t s p e r P b S m o l e c u l e$
Decrease in oxidation number of $O = 1 u n i t p e r \frac{1}{2} H_{2} O_{2} m o l e c u l e$
$= 2 u n i t s p e r H_{2} O_{2} m o l e c u l e$
Multiplying eq. (ii) by $4$ as to make increase and decrease equal.
$P b S + 4 H_{2} O_{2} \to P b S O_{4} + 4 H_{2} O$

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Balance the following equation : PbS+H2O2→PbSO4+H2O

Balance the following equation :
$P b S + H_{2} O_{2} \to P b S O_{4} + H_{2} O$