Predict the oxidizing agent and reducing agent in the following reaction:
PbS(s) + 4H2O2(aq) ? PbSO4(s) +4H2O (l)

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Solution

Dear student, PbS is a reducing agent (reducing agent loses electron), H2O2 is an oxidizing agent(gains electron) S-II - 8 e- â†’ SVI (Oxidation: atom loses its electron) 8 O-I + 8 e- â†’ 8 O-II (reduction: atom gains electron). Regards,

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In the following reaction between lead sulphide adn hydrogen peroxide :

$P b S (s) + 4 H_{2} O_{2} (a q) ⟶ P b S O_{4} (s) + 4 H_{2} O (l)$

(a) which substance is reduced ?

(b) Which substance is oxidised ?

5 H_{2} O_{2} + B r_{2} ⟶ 2 H B r O_{3} + 4 H_{2} O

Hydrogen peroxide in its reaction with $K I O_{4}$ and $N H_{2} O H$ respectively, is acting as:

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