Identify the reducing and oxidising agents in the reaction:
PbS + 4H₂O₂ → PbSO₄ + 4H₂O

Open in App

Solution

1. Reaction
PbS + 4H₂O₂ → PbSO₄ + 4H₂O
Lead sulphide Hydrogen peroxide Lead Sulphate
2. Here oxidation state of S in PbS is -2 and that of O in H₂O₂ is -1 at reactant side but oxidation state of S in PbSO₄ is +6 and that of O in H₂O is -2.
So, we can say that PbS is getting oxidised since its oxidation number is increasing and H₂O₂ is getting reduced since its oxidation number is decreasing.
3. The one who gets oxidised acts as a reducing agent and the one who gets reduced acts as an oxidising agent.
So here PbS is a reducing agent and H₂O₂ is an oxidising agent.

Suggest Corrections

Similar questions

P b_{(s)} + P b O_{2 (s)} + 2 H_{2} S O_{4 (a q)} \to 2 P b S O_{4 (s)} + 2 H_{2} O_{(l)}

2 A g B r (s) + C_{6} H_{6} O_{2} (a q) \to 2 A g (s) + 2 H B r (a q) + C_{6} H_{4} O_{2} (a q)

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

Name the oxidizing and reducing agents in the following

PbS(S) + 4H2O2(aq) = PbSO4(s) + 4H2O(l)

Join BYJU'S Learning Program