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Question

Identify oxidation & reduction reaction oxidising and reducing agent

  1. Pb3O4 + HCl ---------> Pbl2 + Cl2 + H2O
  2. CuSO4 +Zn --------> ZnSO4 + Cu
  3. Fe + S -------> FeS
  4. H2S + SO2 --------> H2O + S

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Solution

1.Pb3O4 + HCl ---------> PbCl2 + Cl2 + H2O is a redox reaction since oxidation number of Pb changes from +8/3 to +2 and Cl changes from -1 to 0

Oxidizing agent - Pb3O4

Reducing agent - HCl

2.CuSO4 + Zn → ZnSO4 + Cu is a redox reaction since oxidation number of Cu changes from +2 to 0 and Zn changes from 0 to +2

Oxidizing agent – CuSO4

Reducing agent – Zn

3.Fe + S → FeS is a redox reaction since oxidation number of Fe changes from 0 to +2 and S changes from 0 to -2.

Oxidizing agent – S

Reducing agent – Fe

4.H2S + SO2 → H2O + S is a redox reaction

Oxidation number of S changes from +4 in SO2 to 0 in S (S is reduced)
oxidation of S goes from -2 in H2S to 0 in S (S is oxidized)

H2S – reducing agent

SO2 – oxidizing agent


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