Question

Identify oxidising and reducing agent in the following:
(i) 3I₂ + NaOH ➝ NaIO₃ + 5NaI + 3H₂O
(ii) AlCl₃ + 3K ➝ Al + 3KCl
(iii) SO₂ + 2H₂S ➝ 3S + 2H₂O
(iv) SnCl₂ + 2FeCl₃ ➝ SnCl₄ + 2FeCl₂
(v) H₂O₂ + H₂O₂ ➝ 2H₂O + O₂

Answer 1

In this reaction, iodine (I₂) is oxidised to NaIO₃ and also reduced to Nal. So, it acts as both oxidising and reducing agent.

In this reaction, potassium (K) reduces AlCl₃ to Al, So it acts as reducing agent and AlCl₃ oxidises K to KCl, so it acts as oxidising agent
Oxidising agent = AlCl₃
Reducing agent = K

In this reaction, SO₂ oxidises H₂S to S, so it acts as oxidising agent and H₂S reduces SO₂ to S, so it acts as reducing agent.
SO₂ = Oxidising agent
H₂S = Reducing agent

In this reaction, FeCl₃ oxidises SnCl₂ to SnCl₄, so it acts as oxidising agent and SnCl₂ reduces FeCl₃ to FeCl₂, so it acts as reducing agent.
FeCl₃ = Oxidising agent
SnCl₂ = Reducing agent

In this reaction, one molecule of H₂O₂ is oxidised to O₂ and another molecule of H₂O₂ is reduced to H₂O. So, H₂O₂ acts as both oxidising and reducing agent.