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in Oxidation-Reduction Reactions by (49.3k points)

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

1 Answer

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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.

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