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Oxidising Reagent and Reducing Reagent

In the follow...

Question

In the following reactions, identify the species oxidised, the species reduced, the oxidising agent and the reducing agent.
$S n C l_{2} + 2 F e C l_{3} \to S n C l_{4} + 2 F e C l_{2}$ .

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Solution

$S n C l_{2} + 2 F e C l_{3} = S n C l_{4} + 2 F e C l_{2}$
Writing the oxidation numbers on various atoms,
$+ 2 S n - 1 C l_{2} + + 3 2 F e - 1 C l_{3} = + 4 S n - 1 C l_{4} + + 2 2 F e - 1 C l_{2}$
Ox. no. of $S n$ changes from $+ 2$ to $+ 4$ , i.e., increase in oxidation number. $S n C l_{2}$ is thus oxidised or it acts as a reducing agent.
Ox. no. of $F e$ changes from $+ 3$ to $+ 2$ , i.e., decrease in oxidation number. $F e C l_{3}$ is thus reduced or it acts as an oxidising agent.

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