State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced.
$C l_{2} + H_{2} S \to 2 H C l + S$

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Solution

Reduction: gain of hydrogen atom.
Chlorine gains hydrogen to form hydrogen chloride (HCl) on reacting with the hydrogen sulphide $(H_{2} S)$ . So, $C l_{2}$ gets reduced in this reaction.

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State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced.

(a) $P b O + C O \to P b + C O_{2}$

(b) $H_{2} S + C l_{2} \to 2 H C l + S$

M g + 2 H C l \to M g C l_{2} + H_{2}

Identify the compounds oxidised and reduced in the following reaction: H₂S + Cl₂ → 2HCl + S

H2S+Cl2=S+2HCl ,

which subtance is :

1)oxidised

2)reduced

3)the oxidising agent

4)the reducing agent

Give reasons?

H_{2} S + 2 F e C l_{3} \to 2 F e C l_{2} + 2 H C l + S

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