State whether the following conversions are oxidation or reduction reactions.
$2 C l^{-} \to C l_{2} + 2 e^{-}$

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Solution

Oxidation: A process in which the oxidation state of an atom or ion increases by losing electrons.

In the given reaction oxidation state of chlorine increases from -1 to 0. So, chlorine gets oxidized.

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Divide the following redox reactions into oxidation and reduction half reactions.

(i) $Z n + P b^{2} \to Z n^{2} + P b$

(ii) $Z n + C u^{2 +} \to Z n^{2} + C u$

(iii) $C l_{2} + 2 B r^{-} \to B r_{2} + 2 C l^{-}$

C u^{2}^{+} + 2 e^{-} \to C u

P b O_{2} + {S O}_{2} \to P b {S O}_{4}

C l_{2} + 2 e^{-} \to 2 C l^{-}

P t^{2 +} + 2 C l^{-} \to P t + C l_{2}, E_{cell}^{o} = - 0.15 V

P t^{2 +} + 2 e^{-} \to P t, E^{o} = 1.20 V

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