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Valency and Oxidation States

Which one of ...

Question

Which one of the following reactions does not occur?

F_{2} + 2 C l^{-} \to 2 F^{-} + C l_{2}

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C l_{2} + 2 F^{-} \to 2 C l^{-} + F_{2}

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V r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}

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C l_{2} + 2 B r^{-} \to 2 C l^{-} + B r_{2}

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Solution

The correct option is B $C l_{2} + 2 F^{-} \to 2 C l^{-} + F_{2}$
$C l 2$ can not dissplace $F_{2}$ from because it is weakest oxidising agent than $F_{2}$ .
So $C l_{2} + 2 F^{-} \to 2 C l^{-} + F_{2}$ can not occur
Hence option B is correct.

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Similar questions

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 l_{2} + 2 B r^{-} (a q) ⟶ 2 C l^{-} (a q) + B r_{2}

[C l^{-}] = [B r_{2}] = [B r^{-}] = 0.01 M

C l_{2}

1

E^{o}

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

(x^{2} + y^{2})

x

y

C l_{2} + 2 I^{- 1} \to 2 C l^{-} + I_{2}

2 I^{-} + C l_{2} \to 2 C l^{-} + I_{2}

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