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Application of Electrolysis

Which of the ...

Question

Which of the following reactions takes place in (ii)?

A

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

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B

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

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C

I_{3}^{-} + 8 C I_{2} + 9 H_{2} O \to 3 I O_{3}^{-} + 16 C l^{-} + 18 H^{+}

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D

B r_{3}^{-} + 8 C I_{2} + 9 H_{2} O \to 3 B r O_{3}^{-} + 16 C l^{-} + 18 H^{+}

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Solution

The correct option is C $I_{3}^{-} + 8 C I_{2} + 9 H_{2} O \to 3 I O_{3}^{-} + 16 C l^{-} + 18 H^{+}$
Reaction is $I_{3}^{-} + 8 C I_{2} + 9 H_{2} O \to 3 I O_{3}^{-} + 16 C l^{-} + 18 H^{+}$

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Similar questions

Q. Which substance/ion is oxidised and which substance/ion is reduced in the following reaction?

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

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

I_{2} + 2 e^{-} \to 2 I^{-} standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-} standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Which of the following reaction(s) is/are spontaneous:

I_{2} + 2 e^{-} \to 2 I^{-}, standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-}, standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?

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

F e + B r_{2} \to F e^{2 +} + 2 B r^{-}

F e + I_{2} \to F e^{2 +} + 2 I^{-}

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

Q. What is an oxidizing agent in

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

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