For the reaction: $$\mathrm{I}^{-}+\mathrm{ClO}_{3}^{-}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{Cl}^{-}+\mathrm{HSO}_{4}^{-}+\mathrm{I}_{2}$$ The correct statement(s) in the balanced equation is/are:

(A) Stoichiometric coefficient of $\mathrm{HSO}_{4}{ }^{-}$ is 6.; (B) Iodide is oxidized.; (D) $\mathrm{H}_{2} \mathrm{O}$ is one of the products.

JEE Advanced · 2014 · 25 May 2014 · Paper 1 · Redox Reactions and Electrochemistry

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For the reaction:

I^{-} + ClO_{3}^{-} + H_{2} SO_{4} \to Cl^{-} + HSO_{4}^{-} + I_{2}

The correct statement(s) in the balanced equation is/are:

(A)Stoichiometric coefficient of $HSO_{4}^{-}$ is 6.✓ Correct
(B)Iodide is oxidized.✓ Correct
(C)Sulphur is reduced.
(D) $H_{2} O$ is one of the products.✓ Correct

Answer: (A), (B), (D)

Solution

Balanced equation:

6 I^{-} + Cl O_{3}^{-} + 6 H_{2} S O_{4} \to 3 I_{2} + C l^{-} + 6 HS O_{4}^{-} + 3 H_{2} O

(Cl:

+ 5 \to - 1

, gain 6 e⁻;

6 I^{-} \to 3 I_{2}

, lose 6 e⁻). So the coefficient of

HS O_{4}^{-}

is 6 (A true); iodide

(- 1 \to 0)

is oxidized (B true); sulphur stays

+ 6

throughout, not reduced (C false);

H_{2} O

is a product (D true).

JEE Advanced · 2014 · 25 May 2014 · Paper 1 · One or more correct options

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