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  • Which of the following statement(s) is incorrect for a given chemical reaction? <img alt="\[{{I}^{-}}+ClO_{3}^{-}+{{H}_{2}}SO_{4}^{-}\to C{{l}^{-}}+HSO_{4}^{-}+{{

Which of the following statement(s) is incorrect for a given chemical reaction?

\[{{I}^{-}}+ClO_{3}^{-}+{{H}_{2}}SO_{4}^{-}\to C{{l}^{-}}+HSO_{4}^{-}+{{I}_{2}}\]

Option: 1

 stoichiometric coefficient of HSO_{4}^{-\: \: }is\: \: \,6


Option: 2

Sulphur is reduced.


Option: 3

Iodide is oxidised.


Option: 4

{{H}_{2}}O is one of the products.

 


Answers (1)

best_answer

This reaction is an example of a redox reaction, where one reactant is reduced and the other is oxidised. Thus, it has one oxidation half-cell reaction and another reduction half-cell reaction.

At oxidation half cell: 6{{I}^{-}}\to 3{{I}_{2}}+6{{e}^{-}}

Therefore, iodide is oxidised by losing electrons.

At reduction half cell: 6{{H}^{+}}+ClO_{3}^{-}+6{{e}^{-}}\to C{{l}^{-}}+3{{H}_{2}}O

As per the reduction half-cell reaction, {{H}^{+}} is reduced by gaining electrons and {{H}_{2}}O is formed as a product.

On balancing the given equation, we obtain:  

6{{I}^{-}}+ClO_{3}^{-}+6{{H}_{2}}S{{O}_{4}}\to C{{l}^{-}}+3{{I}_{2}}+3{{H}_{2}}O+6HSO_{4}^{-}

Sulphur is not reduced in this redox reaction.

Therefore options (1), (3), and (4) are correct but (2) is incorrect.

Posted by

Kuldeep Maurya

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