Question

Identify correct statement for the reaction:
\( I_2 + KClO_3 \rightarrow ICl + KIO_3 \)

• A. \( I_2 \) is an oxidizing agent
• B. \( KClO_3 \) is a reducing agent
• C. Oxidation number of \( Cl \) decreases by 6
• D. Oxidation number of \( I \) increases by 2

Hint:

In redox reactions, oxidation involves an increase in oxidation state, and reduction involves a decrease in oxidation state.

Answer 1

The Correct Option is D

Step 1: Analyze the reaction.
The reaction involves the oxidation of \(I_2\) to \(ICl\) and reduction of \(KClO_3\) to \(KIO_3\). Here, iodine (I) is oxidized and chlorine (Cl) is reduced.

Step 2: Identify oxidation numbers.
- The oxidation number of iodine in \(I_2\) is 0, and in \(ICl\), it is +1. Therefore, iodine undergoes an increase in oxidation state by 1 (from 0 to +1).
- Chlorine in \(KClO_3\) has an oxidation state of +5, and in \(KIO_3\), it remains +5.

Step 3: Analyze the statements.
- Option \((1)\): \(I_2\) acts as an oxidizing agent because it is reduced to \(ICl\), so this statement is correct.
- Option \((2)\): \(KClO_3\) acts as an oxidizing agent, not as a reducing agent, so this is incorrect.
- Option \((3)\): Chlorine does not undergo a change in oxidation number, so this statement is incorrect.
- Option \((4)\): The oxidation number of iodine increases by 2, from 0 in \(I_2\) to +1 in \(ICl\).

Step 4: Final Answer.
Thus, the correct statement is \(I\) increases in oxidation state by 2, corresponding to option \((4)\).