Step 1: Understanding the Question:
We need to calculate oxidation states to determine which statement correctly describes the redox changes.
Step 2: Detailed Explanation:
In \( \text{I}_2 \), O.N. of \( \text{I} = 0 \).
In \( \text{KClO}_3 \), O.N. of \( \text{Cl} = +5 \).
In \( \text{ICl} \), \( \text{Cl} \) is more electronegative, so O.N. of \( \text{Cl} = -1 \), O.N. of \( \text{I} = +1 \).
In \( \text{KIO}_3 \), O.N. of \( \text{I} = +5 \).
Change in O.N. of \( \text{Cl} \): From \( +5 \) to \( -1 \), it decreases by 6.
Change in O.N. of \( \text{I} \): From \( 0 \) to \( +1 \) and \( +5 \), it increases.
Since \( \text{Cl} \) is reduced, \( \text{KClO}_3 \) is the oxidizing agent. Since \( \text{I} \) is oxidized, \( \text{I}_2 \) is the reducing agent.
Step 3: Final Answer:
Statement (C) is correct as the oxidation number of Cl decreases by 6.