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:

Assign oxidation numbers to Cl and I on both sides of the reaction and see how they change.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept
Compare oxidation numbers: \(\text{I}_2+\text{KClO}_3\rightarrow\text{ICl}+\text{KIO}_3\).

Step 2: Chlorine
In \(\text{KClO}_3\), Cl is +5. In ICl, Cl is -1.
The oxidation number of Cl decreases by 6, so \(\text{KClO}_3\) is the oxidising agent.

Step 3: Iodine
In \(\text{I}_2\) it is 0. It becomes +1 in ICl and +5 in \(\text{KIO}_3\).
So \(\text{I}_2\) is the reducing agent, and its oxidation number increases by 1 or 5, not 2.

Step 4: Compare the options
Only the statement that the oxidation number of Cl decreases by 6 is correct, the third option.

Final Answer:
The oxidation number of chlorine decreases by 6. \[ \boxed{\text{(C) }\text{Oxidation number of Cl decreases by 6}} \]