Question

Given below are two statements: Statement-I: In the decomposition of potassium chlorate, Cl is reduced. 
Statement-II: Reaction of Na with \( O_2 \) to form \( Na_2O \) is a redox reaction. 

• A. Both statements-I and II are correct
• B. Both statements-I and II are not correct
• C. Statement-I is correct but statement-II is not correct
• D. Statement-I is not correct but statement-II is correct

Hint:

- In redox reactions, oxidation involves an increase in oxidation state, and reduction involves a decrease.
- Decomposition reactions like \( KClO_3 \rightarrow KCl + O_2 \) involve oxidation-reduction changes.
- When metals react with oxygen, they generally form ionic oxides, leading to redox processes.

Answer 1

The Correct Option is A

Statement-I: In the decomposition of potassium chlorate, Cl is reduced.

This statement is correct. In the decomposition of potassium chlorate (KClO₃), potassium chloride (KCl) and oxygen gas (O₂) are formed. In this reaction, chlorine undergoes reduction as it goes from +5 oxidation state in KClO₃ to -1 oxidation state in KCl.

Statement-II: The reaction of Na with O₂ to form Na₂O is a redox reaction.

This statement is also correct. In the reaction between sodium (Na) and oxygen (O₂) to form sodium oxide (Na₂O), sodium is oxidized from 0 to +1 oxidation state, and oxygen is reduced from 0 to -2 oxidation state. This is indeed a redox reaction.

Since both statements are correct, the correct answer is:

Both statement-I and statement-II are correct.