Redox analysis of NH₄NO₃ decomposition

Steps:

• Balanced equation: NH₄NO₃ → N₂O + 2H₂O.
• Oxidation states of N: -3 in NH₄⁺, +5 in NO₃⁻; in N₂O, one N at +1 and one at -1.
• NH₄⁺ (N from -3 to -1/+1) loses electrons, acting as reducing agent.
• NO₃⁻ (N from +5 to -1/+1) gains electrons, acting as oxidizing agent.
• N in same compound changes from -3 and +5 to +1 and -1, confirming disproportionation.

Why B is correct:

• Statements 1 and 2 identify correct redox roles (reducing agent loses e⁻, oxidizing agent gains e⁻); 3 matches disproportionation definition where same element is both oxidized and reduced.

Why the others are wrong:

• A includes incorrect 4 (likely false, e.g., not thermal decomposition type or similar).
• C omits valid 1 and 2, includes wrong 4.
• D excludes valid 1 and 2.

Final answer: B