Problem 109 - A Complete Resource Book in Chemistry for JEE Main

Question

Nitrogen (I) oxide is produced by 1\. thermal decomposition of ammonium nitrate 2\. disproportionation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) 3\. thermal decomposition of ammonium nitrite 4\. interaction of hydroxyl amine and nitrous acid (a) 1,2 (b) 2,3 (c) 1,4 (d) 2,4

Step-by-Step Solution

Answer

The correct options are (a) 1,2 and (c) 1,4. Option (c) includes both scenarios.

Step 1: Identify the Reaction Types

Review the potential reactions provided in the options and identify their types: thermal decomposition, disproportionation, and interaction.

Step 2: Analyze Thermal Decomposition of Ammonium Nitrate

Consider the reaction: Ammonium nitrate decomposes upon heating to form nitrogen (I) oxide and water. The equation is: \[ ext{NH}_4 ext{NO}_3 ightarrow ext{N}_2 ext{O} + 2 ext{H}_2 ext{O} \]This option produces nitrogen (I) oxide.

Step 3: Examine Disproportionation of \\(\mathrm{N}_{2} \mathrm{O}_{4}\)

Review the reaction: Disproportionation involves a compound being simultaneously oxidized and reduced. The reaction for \(\mathrm{N}_{2} \mathrm{O}_{4}\) produces nitrogen (IV) oxide and nitrogen (I) oxide:\[ \mathrm{N}_{2} \mathrm{O}_{4} \rightarrow \mathrm{NO}_2 + \mathrm{N}_2\mathrm{O} \]This process also creates nitrogen (I) oxide.

Step 4: Evaluate Thermal Decomposition of Ammonium Nitrite

Consider whether ammonium nitrite decomposes to form nitrogen (I) oxide. It actually decomposes to nitrogen gas and water:\[ \mathrm{NH}_4\mathrm{NO}_2 \rightarrow \mathrm{N}_2 + 2\mathrm{H}_2\mathrm{O} \]Therefore, this reaction does not produce nitrogen (I) oxide.

Step 5: Analyze Interaction of Hydroxylamine and Nitrous Acid

Review the interaction: Hydroxylamine reacts with nitrous acid, forming nitrogen (I) oxide and water, characterized by this reaction:\[ \mathrm{NH}_2\mathrm{OH} + \mathrm{HNO}_2 \rightarrow \mathrm{N}_2\mathrm{O} + 2\mathrm{H}_2\mathrm{O} \]This reaction produces nitrogen (I) oxide.

Step 6: Identify Correct Options

From the analysis, reactions 1 and 2 both produce nitrogen (I) oxide, as do reactions 1 and 4. Match the correct options: - (a) 1,2 - (c) 1,4 Thus, both options (a) and (c) are correct, but (c) is the best choice since it includes option 1's result too.

Key Concepts

Thermal Decomposition

Thermal decomposition is a chemical reaction where a compound breaks down into two or more products when heated. It often requires energy input to overcome the limitations that hold different elements or compounds together within a molecule. This type of reaction is pivotal in many chemical processes.

In the case of ammonium nitrate (\( ext{NH}_4 ext{NO}_3\)), when heat is applied, it decomposes by losing water and breaking down into nitrogen (I) oxide (\( ext{N}_2 ext{O}\)) and water. The balanced chemical equation is
\[\text{NH}_4 ext{NO}_3 \rightarrow ext{N}_2 ext{O} + 2 ext{H}_2 ext{O} \]

This demonstrates a practical application of thermal decomposition in producing useful gases.

Ammonium Nitrate

Ammonium nitrate, a chemical compound with the formula \( ext{NH}_4 ext{NO}_3\), is used widely in agriculture as a high-nitrogen fertilizer. Apart from its abundant use in fertilizers, it has applications in explosives and as a key ingredient in some chemical reactions.

The thermal instability of ammonium nitrate makes it an important topic in chemistry classes. Its decomposition helps in producing nitrogen (I) oxide.

• Ammonium nitrate breaks down when heated.
• Produces nitrogen (I) oxide and water.
• Safety concerns limit its storage and handling because it can explosively decompose under certain conditions.

Understanding the decomposition is essential in ensuring safety and exploring its chemical properties.

Disproportionation Reaction

A disproportionation reaction occurs when a single reactant is both oxidized and reduced, forming two separate products. This unique reaction type involves the same element appearing in varying oxidation states.

In the context of \( ext{N}_2 ext{O}_4\), disproportionation breaks it into nitrogen (IV) oxide (\( ext{NO}_2\)) and nitrogen (I) oxide (\( ext{N}_2 ext{O}\)), showcasing how the compound can split under certain conditions:
\[\text{N}_2 ext{O}_4 \rightarrow ext{NO}_2 + ext{N}_2 ext{O}\]

This process is a crucial example of how chemical species can reorganize and change oxidation states in reactions, which is important for understanding complex chemistry concepts.

Hydroxylamine Reaction

Hydroxylamine is a reactive compound often utilized in the production of numerous nitrogen compounds. When it reacts with nitrous acid (\( ext{HNO}_2\)), the reaction produces nitrogen (I) oxide and water.

This reaction plays a role in synthetic and analytical chemistry and is represented by the equation:
\[\text{NH}_2 ext{OH} + ext{HNO}_2 \rightarrow ext{N}_2 ext{O} + 2 ext{H}_2 ext{O}\]

Understanding this reaction helps in grasping how reactive hydroxylamine can be used to produce useful gaseous compounds. The production of nitrogen (I) oxide showcases the versatility and importance of hydroxylamine in chemical processes.