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

Short answer

Options (c) 1,4 and (d) 2,4 are correct.

Step-by-step solution

Understanding Nitrogen (I) Oxide

Nitrogen (I) oxide is also known as nitrous oxide with the formula \(\text{N}_2\text{O}\). Let's explore which reactions produce \(\text{N}_2\text{O}\).

Analyzing Thermal Decomposition of Ammonium Nitrate

The thermal decomposition of ammonium nitrate (\(\text{NH}_4\text{NO}_3\)) produces gases including \(\text{N}_2\text{O}\). The reaction is: \[\text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O}\] Thus, this option indicates production.

Analyzing Disproportionation of \(\mathrm{N}_{2} \mathrm{O}_{4}\)

Disproportionation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) involves changes between different nitrogen oxidation states. Typically, \(\mathrm{N}_{2} \mathrm{O}_{4}\) does not produce \(\mathrm{N}_2\mathrm{O}\) through disproportionation but rather \(\mathrm{NO}_2\) and \(\mathrm{NO}\). Thus, it doesn't contribute to \(\text{N}_2\text{O}\) formation in this case.

Analyzing Thermal Decomposition of Ammonium Nitrite

Ammonium nitrite (\(\text{NH}_4\text{NO}_2\)) decomposes thermally to form \(\text{N}_2\text{O}\) and water:\[\text{NH}_4\text{NO}_2 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O}\] So this reaction produces \(\text{N}_2\text{O}\).

Analyzing Interaction of Hydroxylamine and Nitrous Acid

The reaction of hydroxylamine \((\text{NH}_2\text{OH})\) and nitrous acid \((\text{HNO}_2)\) can produce \(\text{N}_2\text{O}\) as follows:\[\text{NH}_2\text{OH} + \text{HNO}_2 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O}\] This reaction indeed produces \(\text{N}_2\text{O}\).

Identifying Correct Options

From the analysis, reactions 1 (thermal decomposition of ammonium nitrate), 3 (thermal decomposition of ammonium nitrite), and 4 (interaction of hydroxylamine and nitrous acid) produce \(\text{N}_2\text{O}\). Hence, options (c) and (d) are correct.

Key concepts

Thermal Decomposition

Thermal decomposition is a chemical reaction where a single compound breaks down when heated, forming two or more simpler substances. This process is central in understanding how some gases, like nitrous oxide (_2O), are formed from various chemicals.
For example, when ammonium nitrate (H_4NO_3) is heated, it decomposes into nitrous oxide and water: \[ \text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]

• This reaction is a classic example of thermal decomposition because the application of heat causes a chemical split.
• Similarly, ammonium nitrite (H_4NO_2) also undergoes thermal decomposition, producing the same gas _2O along with water:
\[ \text{NH}_4\text{NO}_2 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]

Understanding thermal decomposition helps us predict how certain chemicals will behave under heat and the products they will yield.

Disproportionation

Disproportionation is a specific type of redox reaction where a single element undergoes oxidation and reduction simultaneously, producing two different compounds. This reaction involves changes in oxidation states of elements. However, when it comes to nitrogen oxides, disproportionation has unique characteristics:

• For instance, dinitrogen tetroxide ( _2O_4) typically disproportionates into nitrogen dioxide ( O_2) and nitric oxide ( O), not nitrous oxide ( _2O).
• This misalignment with nitrous oxide production means that _2O_4's disproportionation isn't directly responsible for _2O formation, though it's relevant in other contexts.

Understanding disproportionation can illuminate the complexity of chemical reactions where multiple compounds are generated from a single reagent. It underscores the intricacies found in redox chemistry.

Chemical Reactions Analysis

Chemical reactions analysis is the process of observing and interpreting chemical reactions to understand the underlying principles and product formation. Such analysis is key in assessing how _2O can be produced through different methods.

• By examining reactions like the interaction of hydroxylamine (H_2OH) and nitrous acid (HO_2), we identify nitrous oxide as a product alongside water:
\[ \text{NH}_2\text{OH} + \text{HNO}_2 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]
• This emphasizes the importance of correctly balancing equations to predict actual products.
• Through analysis, we determine which reactions are viable paths to produce certain compounds, as seen with the thermal decompositions of ammonium nitrate and ammonium nitrite.

This approach guides chemists on how different reactions can be utilized or adjusted to obtain desired substances, illustrating a fundamental aspect of chemical synthesis and production.