Problem 61
Question
Nitrogen(I) oxide is produced by:(a) thermal decomposition of ammonium nitrate (b) disproportionation of \(\mathrm{N}_{2} \mathrm{O}_{4}\) (c) thermal decomposition of ammonium nitrite (d) interaction of hydroxylamine and nitrous acid.
Step-by-Step Solution
Verified Answer
Option (b) - disproportionation of \( N_2O_4 \) produces Nitrogen(I) oxide.
1Step 1: Identify the chemical reaction for option (a)
The thermal decomposition of ammonium nitrate (NH_4NO_3) primarily produces dinitrogen monoxide (N_2O) and water (H_2O):\[\text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O}\]This does not produce Nitrogen(I) oxide (NO).
2Step 2: Identify the chemical reaction for option (b)
The disproportionation of N_2O_4 results in the formation of nitrogen dioxide (NO_2) and nitric oxide (NO):\[\text{N}_2\text{O}_4 \rightarrow \text{NO}_2 + \text{NO}\]This produces Nitrogen(I) oxide, which is NO.
3Step 3: Identify the chemical reaction for option (c)
The thermal decomposition of ammonium nitrite (NH_4NO_2) leads to the production of nitrogen gas (N_2) and water (H_2O):\[\text{NH}_4\text{NO}_2 \rightarrow \text{N}_2 + 2\text{H}_2\text{O}\]Nitrogen(I) oxide (NO) is not produced in this reaction.
4Step 4: Identify the chemical reaction for option (d)
The interaction of hydroxylamine (
NH_2OH
) with nitrous acid (
HNO_2
) does not efficiently produce nitrogen oxides as the result is typically complex. However, for the context of this problem, it isn't a specified reaction for forming Nitrogen(I) oxide (
NO
).
5Step 5: Conclusion: Determine which option produces Nitrogen(I) oxide
After analyzing all the options, option (b) - disproportionation of
N_2O_4,
explicitly produces Nitrogen(I) oxide (NO).
Key Concepts
Thermal DecompositionDisproportionationChemical ReactionsAmmonium NitrateAmmonium Nitrite
Thermal Decomposition
Thermal decomposition is a process where a chemical compound is broken down into simpler substances when heated. It is an endothermic reaction, meaning it requires an input of energy. Some common products of thermal decomposition include gases, liquids, or solids. In the context of ammonium nitrate (\(\text{NH}_4\text{NO}_3\)), thermal decomposition primarily yields dinitrogen monoxide (\(\text{N}_2\text{O}\)) and water (\(\text{H}_2\text{O}\)).
Understanding the breakdown of compounds through thermal decomposition is essential as it helps in the study of stability, energy requirements, and reactivity of materials. Not every compound will yield the desired product, as seen in the exercise where ammonium nitrate's decomposition does not produce Nitrogen(I) oxide.
Understanding the breakdown of compounds through thermal decomposition is essential as it helps in the study of stability, energy requirements, and reactivity of materials. Not every compound will yield the desired product, as seen in the exercise where ammonium nitrate's decomposition does not produce Nitrogen(I) oxide.
Disproportionation
Disproportionation is a unique type of chemical reaction where a single substance undergoes both oxidation and reduction, transforming into two or more different substances. This concept is pivotal in redox chemistry.
With the compound \(\text{N}_2\text{O}_4\), disproportionation leads to the formation of nitrogen dioxide (\(\text{NO}_2\)) and nitric oxide (\(\text{NO}\)), the latter being Nitrogen(I) oxide. This type of reaction is interesting because it involves a single molecular species acting in dual roles through electron transfer, thereby resulting in two distinct products.
With the compound \(\text{N}_2\text{O}_4\), disproportionation leads to the formation of nitrogen dioxide (\(\text{NO}_2\)) and nitric oxide (\(\text{NO}\)), the latter being Nitrogen(I) oxide. This type of reaction is interesting because it involves a single molecular species acting in dual roles through electron transfer, thereby resulting in two distinct products.
Chemical Reactions
Chemical reactions involve the transformation of substances through the breaking and forming of chemical bonds. They are categorized based on various criteria, including the type of reactants and products involved.
Chemical reactions are fundamentally the building blocks for creating and understanding new compounds. They allow substances to change states, release or absorb energy, and even change colors or produce new smells.
Chemical reactions are fundamentally the building blocks for creating and understanding new compounds. They allow substances to change states, release or absorb energy, and even change colors or produce new smells.
- Combination reactions where two or more substances combine to form a single product.
- Decomposition reactions, where a compound breaks down into simpler products.
- Disproportionation reactions, a subtype of redox reactions.
Ammonium Nitrate
Ammonium nitrate (\(\text{NH}_4\text{NO}_3\)) is a compound used commonly as a fertilizer in agriculture due to its high nitrogen content. Its decomposition is an important reaction, primarily because it is exothermic and can sometimes be explosive given the right conditions, as with changes in temperature or pressure.
The decomposition of ammonium nitrate is significant in fields other than chemistry, such as safety engineering and agriculture. The primary decomposition reaction produces dinitrogen monoxide (also known as laughing gas) and water. This underscores the importance of understanding decomposition reactions to manage and mitigate risks associated with handling reactive materials.
The decomposition of ammonium nitrate is significant in fields other than chemistry, such as safety engineering and agriculture. The primary decomposition reaction produces dinitrogen monoxide (also known as laughing gas) and water. This underscores the importance of understanding decomposition reactions to manage and mitigate risks associated with handling reactive materials.
Ammonium Nitrite
Ammonium nitrite (\(\text{NH}_4\text{NO}_2\)) is an inorganic compound employed in various chemical processes. Its decomposition is notably distinctive as it leads to the formation of nitrogen gas (\(\text{N}_2\)) and water (\(\text{H}_2\text{O}\)).
Understanding the decomposition of ammonium nitrite highlights the importance of reaction stoichiometry and gas production in chemical reactions. It serves as a simple example of how reactions can yield different, often non-hazardous, products compared to those which might be dangerous. This knowledge is crucial for scientists and engineers to develop safer and more efficient chemical processes.
Understanding the decomposition of ammonium nitrite highlights the importance of reaction stoichiometry and gas production in chemical reactions. It serves as a simple example of how reactions can yield different, often non-hazardous, products compared to those which might be dangerous. This knowledge is crucial for scientists and engineers to develop safer and more efficient chemical processes.
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