`NH_(4)NO_(3) overset(Delta) to N_(2)O+H_(2)O`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To determine the type of reaction represented by the equation \( NH_4NO_3 \overset{\Delta}{\rightarrow} N_2O + H_2O \), we can follow these steps:

### Step 1: Identify the Reactants and Products
The reactant is ammonium nitrate, \( NH_4NO_3 \), and the products are nitrous oxide, \( N_2O \), and water, \( H_2O \).

### Step 2: Analyze the Oxidation States of Nitrogen
1. **In \( NH_4NO_3 \)**:
- The ammonium ion \( NH_4^+ \) has nitrogen in the oxidation state of \(-3\).
- The nitrate ion \( NO_3^- \) has nitrogen in the oxidation state of \(+5\).

2. **In the products**:
- In \( N_2O \), the oxidation state of nitrogen can be calculated as follows:
\[ 2x - 2 = 0 \implies x = +1 \]
- Therefore, nitrogen in \( N_2O \) is in the oxidation state of \(+1\).

### Step 3: Determine the Change in Oxidation States
- In the reaction, nitrogen changes from \(-3\) in \( NH_4^+ \) to \(+1\) in \( N_2O\) and from \(+5\) in \( NO_3^-\) to \(+1\) in \( N_2O\).

### Step 4: Classify the Reaction
Since the same element (nitrogen) is present in different oxidation states in the reactants and products, this reaction can be classified as a **comproportionation reaction**.

### Step 5: Confirm the Reaction Type
Additionally, since the reaction involves the decomposition of a single compound \( NH_4NO_3 \) into two products \( N_2O \) and \( H_2O \) upon heating, it is also a **thermal decomposition reaction**.

### Conclusion
Thus, the reaction \( NH_4NO_3 \overset{\Delta}{\rightarrow} N_2O + H_2O \) is classified as both a **comproportionation reaction** and a **thermal decomposition reaction**.

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