`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 solve the problem of the thermal decomposition of ammonium nitrate (NH₄NO₃) into nitrous oxide (N₂O) and water (H₂O), we will follow these steps:

### Step 1: Write the balanced equation
The reaction is given as:
\[ \text{NH}_4\text{NO}_3 \xrightarrow{\Delta} \text{N}_2\text{O} + \text{H}_2\text{O} \]

### Step 2: Determine the oxidation states of nitrogen in the reactants
1. **For NH₄⁺ (ammonium ion)**:
- Let the oxidation state of nitrogen be \( x \).
- The equation is:
\[ x + 4(-1) = +1 \]
- Solving gives:
\[ x - 4 = 1 \]
\[ x = +3 \]
- Thus, the oxidation state of nitrogen in NH₄⁺ is **-3**.

2. **For NO₃⁻ (nitrate ion)**:
- Let the oxidation state of nitrogen be \( y \).
- The equation is:
\[ y + 3(-2) = -1 \]
- Solving gives:
\[ y - 6 = -1 \]
\[ y = +5 \]
- Thus, the oxidation state of nitrogen in NO₃⁻ is **+5**.

### Step 3: Determine the oxidation state of nitrogen in the products
1. **For N₂O**:
- Let the oxidation state of nitrogen be \( z \).
- The equation is:
\[ 2z + (-2) = 0 \]
- Solving gives:
\[ 2z - 2 = 0 \]
\[ 2z = 2 \]
\[ z = +1 \]
- Thus, the oxidation state of nitrogen in N₂O is **+1**.

### Step 4: Analyze the changes in oxidation states
- In the reaction:
- Nitrogen in NH₄⁺ changes from **-3** to **+1** (oxidation).
- Nitrogen in NO₃⁻ changes from **+5** to **+1** (reduction).

### Step 5: Classify the type of reaction
- Since a single element (nitrogen) is present in different oxidation states in the reactants, this reaction is classified as a **comproportionation reaction**.
- Additionally, since NH₄NO₃ decomposes into two products, it is also a **thermal decomposition reaction**.

### Conclusion
The reaction of NH₄NO₃ when heated leads to the formation of N₂O and H₂O, and it can be classified as both a **comproportionation reaction** and a **thermal decomposition reaction**.

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