When `AgNO_(3)` is heated strongly, the products fomed are

Options

A. NO and `NO_(2)`
B. `NO_(2)` and `O_(2)`
C. `NO_(2)` and `N_(2)O`
D. `NO and O_(2)`

Answer

To determine the products formed when silver nitrate (AgNO₃) is heated strongly, we can follow these steps:

### Step 1: Write the decomposition reaction of silver nitrate.
When silver nitrate is heated, it decomposes into silver oxide (Ag₂O), nitrogen dioxide (NO₂), and oxygen (O₂).

**Reaction:**
\[ 2 \, \text{AgNO}_3 \, \text{(s)} \rightarrow \text{Ag}_2\text{O} \, \text{(s)} + 2 \, \text{NO}_2 \, \text{(g)} + \text{O}_2 \, \text{(g)} \]

### Step 2: Identify the instability of silver oxide.
The silver oxide (Ag₂O) formed is unstable at high temperatures and will further decompose into silver (Ag) and oxygen (O₂).

**Decomposition of silver oxide:**
\[ 2 \, \text{Ag}_2\text{O} \, \text{(s)} \rightarrow 4 \, \text{Ag} \, \text{(s)} + \text{O}_2 \, \text{(g)} \]

### Step 3: Combine the reactions to find the overall reaction.
Now, we can combine the two reactions to find the overall products of heating silver nitrate.

**Overall reaction:**
\[ 4 \, \text{AgNO}_3 \, \text{(s)} \rightarrow 4 \, \text{Ag} \, \text{(s)} + 2 \, \text{NO}_2 \, \text{(g)} + \text{O}_2 \, \text{(g)} \]

### Step 4: Balance the overall reaction.
To ensure the reaction is balanced, we can check the number of atoms of each element on both sides of the equation.

- **Silver (Ag):** 4 on both sides
- **Nitrogen (N):** 4 on both sides
- **Oxygen (O):** 12 on the left (from 4 AgNO₃) and 12 on the right (2 from NO₂ and 1 from O₂)

The overall balanced equation is:
\[ 4 \, \text{AgNO}_3 \, \text{(s)} \rightarrow 4 \, \text{Ag} \, \text{(s)} + 2 \, \text{NO}_2 \, \text{(g)} + \text{O}_2 \, \text{(g)} \]

### Conclusion:
The products formed when silver nitrate (AgNO₃) is heated strongly are silver (Ag), nitrogen dioxide (NO₂), and oxygen (O₂).

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