### Ionic Equation for the Oxidation of Ammonium Ions

To write the ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions, we follow these steps:

1. **Identify Reactants and Products**
The reactant is the ammonium ion (NH₄⁺) and the product is nitrogen gas (N₂). In acidic conditions, hydrogen ions (H⁺) and water (H₂O) may also be involved in the oxidation process.

2. **Balanced Half-Reaction**
The oxidation of ammonium ions can be represented as a half-reaction. The oxidation of NH₄⁺ to N₂ involves the loss of electrons.

3. **Write the Ionic Equation**
The balanced half-reaction can be expressed as:
$$
2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
$$

This equation indicates that two ammonium ions oxidize to form one molecule of nitrogen gas, releasing protons (H⁺) and electrons in the process.

### Final Answer
The ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions is:
$$
2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
$$

Question

### Ionic Equation for the Oxidation of Ammonium Ions

To write the ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions, we follow these steps:

1. **Identify Reactants and Products**  
   The reactant is the ammonium ion (NH₄⁺) and the product is nitrogen gas (N₂). In acidic conditions, hydrogen ions (H⁺) and water (H₂O) may also be involved in the oxidation process.

2. **Balanced Half-Reaction**  
   The oxidation of ammonium ions can be represented as a half-reaction. The oxidation of NH₄⁺ to N₂ involves the loss of electrons.

3. **Write the Ionic Equation**
   The balanced half-reaction can be expressed as:
   $$
   2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
   $$

This equation indicates that two ammonium ions oxidize to form one molecule of nitrogen gas, releasing protons (H⁺) and electrons in the process.

### Final Answer
The ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions is:
$$
2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
$$

Knowee AI · Accepted Answer

### Ionic Equation for the Oxidation of Ammonium Ions

To write the ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions, we follow these steps:

1. **Identify Reactants and Products**  
   The reactant is the ammonium ion (NH₄⁺) and the product is nitrogen gas (N₂). In acidic conditions, hydrogen ions (H⁺) and water (H₂O) may also be involved in the oxidation process.

2. **Balanced Half-Reaction**  
   The oxidation of ammonium ions can be represented as a half-reaction. The oxidation of NH₄⁺ to N₂ involves the loss of electrons.

3. **Write the Ionic Equation**
   The balanced half-reaction can be expressed as:
   $$
   2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
   $$

This equation indicates that two ammonium ions oxidize to form one molecule of nitrogen gas, releasing protons (H⁺) and electrons in the process.

### Final Answer
The ionic equation for the oxidation of ammonium ions (NH₄⁺) to nitrogen gas (N₂) under acidic conditions is:
$$
2 \, \text{NH}_4^+ \rightarrow \text{N}_2 + 8 \, \text{H}^+ + 6 \, e^-
$$

ammonium ions NH4+,are oxidised to nitrogen under acidic conditions.write an ionic equation

Question

Ammonium ions $NH_4^+$ are oxidised to nitrogen under acidic conditions. Write an ionic equation.

Solution