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The image provided depicts a chemical equilibrium problem involving the reaction:

\[
4 \text{NH}_3 (g) + 3 \text{O}_2 (g) \rightarrow 2 \text{N}_2 (g) + 6 \text{H}_2O (g)
\]

The problem involves analyzing the effects of perturbations (such as removal of \(\text{N}_2\) or addition of \(\text{O}_2\)) on the equilibrium of the reaction.

### First Perturbation: "Some \(\text{N}_2\) is removed"
- **Effect on the pressure of \(\text{NH}_3\)**: If \(\text{N}_2\) is removed, according to Le Chatelier’s principle, the system will try to oppose this change by shifting the equilibrium to the right, to produce more \(\text{N}_2\).
  - This means more reactants (\(\text{NH}_3\) and \(\text{O}_2\)) will be consumed, decreasing the pressure of \(\text{NH}_3\).

- **Effect on the pressure of \(\text{O}_2\)**: Since the reaction is shifting to the right, \(\text{O}_2\) will also be consumed, reducing its pressure.

- **Shift in equilibrium**: The equilibrium will shift **to the right**.

### Second Perturbation: "Some \(\text{O}_2\) is added"
- **Effect on the pressure of \(\text{NH}_3\)**: Adding more \(\text{O}_2\) will cause the system to try to counteract this by shifting the equilibrium to the right, consuming more \(\text{NH}_3\), and therefore decreasing its pressure.

- **Effect on the pressure of \(\text{N}_2\)**: As the equilibrium shifts to the right, more \(\text{N}_2\) will be produced, increasing its pressure.

- **Shift in equilibrium**: The equilibrium will shift **to the right**.

### Summary:
1. **When \(\text{N}_2\) is removed**:
   - Pressure of \(\text{NH}_3\) decreases.
   - Pressure of \(\text{O}_2\) decreases.
   - Equilibrium shifts to the right.
  
2. **When \(\text{O}_2\) is added**:
   - Pressure of \(\text{NH}_3\) decreases.
   - Pressure of \(\text{N}_2\) increases.
   - Equilibrium shifts to the right.

Would you like a detailed explanation of Le Chatelier's principle or how equilibrium shifts affect chemical systems?

### Follow-up Questions:
1. What happens if \(\text{NH}_3\) is added instead of \(\text{O}_2\)?
2. How would removing \(\text{O}_2\) affect the equilibrium?
3. What role does pressure play in equilibrium involving gases?
4. How does the removal of products affect endothermic and exothermic reactions?
5. How can temperature changes influence the equilibrium of this reaction?

### Tip:
When dealing with equilibrium, always remember that the system will adjust to counteract any imposed change, as per Le Chatelier's principle.

Ammonia and oxygen react to form nitrogen and water. What happens when nitrogen is removed or oxygen is added in an equilibrium system?

Analyze how removing nitrogen or adding oxygen affects the equilibrium of the reaction between ammonia and oxygen to form nitrogen and water. This problem involves Le Chatelier's principle and chemical equilibrium shifts. Suitable for high school chemistry students.

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