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The problem you're dealing with involves a chemical equilibrium for the exothermic reaction between sulfur dioxide (SO₂) and oxygen (O₂) to form sulfur trioxide (SO₃):

\[ 2 \text{SO}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2 \text{SO}_3 (g) \]

Le Châtelier's principle tells us how the system at equilibrium will respond to changes in temperature and pressure.

### 1. Lowering the Temperature:
- Since the reaction is exothermic, heat can be considered a "product." Lowering the temperature favors the exothermic direction, shifting the equilibrium **to the right** (towards more SO₃).
- As a result, the **pressure of SO₃** will **increase**.

### 2. Raising the Temperature:
- Raising the temperature will favor the endothermic direction, shifting the equilibrium **to the left** (towards more SO₂ and O₂).
- As a result, the **pressure of SO₂** will **increase**.

### Final Answers for the Table:
1. **Lowering the Temperature:**
   - The pressure of SO₃ will **increase**.
   - The equilibrium shifts **to the right**.

2. **Raising the Temperature:**
   - The pressure of SO₂ will **increase**.
   - The equilibrium shifts **to the left**.

Would you like further explanation on any part of this?

### Here are five related questions you might consider:
1. How does increasing the concentration of SO₂ affect the equilibrium position?
2. What would happen if the volume of the reaction vessel is increased?
3. How does a catalyst affect the equilibrium position of this reaction?
4. How would the system respond if additional O₂ is introduced?
5. What are the real-life implications of controlling temperature in the production of SO₃?

### Tip: 
Le Châtelier's principle is a great tool to predict the direction of equilibrium shifts, but it does not give information about the rate at which equilibrium is re-established.

Predict the changes in composition and the equilibrium shift for the exothermic reaction: 2SO₂(g) + O₂(g) → 2SO₃(g), when temperature is raised or lowered.

Learn how changes in temperature affect the equilibrium and pressure of products in the exothermic reaction between sulfur dioxide (SO₂) and oxygen (O₂) to form sulfur trioxide (SO₃). Based on Le Châtelier’s principle, lowering the temperature favors SO₃ formation, while raising the temperature shifts equilibrium to favor SO₂ and O₂. Suitable for advanced high school chemistry students.

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