| Lesson Plan |
| Grade: |
Date: 25/02/2026 |
| Subject: Chemistry |
| Lesson Topic: State the typical conditions for the conversion of sulfur dioxide to sulfur trioxide in the Contact process as $450^{\circ}\mathrm{C}, 200\mathrm{kPa} / 2\mathrm{~atm}$ and a vanadium(V) oxide catalyst |
Learning Objective/s:
- Describe the reversible oxidation of SO₂ to SO₃ and write the balanced chemical equation.
- Explain how temperature, pressure, and a V₂O₅ catalyst influence the equilibrium position using Le Chatelier’s principle.
- Predict the effect of increasing temperature, decreasing pressure, or removing SO₃ on the yield of SO₃.
- Apply the typical industrial conditions (450 °C, 200 kPa, V₂O₅) to justify why they are chosen for maximum yield.
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Materials Needed:
- Projector or interactive whiteboard
- Printed worksheet with equilibrium tables and Le Chatelier scenarios
- Calculator for quick quantitative checks
- Energy‑profile diagram of the SO₂ → SO₃ reaction (handout or slide)
- Small group cards with “what‑if” condition changes
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Introduction:
Begin with a short video clip of an industrial sulfuric‑acid plant to capture interest. Ask students what they already know about reversible reactions and Le Chatelier’s principle. State that by the end of the lesson they will be able to list the exact temperature, pressure, and catalyst used in the Contact process and explain why each is optimal.
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Lesson Structure:
- Do‑Now (5 minutes): Quick quiz on dynamic equilibrium and Le Chatelier’s principle.
- Mini‑lecture (10 minutes): Introduce the Contact process, show the balanced equation and the typical operating conditions.
- Guided analysis (10 minutes): Using the provided table, discuss why 450 °C balances rate and equilibrium, why 200 kPa favours product formation, and how V₂O₅ acts as a catalyst.
- Group activity (15 minutes): Each group receives a “what‑if” scenario (e.g., raise temperature to 600 °C) and predicts the shift in equilibrium, then shares conclusions.
- Check for understanding (5 minutes): Exit‑ticket where students write one condition and its effect on SO₃ yield.
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Conclusion:
Summarise the key reasons for the chosen temperature, pressure, and catalyst, linking each back to Le Chatelier’s principle. Collect the exit tickets to gauge understanding and assign a worksheet for homework that asks students to apply the same reasoning to another industrial equilibrium.
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