Lesson Plan

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Lesson Plan
Grade: Date: 25/02/2026
Subject: Chemistry
Lesson Topic: Describe how changing the conditions can change the direction of a reversible reaction for: (a) the effect of heat on hydrated compounds (b) the addition of water to anhydrous compounds limited to copper(II) sulfate and cobalt(II) chloride
Learning Objective/s:
  • Describe how heat affects the direction of reversible reactions involving hydrated salts.
  • Explain how adding or removing water shifts the equilibrium of copper(II) sulfate and cobalt(II) chloride.
  • Predict colour changes associated with dehydration and rehydration of these salts.
  • Apply Le Chatelier’s principle to determine the effect of temperature and water concentration on reaction direction.
  • Solve typical exam‑style questions on reversible hydrate reactions.
Materials Needed:
  • Copper(II) sulfate pentahydrate and anhydrous copper(II) sulfate.
  • Cobalt(II) chloride anhydrous and hexahydrate.
  • Bunsen burners or hot plates.
  • Test tubes, stands, and tongs.
  • Distilled water dropper.
  • Whiteboard/projector for diagrams.
  • Worksheet with practice questions.
 Introduction:
Begin with a quick demonstration of a blue CuSO₄·5H₂O sample turning white on heating to capture interest. Review prior learning of equilibrium and Le Chatelier’s principle. State that today students will predict colour changes when temperature or water is altered.
Lesson Structure:
  1. Do‑now (5’) – Students answer a recall question on equilibrium.
  2. Mini‑lecture (10’) – Explain Le Chatelier’s principle and hydrate equilibria with diagrams.
  3. Demonstration 1 (8’) – Heat CuSO₄·5H₂O, observe colour change, discuss shift.
  4. Demonstration 2 (8’) – Add water to anhydrous CuSO₄ and CoCl₂, observe colour changes, link to equilibrium.
  5. Guided practice (12’) – Worksheet questions in pairs, teacher circulates.
  6. Quick check (5’) – Exit ticket: write the predicted direction of shift for a given condition.
  7. Summary discussion (5’) – Recap key concepts.
Conclusion:
Summarise that heat drives dehydration (right shift) while cooling promotes rehydration, and that water addition pushes the equilibrium toward the hydrated form. Collect exit tickets as a retrieval check and assign a short homework to write balanced equations for a new hydrate.