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Understanding Reversible Reactions and Dynamic Equilibrium in Chemistry

In this lesson, we explore the fundamental concepts of reversible reactions and dynamic equilibrium in chemical processes. We will discuss how certain chemical reactions can proceed in both directions, resulting in a mixture where the forward and backward reactions occur simultaneously at the same rate. Key examples include the hydration and dehydration of copper sulfate and the formation of ammonia via the Haber process. Students will learn to identify signs of chemical reactions, such as color change and gas production, and engage in activities like creating informative posters about the Haber process.

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Understanding Reversible Reactions and Dynamic Equilibrium in Chemistry

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Presentation Transcript

  1. Today’s lesson • Discuss the idea of a simple reversible reaction • Explain the concept of dynamic equilibrium

  2. Chemical reactions – What to look for This is from year 7!

  3. Chemical reactions – What to look for • There may be a change ofcolour

  4. Chemical reactions – What to look for • There may be a gas given off (bubbles)

  5. Chemical reactions – What to look for • There may be an energy change (gets hotter or colder)

  6. Chemical reactions – What to look for • New substances are formed, and the change is usually difficult to reverse

  7. Word equations Zinc + sulphur reactants

  8. Word equations Zinc + sulphur zinc sulphide reactants product(s)

  9. Chemical reactions – What to look for • New substances are formed, and the change is usually difficult to reverse

  10. Reversible reactions

  11. Reversible reactions • A reversible reaction is a chemical reaction that can go both ways. Hydrated copper sulphate Anhydrous copper sulphate + water

  12. Reversible reactions • A reversible reaction is a chemical reaction that can go both ways. Ammonium chloride Ammonia + hydrogen chloride NH4Cl(s) NH3(g) + HCl (g)

  13. Reversible reactions It often results in an dynamic equilibrium mixture in which the forward and backward reactions occur at the same rate. CH3COOH (aq) H+(aq) + CH3COO-(aq)

  14. le Chatelier's principle The position of equilibrium shifts to try to cancel out any changes you make

  15. Haber Process Do you like my glasses?

  16. Objectives • State that ammonia is an important chemical • Describe how ammonia can be made • State how waste of raw materials can be minimised in making ammonia

  17. Today’s Task • Using your book and the internet to create a poster explaining the Haber process. • You should include: • What does the Haber process do? • Why is ammonia important? What do we use it for? • Where do we get the materials to make the ammonia? • Give the balanced equation for the Haber process • What temperature and pressure do we use? What is the catalyst used? • Why do we use this temperature and pressure? • Include a flow diagram of the process

  18. Quick game • Hunt down the questions round the room take them back to your team and give me an answer. • If you get it right you can go find question 2 and so on!

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