Sketch and label an energy level diagram that includes a catalyst. 9. ... Distinguish between homogeneous and heterogeneous reactions, and explain why...
Classwork – Reaction Rates and Equilibrium 1. Describe the collision model for chemical reactions. 2. Sketch a molecular level diagram showing the collision of reactants to form products. 3. Explain how and why changes in concentration affect chemical reaction rate. 4. Describe the concept of “activation energy.” 5. Explain how and why changes in temperature affect chemical reaction rate. 6. Sketch and label an energy level diagram that shows the formation of products from reactants. 7. Describe “catalysts” and “enzymes.” 8. Sketch and label an energy level diagram that includes a catalyst. 9. Show with chemical equations that chlorine atoms (Cl) act as a catalyst in the destruction of ozone (O3). 10. Distinguish between homogeneous and heterogeneous reactions, and explain why the reaction between zinc metal and hydrochloric acid solution is heterogeneous. 11. Restate the four major factors that affect reaction rate. 12. Describe the condition of equilibrium. 13. Explain chemical equilibrium. 14. What do the double arrows in a chemical reaction indicate? 15. Explain the following statement: “Equilibrium is not static, it is a dynamic condition.” 16. Explain why equilibrium occurs. 17. Sketch and label a graph of reaction rate versus time to show how a reaction can reach equilibrium. 18. Describe the Law of Chemical Equilibrium and write a general equilibrium expression. Explain what the square brackets represent. 19. Describe the equilibrium constant. 20. Why must we first balance a chemical equation before we can write the equilibrium expression? 21. Explain the difference between “equilibrium Constant” and “equilibrium position.” 22. Distinguish between homogeneous equilibrium and heterogeneous equilibrium. 23. Which species are not included in the equilibrium expression? Explain. 24. Describe Le Chatlier’s Principle. 25. Use Le Chatlier’s Principle to describe and explain the effect of changing concentration on a system at equilibrium. Use the reaction between nitrogen gas and hydrogen gas to form ammonia n your explanation. 26. If a reactant is removed from a chemical system at equilibrium, what happens to the concentration of the products? 27. Use Le Chatlier’s Principle to describe and explain the effect of changing the volume on a gaseous system at equilibrium. Use the reaction between nitrogen gas and hydrogen gas to form ammonia in your explanation. 28. Use Le Chatlier’s Principle to describe and explain the effect of changing the temperature on a system at equilibrium for both an exothermic and an endothermic reaction. 29. What does the value of “K” the equilibrium constant tell us? 30. Describe on real life example of the importance of solubility Equilibria. 31. Describe the solubility product constant. 32. Do very soluble salts have large or small Ksp values?
