Level 1 — Basic Recall (1–10)

1. What is the definition of reaction rate?

2. What is the SI unit of reaction rate?

3. State the collision theory requirement for a reaction to occur.

4. Define activation energy.

5. What is a catalyst?

6. Define rate constant (k).

7. What is meant by “order of reaction”?

8. Write the general form of a rate law.

9. Define half-life of a reaction.

10. What is the Arrhenius equation?

Level 2 — Understanding (11–20)

11. Explain why increasing temperature increases reaction rate.

12. Why does increasing concentration increase reaction rate?

13. Describe how a catalyst affects activation energy.

14. Explain the difference between rate of reaction and rate constant.

15. Why does a higher activation energy correspond to a slower reaction?

16. Why is orientation important during molecular collisions?

17. Distinguish between zero-order and first-order reactions.

18. What does a straight line on a ln[A] vs time graph indicate?

19. Explain why the rate of reaction decreases over time.

20. How does pressure affect the rate of gaseous reactions?

Level 3 — Application (21–30)

21. Given rate = k[A], determine the order with respect to A.

22. Calculate half-life for a first-order reaction given k.

23. Sketch an energy profile diagram for a catalysed and uncatalysed reaction.

24. Use experimental data to determine the order of reaction.

25. Explain why some reactions appear instantaneous.

26. Predict the effect of doubling concentration on a second-order reaction.

27. Calculate the rate constant using experimental rate data.

28. Interpret a concentration–time graph to find rate at a specific point.

29. Explain the effect of surface area on heterogeneous reactions.

30. Calculate activation energy from an Arrhenius plot.

Level 4 — Analysis (31–40)

31. Analyse temperature dependence of rate constant using Arrhenius theory.

32. Compare reactions that follow the same rate law but have different activation energies.

33. Explain how intermediates affect the rate-determining step.

34. Determine the rate-determining step in a given mechanism.

35. Discuss why multi-step reactions have complex rate laws.

36. Compare catalytic and non-catalytic pathways using energy diagrams.

37. Analyse why enzyme catalysis follows saturation kinetics.

38. Predict the effect of inhibitors on reaction rate.

39. Evaluate how solvent polarity influences reaction rates.

40. Explain how molecular complexity affects rate of reaction.

Level 5 — Exam/Challenge (41–50)

41. Explain why first-order reactions have constant half-lives.

42. Given a multi-step mechanism, derive the overall rate law.

43. Compare collision theory with transition state theory.

44. Derive the Arrhenius equation in logarithmic form.

45. Use ln(k) vs 1/T graph to calculate activation energy.

46. Predict the effect of isotope substitution on reaction rate (kinetic isotope effect).

47. Analyse the mechanism of SN1 vs SN2 reactions using kinetics.

48. Evaluate the role of catalysis in industrial processes using numerical examples.

49. Given a reaction mechanism, identify intermediates and transition states.

50. Explain how activation entropy and enthalpy contribute to rate according to Eyring theory.