Reference no: EM132342049

Physical Chemistry II - (Chemical Kinetics)

GENERAL OBJECTIVES:

1. Understand the principles and applications of chemical kinetics

2.Understand the dynamics of molecular reactions

1. Define true rate in terms of the advancement of a reaction.

2. Describe how rates are measured experimentally

3. Derive the first and second order rate laws.

4. Define the rate coefficient of a reaction.

5. Define the order of a reaction.

6. Describe how the concentrations of reactants and products are monitored in a chemical reaction.
 
7.Define pseudo-first order rate law.

8. Describe Ostwald’s isolation method.

9. Define the half-life of a reaction.

10. Relate the half-life of a reaction to reaction order.

11. Explain the terms molecularity of reaction, mechanism of reaction, simple reaction.

12. Distinguish between order and molecularity of reaction.

13. Describe Arrhenius - type behaviour of simple reactions.

14. Explain the Arrhenius - type behaviour of bimolecular gas phase reactions.

15. Derive the rate laws for reactions involving equilibria.

16. Relate equilibrium constant to the rate coefficient of simple reactions

17. Derive the rate law for parallel reactions.

18. Derive the rate law for consecutive reactions.

19. Explain the steady - state approximation.

20. Define the rate - determining step of a reaction.

21. Derive the rate laws for reactions involving a preequilibrium.

22. Define the terms catalysts, acid catalyst and base catalyst and explain their mode of operation

2.1 State the collision theory of bimolecular gas-phase reactions.

2.2 Calculate the second - order rate coefficient from collision theory.

2.3 Define P-factor and the reactive cross-section.

2.4 Distinguish between diffusion - controlled and activation - controlled reactions in solution.

2.5 Relate the second order rate coefficient to the diffusion coefficient.

2.6 Relate the second order rate coefficient to viscosity.

2.7 Explain the terms - activated complex, reaction co-ordinate and transition state.

2.8 Describe the activated complex theory of reaction rates.

2.9 Define Gibb’s function of activation, entropy of activation and enthalpy of activation.

2.10 Explain the basis of the kinetic salt effect.

2.11 Derive the magnitude of kinetic salt effect.

2.12 Explain how molecular beams are used to study reactive collisions.

2.13 Sketch the potential - energy surface of a simple reaction.

2.14 Distinguish between attractive and repulsive surfaces and explain how they control the energy requirements of a reaction.