Objectives: To meet the requirements of Goal I, you must be able to:

1. describe the rate of a chemical reaction in terms of concentration and time.
   
2. understand average rate, instantaneous rate, and initial rate of a reaction.
   
3. understand rate constant, order of the reaction with respect to each reactant, half life of a first order reaction and a second order reaction. Understand and use integrated rate laws for first order and second order reactions (sample and follow-up problems 16.4, 16.5).

Objectives: To meet the requirements of Goal II, you must be able to:

4. study the relation between the rate constant and the identity of reactants.
   
5. understand the effect of a solvent on the reaction and the difference between reactions in solution and heterogeneous reactions.
   
6. study the Arrhenius Equation and understand the significance of activation energy. Work out problems using the Arrhenius Equation to solve for the new rate constant given the original rate constant, original temperature, and the new temperature (sample and follow-up problem 16.6).
   
7. understand how catalysts work; homogeneous, heterogeneous and enzymes.

Objectives: To meet the requirements of Goal III, you must be able to:

8. understand the Collision Theory.
   
9. understand the Activated Complex Theory.
   
10. predict the rate-determining step and the intermediates, given the reaction mechanism. 

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Objectives: To meet the requirements of Goal IV, you must be able to:

11. describe the condition known as chemical equilibrium by:
• defining “forward” and “reverse” reactions in an equilibrium system;
• describing the relative rates with which the forward and reverse reactions occur in a system at equilibrium.
  
12. distinguish between homogeneous and heterogeneous equilibria, and write the equilibrium constant expression from a balanced chemical equation for either type of equilibria.
    
13. relate the magnitude of the equilibrium constant for a given reaction:
• to the relative amounts of “reactants” and “products” present at equilibrium;
• to the speed with which equilibrium is reached, and explain what is meant saying a reaction “goes to completion.”
  
14. predict the direction of reaction from the reaction quotient, Q_c, and the numerical value of K_c, given concentrations of all chemical species involved in a reaction system which is not at equilibrium (sample and follow-up problem 17.5).
    
15. relate the numerical value of equilibrium constant to how the chemical equation is written and balanced. Understand the relationship between K_c forward, K_c reverse, and the two K_cs for two chemical equations that are related by a numeric factor (sample and follow-up problem 17.3).

Objectives: To meet the requirements of Goal V, you must be able to:

16. describe the effect on the numerical value of the equilibrium constant K_c for a system at equilibrium of:
• increasing or decreasing concentration of a reactant or product;
• increasing or decreasing the pressure on the system;
• changing the temperature of the system;
• adding a catalyst to the system.

17. describe qualitatively the effects on the amount of any specified component of a system at equilibrium of changing the conditions of the system by:
• changing the equilibrium concentration of a specified component;
• changing the pressure on the equilibrium system;
• changing the temperature of the system;
• adding a catalyst to the system.
  
18. understand the relationship between K_c and K_p, convert from one to the other (sample and follow-up problems 17.4). Calculate the K_c given the equilibrium concentration data (sample and follow-up problems 17.6). Calculate equilibrium concentrations given K_c (sample and follow-up problems 17.7 and 17.8). Learn to construct a reaction table (p. 737)