our assignment. . . .

Chapter 3 : Reaction Kinetics




3.1 Chemical Kinetics

Reaction Rates : - Change in concentration of reactants (or products) as a function of time
 

3.2 How to Express Reaction Rate

=> Rate = d[A] 
                   dt

     change in concentration of A over a period, t when 
     [A] decrease with time, change of [A] is -ve.


=> Unit : mol/Ls @ M/s

3.3 Differential Rate Equation

     aA + bB ---------> cC + dD

     

   
     * Keep In Mind : 2A ----> B means by 2 mol of A 
        dissappear in each mole B formed.

3.4 Rate Law

    - expressing rate as function of reactant 
     concentration and temperature

   - given aA + bB ----------> cC + dD, so the rate law 
      is :
     

 

    - also called rate equation

 3.5 Rate Equation

 

k = rate constant



- proportionally constant for a given reaction and     
   temperature.

        
- does not change as reaction proceed.

3.6 Reaction Orders

  => Define how the rate affected by reactant 
        concentration

  => Always determine by experimentally

  => Order or reaction is no related to stoichiometry 
        ceofficent of reactant in balance chemical eqn.

     

  

    

          

           Example 1 :

      

             

         Example 2 :

         Find the overall order from rate equation below :

           

          

             

           

    ORDERS

       

     OVERALL REACTION ORDERS

  

    KEEP IN MIND =)

    

   

 3.7 Integrated Rate Law 

 Function of integrated rate law :

 * can estimate the period taken for x mol/L of 

   compound A to be used up            

  * we can know the concentration of compound A after

    the reaction in specific time

 

            RATE = k [A]

 

 

 

 

    

 

 

 

        

    KEEP IN MIND =)