Rate Laws Worksheet

1. Kinetics is the study of the ___________.
   

 

 

2. What is a Rate Law?
   
• How is a rate law determined?
  

 

 

3. What are the two types of rate law and what does each compare?
   
• 
  
• 
  

 

 

4. The general appearance of a differential rate law is:
   

 

• Where k represents the ____ ________. 
  

 

• What are the units for k?
  

 

• Where n represents the ______  ___ ______.
  

 

• If n=1 this is said to be a ______ _______ reaction.
  
• If n=2 this is said to be a  ______ _______reaction.
  
• If n=0 this is said to be a  ______ _______reaction.
  

 

• If there is more than one reactant in a rate law you must _____ their n values to determine the overall order of the reaction.
  

 

 

5. For a zero order reaction
   

 

• What does zero order tell us with respect to concentration & rate?
  

 

• Differential Rate Law
  

 

• Integrated Rate Law
  

 

• How can we utilize this information?
  

 

• Half Life Equation
  

 

6. For a first order reaction
   

 

• What does first order tell us with respect to concentration & rate?
  

 

• Differential Rate Law
  

 

• Integrated Rate Law         
  

 

• What format is this equation written in?  How can we utilize this information?
  

 

• Half Life Equation
  

 

 

7. For a second order reaction
   

 

• What does second order tell us with respect to concentration & rate?
  

 

• Differential Rate Law
  

 

• Integrated Rate Law
  

 

• What format is this equation written in?  How can we utilize this information?
  

 

• Half Life Equation
  

 

8. Determine the differential rate law and rate constant for
   
   2NO_(g) + Cl_2(g)→ 2NOCl(g)
   

    

   given:                                                                                           

           [NO]_o             [Cl₂]_o               Initial Rate

 

          0.10 M          0.10 M           0.18 M/min
          0.10 M          0.20 M           0.36 M/min
          0.20 M          0.20 M           1.45 M/min

 

9. Determine the rate law for
   

    

   2NO_(g) + O_2(g)→2NO_2(g)
   
   given:
   

    

   [NO]_o                        [Cl₂]_o               Initial Rate
   

    

   1.66 x 10^-9    1.66 x 10^-9    3..32 x 10^-11
   1.98 x 10^-9    1.66 x 10^-9    2.99 x 10^-10
   4.15 x 10^-9    4.15 x 10^-9    5.20 x 10^-10
   

 

 

10. A certain reaction has the following general form
    
    aA→bB
    
    At a particular temperature and [A]₀=2.80 x 10^-3 M concentration versus time data were collected and a plot of 1/[A] versus time resulted in a straight line with a slope value of   +3.60 x 10^—2 L/mol*min
    

• Determine the differential and integrated rate laws and the value of the rate constant.
  
• Calculate the half-life for this reaction.
  
• How much time is required for the concentration of A to decrease to 2.50 x 10^-3M?
  

 

 

11. The decomposition of hydrogen peroxide was studied and the following data was obtained
    

     

    Time (s)         [H₂O₂] (M)
    

     

    0                      1
    120                 0.91
    300                 0.78
    600                 0.59
    1200              0.37
    1800              0.22
    2400              0.13
    3000              0.082
    3600              0.05
    

• Determine the integrated rate law, the differential rate law, and the value of the rate constant.        
  
• Calculate the [H₂O₂] at 4000. s after the start of the reaction.
  

 

 

12. A first order reaction is 75.0% complete in 320. s.
    

• What are the first and second half-lives for this reaction?
  

 

• How long does it take for this reaction to be 90.0% complete?