1. 1. For the reaction A + B  C, the rate constant at 215 o C is 5.0 x 10 -3 1/s and the rate constant at 452 o C is 1.2 x 10 -1 1/s. What is the activation energy in kJ/mol?

2. 1. For the reaction A + B  C, the rate constant at 215 o C is 5.0 x 10 -3 1/s and the rate constant at 452 o C is 1.2 x 10 -1 1/s. What is the activation energy in kJ/mol?

3. 2. It took 143. seconds for 50.0% of a substance to decompose. If the initial concentration was 0.060 M and the reaction is first order, what is the value of the rate constant with units?

5. 3. The reaction 2NOBr  2NO + Br2 exhibits the rate law Rate = k[NOBr] 2 where k = 1.0 x10 – 5 M – 1  s – 1 at 25  C. This reaction is run where the initial concentration of NOBr ([NOBr] 0 ) is 1.00 x 10 – 1 M. What is one half-life for this experiment?

6. 3. The reaction 2NOBr  2NO + Br2 exhibits the rate law Rate = k[NOBr] 2 where k = 1.0 x10 – 5 M – 1  s – 1 at 25  C. This reaction is run where the initial concentration of NOBr ([NOBr] 0 ) is 1.00 x 10 – 1 M. What is one half-life for this experiment?

7. 4. The decomposition of a compound has a rate constant (k) = 0.208 1/min. How many minutes does it take for the concentration to drop from 0.50M to 0.10M?

8. 4. The decomposition of a compound has a rate constant (k) = 0.208 1/min. How many minutes does it take for the concentration to drop from 0.50M to 0.10M?

9. 5. A reaction exhibits has a value for k = 25.0 L/mol∙s at 420K. If the concentration of the reactant is originally 3.54 x 10 -3 M, what will the concentration be after 15.0 seconds?

10. 5. A reaction exhibits has a value for k = 25.0 L/mol∙s at 420K. If the concentration of the reactant is originally 3.54 x 10 -3 M, what will the concentration be after 15.0 seconds?

11. 6. The rate constant for the decomposition of a compound at 620K is 1.066 x 10 -4 s -1. How much time is required for the concentration of the compound to drop from 0.0300 M to 0.0125M?

12. 6. The rate constant for the decomposition of a compound at 620K is 1.066 x 10 -4 s -1. How much time is required for the concentration of the compound to drop from 0.0300 M to 0.0125M?

13. 7. The half-life of carbon-14 is 5730 years. Grain found is found to have a ratio of 14 C to 12 C that is 0.350 times that found in living organisms. Calculate the age of the grain.

15. 8. A graph of 1/[A] vs. time for a certain reaction is found to be a straight line. If 3.0 minutes is needed for the concentration of A to drop from 0.050M to 0.030M, what is the k value?

17. 9. Determine the activation energy for the reaction N 2 O 5  2NO 2 + ½ O 2 based on the following observed rate constants and temperatures. Temperature (°C) k (s -1 ) 25 3.46 x 10 -5 55 1.50 x 10 -3

18. 9. Determine the activation energy for the reaction N 2 O 5  2NO 2 + ½ O 2 based on the following observed rate constants and temperatures. Temperature (°C) k (s -1 ) 25 3.46 x 10 -5 55 1.50 x 10 -3

19. 10. The half life for uranium-238 is 4.5 x 10 9 years. What is the rate constant for the decay of 238 U?

20. 10. The half life for uranium-238 is 4.5 x 10 9 years. What is the rate constant for the decay of 238 U?