AP Chemistry/Kinetics Review

AP Chemistry/Kinetics review

AP Chemistry : Ch. 12 : Obj. 1-15 (Quantitative)

1. The average rate of appearance of ammonia in the reaction N2(g) + 3H2(g) --> 2 NH3(g) is found to be .25 atm/s over a certain period of time. What is the average rate of disappearance of nitrogen over the same time period?

a) .13 atm/s

b) .50 atm/s

c) .25 atm/s

d) .50 atm/s

2. For the above reaction under a different set of conditions, if the rate of disappearance of hydrogen is 1.0 atm/s, what would the rate of disappearance of nitrogen be?

a) .67 atm/s

b) 3.0 atm/s

c) .33 atm/s

d) .25 atm/s

3. The following information was obtained for the reaction X + Y --> Z. What is the rate law for this reaction?

a) Rate = k[X][Y]

b) Rate = k[X]2[Y]

c) Rate = k[X][Y]2

d) Rate = k[X]2[Y]2

4. What is the value of k for the above reaction?

a) 5.3 x 10-4

b) 2.2 x 10-5

c) 1.6 x 10-3

d) 8.7 x 10-1

5. What are the units for k in the above reaction?

a) L2/mol2 x s

b) L/mol x s

c) s-1

d) L3/mol3 x s

6. For the above reaction, what would the rate be if [X] = .060 M and [Y] = .080 M, under the same reaction conditions?

a) 2.3 x 10-6 mol/L x s

b) 4.1 x 10-8 mol/L x s

c) 8.5 x 10-6 mol/L x s

d) 4.6 x 10-7 mol/L x s

7. For a certain reaction the following data were obtained. Calculate the rate law from this data.

a) Rate = k[A][B][C]

b) Rate = k[A]2[B][C]

c) Rate = k[A][B]2[C]

d) Rate = k[A][B]

e) Rate = k[B][C]

8. What is the value of the rate constant for the above reaction?

a) .012

b) .88

c) .64

d) 24

e) 64

9. What are the units for the rate constant for the above reaction?

a) L/mol x s

b) L2/mol2 x s

c) L3/mol3 x s

d) s-1

10. What would the molar concentration of reactant C be ([C]) if the rate of the reaction was 4.8 mol/L x s and the concentration of B was .25M?

a) .10 M

b) .15 M

c) .20 M

d) .24 M

e) .30 M

11. What is the rate law for the reaction described by the following data?

a) Rate = k[X][Y]

b) Rate = k[X]2[Y]

c) Rate = k[X]

d) Rate = k[Y]

e) Rate = k

12. What is the value for the rate constant in the above reaction?

a) 1.2 x 10-3 s-1

b) 1.2 x 10-3 mol/L x s

c) 1.2 x 10-3 L/mol x s

d) 1.0

13. Determine the integrated rate law for the decomposition reaction of C2H5Cl from the following data

a) [C2H5Cl] = -kt + [C2H5Cl]0

b) ln[C2H5Cl] = -kt +ln [C2H5Cl]0

c) 1/[C2H5Cl] = kt + 1/[C2H5Cl]0

14. What is the value of the rate constant for the above reaction?

a) .025

b) .098

c) .11

d) .67

e) .89

15. What are the units for rate constant for the above reaction?

a) s-1

b) mol/L x s

c) L/mol x s

d) L2/mol2 x s

16. What would [C2H5Cl] be at t = 8.0 s?

a) .23 M

b) .22 M

c) .21 M

d) .20 M

e) .19 M

17. The following data were obtained for the decomposition of nitrous oxide (N2O). What is the integrated rate law for this reaction?

a) [N2O] = -kt + [N2O]0

b) ln[N2O] = -kt + ln[N2O]0

c) 1/[N2O] = kt + 1/[N2O]0

18. What is the value of the rate constant for the above reaction?

a) .244 L/mol x s

b) .451 L/mol x s

c) .692 L/mol x s

d) .885 L/mol x s

19. For the reaction of aA --> B, where [A]0 = .250 M, a plot of ln[A] vs t produced a straight line with a slope of -2.3 x 10-2. What is the half life of this reaction?

a) 15 s

b) 25 s

c) 30. s

d) 38 s

20. For the reaction of aA --> B, where [A]0 = .150 M, a plot of 1/[A] vs t (in seconds)produced a straight line with a slope of 5.5 x 10-4. What is the half life of this reaction?

a) .80 hrs

b) 1.6 hrs

c) 2.2 hrs

d) 3.4 hrs

21. How long would it take for the above reaction to be 75% complete?

a) 1.6 hrs

b) 4.4 hrs

c) 6.8 hrs

d) 10. hrs

22. A certain first order reaction is 42.0 % complete in 85 s. Calculate the rate constant for this reaction.

a) 3.1 x 10-4 s-1

b) 8.9 x 10-3 s-1

c) 6.4 x 10-3 s-1

d) 8.7 x 10-2 s-1

23. What is the half-life for the above reaction?

a) 58 s

b) 82 s

c) 110 s

d) 140 s

e) 190 s

24. How long would it take for the above reaction to be 90.0% complete?

a) 360 s

b) 320 s

c) 290 s

d) 250 s

25. The reaction A --> B + C is known to be zero order with a rate constant of 2.2 x 10-2 mol/L x s at 25 ºC. What is the rate law for this reaction where [A]0 is 1.20M?

a) 1/[A] = (2.2 x 10-2 mol/L x s)t + 1/1.20 M

b) ln[A] = -(2.2 x 10-2 mol/L x s )t + ln1.20 M

c) [A] = -(2.2 x 10-2 mol/L x s )t + 1.20 M

26. What is the half-life of the above reaction?

a) 27 s

b) 32 s

c) 39 s

d) 44 s

27. For a reaction A --> B + C, the half-lives were found to be 2.2 s, 4.4 s and 8.8 s. If [A]0 = .50 M, what will [A] be at t = 17.6 s?

a) .068 M

b) .056 M

c) .016 M

d) .0078 M

28. For the above reaction, what will [A] be at t = 80.0 s?

a) .23 M

b) .12 M

c) .095 M

d) .013 M

Answers : 1. a 2.c 3.b 4.c 5.a 6.d 7.e 8.e 9.a 10.e 11.e 12.b 13.b 14.c 15.a 16.c 17.c 18.a 19.c 20.d 21.d 22.c 23.c 24.a 25.c 26.a 27.b 28.d