chemistryhelprush.wikispaces.comchemistryhelprush.wikispaces.com/file/view/12+and+13+ap... · web...

AP Chemistry Practice Test Zumdahl Chapter 12 Kinetics and 13 EquilibriumThis is converted using RTF so some of the symbols are strange. Infinity is really times.Looks like has been replaced by an O with a slash. You should be able to figure out most of them. Sorry, but I don’t have time to do more.

1. The average rate of disappearance of ozone in the reaction is found to be 8.49 10–3 atm over a certain interval of time. What is the rate of appearance of O2 during this interval?

A) 12.7 10–3 atm/s B) 8.49 10–3atm/s C) 5.66 10–3atm/s D) 306 10–3atm/s E) 24.0 10–3atm/s

2. The balanced equation for the reaction of bromate ion with bromide ion in acidic solution is given by:

At a particular instant in time, the value of –[Br–]/t is 2.0 10–3 mol/L s. What is the value of [Br2]/t in the same units?

A) 1.2 10–3 B) 2.0 10–3 C) 3.3 10–3 D) 1.0 10–3 E) 1.7 10–3

3. Consider the reaction 2H2 + O2 2H2OWhat is the ratio of the initial rate of the appearance of water to the initial rate of disappearance of oxygen?

A) 1 : 1 B) 2 : 1 C) 1 : 2 D) 2 : 2 E) 3 : 2

4. Consider the reaction: 4NH3 + 7O2 4NO2 + 6H2OAt a certain instant the initial rate of disappearance of the oxygen gas is X. What is the value of the appearance of water at the same instant?

A) 1.2 X B) 1.1 X C) 0.86 X D) 0.58 X E) cannot be determined from the data

5. For the reaction 5A + 3B ? 5C + 4D, at a particular instant in time, the rate of the reaction is 0.0272 M/s. What is the rate of change of A?

A) –0.0272 M/s B) 0.136 M/s C) –0.136 M/s D) –0.00544 M/s E) 0.00544 M/s

6. Consider the reaction X Y + ZWhich of the following is a possible rate law?

A) Rate = k[X] B) Rate = k[Y] C) Rate = k[Y][Z] D) Rate = k[X][Y] E) Rate = k[Z]

7. Consider the following rate law: Rate = k[A]n[B]mHow are the exponents n and m determined?

A) by using the balanced chemical equation B) by using the subscripts for the chemical formulas C) by using the coefficients of the chemical formulas D) by educated guess E) by experiment

8. The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm3 and rates are in molecules/cm3s.[NO]0 [O2]0 Initial Rate1 ¥ 1018 1 ¥ 1018 2.0 ¥ 1016

2 ¥ 1018 1 ¥ 1018 8.0 ¥ 1016

3 ¥ 1018 1 ¥ 1018 18.0 ¥ 1016

1 ¥ 1018 2 ¥ 1018 4.0 ¥ 1016

1 ¥ 1018 3 ¥ 1018 6.0 ¥ 1016

What is the rate law? A) Rate = k[NO][O2] B) Rate = k[NO][O2]2 C) Rate = k[NO]2[O2] D) Rate = k[NO]2 E) Rate = k[NO]2[O2]2

9. The reaction of (CH3)3CBr with hydroxide ion proceeds with the formation of

(CH3)3COH. (CH3)3CBr(aq) + OH–(aq) (CH3)3COH(aq) + Br–(aq)The following data were obtained at 55C.

[(CH3)3CBr]0 [OH–]0 Initial RateExp. (mol/L) (mol/L) (mol/L)1 0.10 0.10 1.0 ¥ 10–3

2 0.20 0.10 2.0 ¥ 10–3

3 0.10 0.20 1.0 ¥ 10–3

4 0.30 0.20 ?What will the initial rate (in mol/L·s) be in Experiment 4? A) 3.0 10–3 B) 6.0 10–3 C) 9.0 10–3 D) 18 10–3 E) none of these

10. For a reaction in which A and B react to form C, the following initial rate data were obtained:

[A] [B] Initial Rate of Formation of C

(mol/L) (mol/L) (mol/L·s)0.10 0.10 1.000.10 0.20 4.000.20 0.20 8.00

What is the rate law? A) Rate = k[A][B] B) Rate = k[A]2[B] C) Rate = k[A][B]2 D) Rate = k[A]2[B]2 E) Rate = k[A]3

11. Tabulated below are initial rate data for the reaction 2Fe(CN)63– + 2I– 2Fe(CN)64– + I2

InitialRun [Fe(CN)6

3–]0 [I–]0 [Fe(CN)64–]0 [I2]0 Rate (M/s)

1 0.01 0.01 0.01 0.01 1 ¥ 10–5

2 0.01 0.02 0.01 0.01 2 ¥ 10–5

3 0.02 0.02 0.01 0.01 8 ¥ 10–5

4 0.02 0.02 0.02 0.01 8 ¥ 10–5

5 0.02 0.02 0.02 0.02 8 ¥ 10–5

The experimental rate law is: A) = k[Fe(CN)63–]2[I–]2[Fe(CN)64–]2[I2] B) = k[Fe(CN)63–]2[I–][Fe(CN)64–][I2]

C) = k[Fe(CN)63–)]2[I–] D) = k[Fe(CN)63–][I–]2 E) = k[Fe(CN)63–][I–] [Fe(CN)64–]

12. Tabulated below are initial rate data for the reaction: 2Fe(CN)63– + 2I– 2Fe(CN)64– + I2

Run [Fe(CN)63–]0 [I–]0 [Fe(CN)6

4–]0 [I2]0 Rate (M/s)1 0.01 0.01 0.01 0.01 1 ¥ 10–5

2 0.01 0.02 0.01 0.01 2 ¥ 10–5

3 0.02 0.02 0.01 0.01 8 ¥ 10–5

4 0.02 0.02 0.02 0.01 8 ¥ 10–5

5 0.02 0.02 0.02 0.02 8 ¥ 10–5

What is the value of k? A) 107 M–5 s–1 B) 103 M–3 s–1 C) 10 M–2 s–1 D) 50 M–2 s–1 E) none of these

Use the following to answer questions 13-18.

A general reaction written as A + 2B C + 2D is studied and yields the following data:[A]0 [B]0 Initial D[C]/Dt0.150 M 0.150 M 8.00 ¥ 10–3 mol/L·s0.150 M 0.300 M 1.60 ¥ 10–2 mol/L·s

0.300 M 0.150 M 3.20 ¥ 10–2 mol/L·s

13. What is the order of the reaction with respect to B? A) 0 B) 1 C) 2 D) 3 E) 4

14. What is the order of the reaction with respect to A? A) 0 B) 1 C) 2 D) 3 E) 4

15. What is the overall order of the reaction? A) 0 B) 1 C) 2 D) 3 E) 4

16. What is the numerical value of the rate constant? A) 0.053 B) 1.19 C) 2.37 D) 5.63 E) none of these (A-D)

17. Determine the initial rate of B consumption ([B]/t) for the first trial? A) 8.00 10–3 mol/L·s B) 1.60 10–2 mol/L·s C) 3.20 10–2 mol/L·s D) 4.00 10–3 mol/L·s E) none of these (A-D)

18. Determine the initial rate of C production ([C]/t) if [A] = 0.200 M and [B] = 0.500 M.

A) 4.74 10–2 mol/L·s B) 2.37 10–1 mol/L·s C) 1.19 10–1 mol/L·s D) 8.23 10–2 mol/L·s E) none of these (A-D)


Consider the following data concerning the equation: H2O2 + 3I– + 2H+ I3– + 2H2O

[H2O2] [I–] [H+] rate I 0.100 M 5.00 10–4 M 1.00 10–2 M 0.137 M/sec II. 0.100 M 1.00 10–3 M 1.00 10–2 M 0.268 M/sec III. 0.200 M 1.00 10–3 M 1.00 10–2 M 0.542 M/sec IV. 0.400 M 1.00 10–3 M 2.00 10–2 M 1.084 M/sec

19. The rate law for this reaction is A) rate = k[H2O2][I–][H+] B) rate = k[H2O2]2[I–]2[H+]2 C) rate = k[I–][H+] D) rate = k[H2O2][H+] E) rate = k[H2O2][I–]

20. The average value for the rate constant k (without units) is A) 2710 B) 2.74 104 C) 137 D) 108 E) none of these

21. Two mechanisms are proposed:

A) Mechanism I, with the first step the rate determining step. B) Mechanism I, with the second step the rate determining step. C) Mechanism II, with the first step rate determining. D) Mechanism II, with the second step rate determining. E) None of the above could be correct.


The following initial rate data were found for the reaction2MnO4

– + 5H2C2O4 + 6H+ Æ 2Mn2+ + 10CO2 + 8H[MnO4

–]0 [H2C2O4]0 [H+]0

1 ¥ 10–3 1 ¥ 10–3 1.02 ¥ 10–3 1 ¥ 10–3 1.02 ¥ 10–3 2 ¥ 10–3 1.0

2 ¥ 10–3 2 ¥ 10–3 2.0

22. Which of the following is the correct rate law? A) Rate = k[MnO4–]2[H2C2O4]5[H+]6 B) Rate = k[MnO4–]2[H2C2O4][H+] C) Rate = k[MnO4–][H2C2O4][H+] D) Rate = k[MnO4–]2[H2C2O4] E) Rate = k[MnO4–]2[H2C2O4]2

23. What is the value of the rate constant? A) 2 105 Ms–1 B) 2 105 M–2s–1 C) 200 M–1s–1 D) 200 M–2s–1 E) 2 10–4 Ms–1


The following questions refer to the reaction between nitric oxide and hydrogen 2NO + H2 N2O + H2OExperiment Initial [NO], M Initial [H2], M Initial Rate of Disappearance of

NO (mol/L sec)1 6.4 ¥ 10–3 2.2 ¥ 10–3 2.7 ¥ 10–5

2 12.8 ¥ 10–3 2.2 ¥ 10–3 1.1 ¥ 10–4

3 6.4 ¥ 10–3 4.5 ¥ 10–3 5.4 ¥ 10–5

24. What is the rate law for this reaction? A) Rate = k[NO] B) Rate = k[NO]2 C) Rate = k[NO]2[H2] D) Rate = k[NO][H2] E) Rate = k[N2O][H2O]

25. What is the magnitude of the rate constant for this reaction? A) 0.66 B) 4.2 10–3 C) 870 D) 1.9 E) 300

26. What are the units for the rate constant for this reaction? A) L/mol·s B) L2/mol2·s C) mol/L·s D) s–2 E) L–2

27. What is the order of this reaction?

A) 3 B) 2 C) 1 D) 0 E) cannot be determined from the data


The reaction H2SeO3(aq) 6I–(aq) + 4H+(aq) 2I3–(aq) + 3H2O(l) + Se(s) was studied at 0°C by the method of initial rates:

[H2SeO3]0 [H+]0 [I–]0 Rate (mol/L s)1.0 ¥ 10–4 2.0 ¥ 10–2 2.0 ¥ 10–2 1.66 ¥ 10–7

2.0 ¥ 10–4 2.0 ¥ 10–2 2.0 ¥ 10–2 3.33 ¥ 10–7

3.0 ¥ 10–4 2.0 ¥ 10–2 2.0 ¥ 10–2 4.99 ¥ 10–7

1.0 ¥ 10–4 4.0 ¥ 10–2 2.0 ¥ 10–2 6.66 ¥ 10–7

1.0 ¥ 10–4 1.0 ¥ 10–2 2.0 ¥ 10–2 0.41 ¥ 10–7

1.0 ¥ 10–4 2.0 ¥ 10–2 4.0 ¥ 10–2 13.4 ¥ 10–7

1.0 ¥ 10–4 4.0 ¥ 10–2 4.0 ¥ 10–2 5.33 ¥ 10–6

28. The rate law is A) Rate = k[H2SeO3][H+][I–] B) Rate = k[H2SeO3][H+]2[I–] C) Rate = k[H2SeO3][H+][I–]2 D) Rate = k[H2SeO3]2[H+][I–] E) Rate = k[H2SeO3][H+]2[I–]3

29. The numerical value of the rate constant is A) 5.2 105 B) 2.1 102 C) 4.2 D) 1.9 10–6 E) none of these


The following questions refer to the reaction shown below:

Initial Rate ofInitial [A] Initial [B] Disappearance of A

Experiment (mol/L) (mol/L) (mol/L·s)1 0.16 0.15 0.08

2 0.16 0.30 0.303 0.08 0.30 0.08

30. What is the rate law for this reaction? A) Rate = k[A][B] B) Rate = k[A]2[B] C) Rate = k[A][B]2 D) Rate = k[A]2[B]2 E) Rate = k[B]

31. What is the magnitude of the rate constant for the reaction? A) 140 B) 79 C) 119 D) 164 E) 21

32. What are the units for the rate constant for this reaction? A) L/mol·s B) L2/mol2·s C) mol/L·s D) L3/mol3·s E) mol3/L

33. What is the order of this reaction? A) 4 B) 3 C) 2 D) 1 E) 0

34. Initial rate data have been determined at a certain temperature for the gaseous reaction 2NO + 2H2 N2 + 2H2O.[NO]0 [H2]0 Initial Rate (M/s)0.10 0.20 0.01500.10 0.30 0.02250.20 0.20 0.0600

What is the value of the rate constant? A) 7.5 B) 3.0 10–3

C) 380 D) 0.75 E) 3.0 10–4

35. The following data were obtained at 25°C:[A]0 [B]0 [C]0 Rate0.1 0.2 0.3 0.0630.3 0.4 0.2 0.0840.6 0.4 0.2 0.1680.3 0.4 0.1 0.0210.6 0.2 0.2 0.168

What is the correct rate law? A) Rate = k[A][B][C] B) Rate = k[A][B][C]2 C) Rate = k[A][C] D) Rate = k[A]3[B]2[C] E) Rate = k[A][C]2


The oxidation of Cr3+ to CrO42– can be accomplished using Ce4+ in a buffered solution. The following data were obtained:

RelativeInitial Rate [Ce4+]0 [Ce3+]0 [Cr3+]0

1 2.0 ¥ 10–3 1.0 ¥ 10–2 3.0 ¥ 10–2

2 4.0 ¥ 10–3 2.0 ¥ 10–2 3.0 ¥ 10–2

4 4.0 ¥ 10–3 1.0 ¥ 10–2 3.0 ¥ 10–2

16 8.0 ¥ 10–3 2.0 ¥ 10–2 6.0 ¥ 10–2

36. Determine the order in the rate law of the species Ce4+. A) 1 B) 2 C) 3 D) –1 E) –2

37. Determine the order in the rate law of the species Ce3+. A) 1 B) 2

C) 3 D) –1 E) –2

38. Determine the order in the rate law of the species Cr3+. A) 1 B) 2 C) 3 D) –1 E) –2

39. The rate expression for a particular reaction is rate = k[A][B]2. If the initial concentration of B is increased from 0.1 M to 0.3 M, the initial rate will increase by which of the following factors?

A) 2 B) 6 C) 12 D) 3 E) 9

40. The following data were obtained for the reaction 2A + B C where rate = [C]/t[A](M) [B](M) Initial Rate (M/s)0.100 0.0500 2.13 ¥ 10–4

0.200 0.0500 1.70 ¥ 10–2

0.400 0.100 1.36 ¥ 10–1

What is the value of the rate constant? A) 2.13 B) 0.213 C) 0.426 D) 1.70 E) none of these

41. The reaction 2A + 5B ? products is third order in A and third order in B. What is the rate law for this reaction?

A) rate = k[A]2[B]5 B) rate = k[A]3[B]3 C) rate = k[A]3[B]3 D) rate = k[A]5[B]2 E) rate = k[A]2/7[B]5/7

42. The reaction 3A + 4B ? products is first order in A and third order in B. What is the

overall order of the reaction? A) 0 B) 7 C) 1 D) 4 E) 3

43. The reactants A and B are mixed, and the reaction is timed until a color change occurs. The data are as follows:

[A] [B] Time (s) 0.100 0.140 250.050 0.140 500.100 0.070 100

The order of the reaction in terms of B is A) 2. B) 1/2. C) 0. D) –1/2. E) 1.

44. The reaction has the following rate law:

After a period of 2.4 103 s, the concentration of NO falls from an initial value of 2.8 10–3 mol/L to 2.0 10–3 mol/L. What is the rate constant, k?

A) 1.7 10–7 M–1·s–1 B) 6.0 10–2 M–1·s–1 C) 3.6 10–1 M–1·s–1 D) 1.4 10–4 M–1·s–1 E) 3.0 10–2 M–1·s–1

45. The following data were collected for the decay of HO2 radicals:Time [HO2] Time [HO2]0 s 1.0 ¥ 1011 molec/cm3 14 s 1.25 ¥ 1010 molec/cm3

2 s 5.0 ¥ 1010 molec/cm3 30 s 6.225 ¥ 109 molec/cm3

6 s 2.5 ¥ 1010 molec/cm3

A) The decay of HO2 occurs by a first-order process. B) The half-life of the reaction is 2 ms. C) A plot of ln [HO2] versus time is linear with a slope of –k. D) The rate of the reaction increases with time. E) A plot of 1/[HO2] versus time gives a straight line.

46. A first-order reaction is 45% complete at the end of 36 minutes. What is the length of the half-life of this reaction?

A) 42 min B) 31 min C) 2.2 h D) 52 min E) none of these


The following questions refer to the gas-phase decomposition of ethylene chloride.C2H5Cl products

Experiment shows that the decomposition is first order.The following data show kinetics information for this reaction:

Time (s) ln [C2H5Cl] (M) 1.0 –1.625 2.0 –1.735

47. What is the rate constant for this decomposition? A) 0.29/s B) 0.35/s C) 0.11/s D) 0.02/s E) 0.22/s

48. What was the initial concentration of the ethylene chloride? A) 0.29 M B) 0.35 M C) 0.11 M D) 0.02 M E) 0.22 M

49. What would the concentration be after 5.0 seconds? A) 0.13 M B) 0.08 M C) 0.02 M

D) 0.19 M E) 0.12 M

50. What is the half-life time for this reaction? A) 0.7 s B) 1.3 s C) 8.9 s D) 6.3 s E) 2.2 s

51. For a reaction: aAProducts, [A]0 = 5.4 M, and the first two half-lives are 56 and 28 minutes, respectively. Calculate k (without units).

A) 9.6 10–2 B) 3.3 10–3 C) 4.8 10–2 D) 6.6 10–3 E) none of these

52. For a reaction: aAProducts, [A]0 = 6.0 M, and the first two half-lives are 56 and 28 minutes, respectively. Calculate [A] at t = 105.3 minutes.

A) 5.6 M B) 12 M C) 0.71 M D) 0.36 M E) none of these

53. For which order reaction is the half-life of the reaction proportional to 1/k (k is the rate constant)?

A) zero order B) first order C) second order D) all of the above E) none of the above


The kinetics of the reaction A + 3B C + 2D were studied and the following results obtained, where the rate law is:

–DSMTEF0501010502425245453500001357696E416C6C4261736963436F64

65506167657300110554696D6573204E657720526F6D616E00110353796D626F6C0011044D5420457874726100120008212F458F442F4150F4100F475F4150F21F1E4150F4150F4100F445F425F48F425F4100F4100F435F4100F48F45F42A5F48F48F4100F4100F40F48F417F48F4100F412A5F445F45F45F45F45F410F0C0100010001020202020002000101010000000300000A010003000B00000100020485940344030003030001000200814100000200965B000200965D0000000100020485940344020083

740000000000

At

= k[A]n[B]m

For a run where [A]0 = 1.0 10–3 M and [B]0 = 5.0 M, a plot of ln [A] versus t was found to give a straight line with slope = –5.0 10–2 s–1.For a run where [A]0 = 1.0 10–3 M and [B]0 = 10.0 M, a plot of ln [A] versus t was found to give a straight line with slope = –7.1 10–2 s–1.

54. What is the value of n? A) 0 B) 0.5 C) 1 D) 1.5 E) 2

55. What is the value of m? A) 0 B) 0.5 C) 1 D) 1.5 E) 2

56. Calculate the value of k (ignore units). A) 22 B) 10 C) 50 D) 1.1 E) none of these


For the reaction 2N2O5(g) 4NO2(g) + O2(g), the following data were collected:t (minutes) [N2O5] (mol/L)0 1.24 ¥ 10–2

10. 0.92 ¥ 10–2

20. 0.68 ¥ 10–2

30. 0.50 ¥ 10–2

40. 0.37 ¥ 10–2

50. 0.28 ¥ 10–2

70. 0.15 ¥ 10–2

57. The order of this reaction in N2O5 is A) 0 B) 1 C) 2 D) 3 E) none of these

58. The concentration of O2 at t = 10. minutes is A) 2.0 10–4 mol/L B) 0.32 10–2 mol/L C) 0.16 10–2 mol/L D) 0.64 10–2 mol/L E) none of these

59. The initial rate of production of NO2 for this reaction is approximately A) 7.4 10–4 mol/L·min B) 3.2 10–4 mol/L·min C) 1.24 10–2 mol/L·min D) 1.6 10–4 mol/L·min E) none of these

60. The half-life of this reaction is approximately A) 15 minutes B) 18 minutes C) 23 minutes D) 36 minutes E) 45 minutes

61. The concentration N2O5 at 100 minutes will be approximately

A) 0.03 10–2 mol/L B) 0.06 10–2 mol/L C) 0.10 10–2 mol/L D) 0.01 10–2 mol/L E) none of these


The following questions refer to the hypothetical reaction A + B products. The kinetics data given can be analyzed to answer the questions.

[A]0 [B]0 Rate of decrease(mol/L) (mol/L) of [A] (M/s)5.0 5.0 X10.0 5.0 2X5.0 10.0 2XTime (s) [B] (mol/L)10.0 10020.0 100

30.0 100

62. The rate law for the reaction is Rate = k[A]x[B]y. What are the values of x and y? A) x = 0 y = 1 B) x = 1 y = 0 C) x = 1 y = 1 D) x = 2 y = 1 E) x = 1 y = 2

63. What form will the pseudo-rate law have? A) Rate = k'[A]x B) Rate = k'[B]y C) Rate = k'[A]x[B]y D) Rate = kk'[A]x E) Rate = kk'[B]y

64. Determine the magnitude of the pseudo-rate constant (k') if the magnitude of X in the rate data is 0.00905.

A) 4.3 10–3 B) 1.2 10–2 C) 0.86 D) 0.31 E) 1.81 10–3


The reaction A B + C is known to be zero order in A with a rate constant of 5.0 10–2 mol/L·s at 25°C. An experiment was run at 25°C where [A]0 = 1.0 10–3 M.

65. The integrated rate law is A) [A] = kt B) [A] – [A]0 = kt C) D) ln E) [A]0 – [A] = kt

66. What is the concentration of B after 5 10–3 sec? A) 5.0 10–5 M B) 5.0 10–4 M C) 7.5 10–4 M D) 2.5 10–4 M E) none of these

67. The reaction is known to be zero order in A with a rate constant of 5.0 10–2 mol/L s at 25°C. An experiment was run at 25°C where [A]0 = 3.0 10–3 M. After 5.0 minutes, the rate is

A) 5.0 10–2 mol/L·s B) 2.5 10–2 mol/L·s C) 1.3 10–2 mol/L·s D) 3.0 10–3 mol/L·s E) none of these

68. The reaction is known to be zero order in A with a rate constant of 5.0 10–2 mol/L s at 25°C. An experiment was run at 25°C where [A]0 = 3.0 10–3 M. The half-life for the reaction is

A) 3.0 10–2s B) 3.0 102s C) 5.0 10–2 s D) 6.0 10–4s E) none of these

69. The reaction

exhibits the rate law

where k = 1.0 10–5 M–1 s–1 at 25°C. This reaction is run where the initial concentration of NOBr ([NOBr]0) is 0.15 M. What is one half-life for this experiment?

A) 1.5 s B) 0.8 10–5 s C) 6.9 10–4 s D) 6.7 105 s E) none of these

70. The reaction2NOBr 2NO + Br2

exhibits the rate lawRate = k[NOBr]2 = – DSMTEF0501010502425245453500001357696E416C6C4261736963436F6465506167657300110554696D6573204E657720526F6D616E00110353796D626F6C0011044D5420457874726100120008212F458F442F4150F4100F475F4150F21F1E4150F4150F4100F445F425F48F425F4100F4100F435F4100F48F45F42A5F48F48F4100F4100F40F48F417F48F4100F412A5F445F45F45F45F45F410F0C0100010001020202020002000101010000000300000A010003000B00000100020485940344030003030001000200814E000200814F0002008142000200817200000200965B000200965D00000001000204859403440200837

40000000000

NOBrt

where k = 1.0 10–5 M–1 s–1 at 25°C. This reaction is run where the initial concentration of NOBr ([NOBr]0) is 1.00 10–1 M.The [NO] after 1.00 hour has passed is A) 3.6 10–4 M B) 9.9 10–3 M C) 9.7 10–3 M D) 1.0 10–3 M E) none of these


For the reaction A Products, successive half-lives are observed to be 10.0 min and 40.0 min.

71. The reaction follows the integrated rate law A) [A] = –kt + [A]0 B) ln [A] = –kt + ln [A]0 C) = kt + D) = kt + E) none of these

72. At the beginning of the reaction, [A] was 0.68 M. The numerical value of the rate constant is

A) 0.069 B) 0.15 C) 10. D) 0.034 E) none of these

73. The reaction

is first order in N2O5. For this reaction at 45oC, the rate constant k = 1.0 10–5 s–1, where the rate law is defined as

For a particular experiment ([N2O5]0 = 1.0 10–3 M), calculate [N2O5] after 2.7 105 seconds.

A) 2.7 M B) 1.0 10–3 M C) 6.7 10–5 M D) 0 M E) 9.6 M


Consider the reaction 3A + B + C D + E where the rate law is defined as – = k[A]2[B][C] An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 10–4 M.

74. After 3.00 minutes, [A] = 3.26 10–5 M. The value of k is A) 6.23 10–3 L3/mol3·s B) 3.26 10–5 L3/mol3·s C) 1.15 102 L3/mol3·s D) 1.00 108 L3/mol3·s E) none of these

75. The half-life for this experiment is A) 1.11 102 s B) 87.0 s C) 6.03 10–3 s D) 117 s E) none of these

76. The concentration of C after 10.0 minutes is A) 1.00 M B) 1.10 10–5 M C) 0.330 M D) 0.100 M E) none of these

77. The concentration of A after 10.0 minutes is A) 1.06 10–9 M B) 2.38 10–6 M C) 9.80 10–6 M D) 1.27 10–5 M E) none of these

78. The reactionA B + C

is second order in A. When [A]0 = 0.100 M, the reaction is 20.0% complete in 28.7 minutes. Calculate the value of the rate constant (in L/min·mol).

A) 8.71 10–2 B) 6.97 10–4 C) 1.96 D) 1.39 E) none of these

79. The reactionA B + C

is second order in A. When [A]0 = 0.100 M, the reaction is 20.0% complete in 43.1 minutes. Calculate the half-life for the reaction.

A) 1.72 102 min B) 10.8 min C) 2.15 104 min D) 7.66 min E) none of these

80. A first-order reaction is 40.0% complete at the end of 42.6 minutes. What is the value of the rate constant (in min–1)?

A) 2.15 10–2 B) 1.20 10–2 C) 83.4 D) 46.5 E) none of these

81. The OH· radical disproportionates according to the elementary chemical reaction This reaction is second order in OH·. The rate constant for the reaction is 2.0 10–12 cm3/molecules at room temperature. If the initial OH· concentration is 1.9 1013 molecules/cm3, what is the first half-life for the reaction?

A) 3.5 1011 s B) 3.8 101 s C) 2.6 10–2 s D) 5.3 10–14 s E) 1.3 10–2 s

82. At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 11.9 s?

A) 6.4 1014 B) 3.4 101 C) 1.0 1016 D) 1.9 1014 E) 2.3 10–1

83. At a given temperature, a first-order reaction has a rate constant of 2.5 10–3 s–1. The time required for the reaction to be 28% completed is

A) 8.5 min B) 0.95 min C) 29 min D) 2.2 min E) 22 min

84. A chemical reaction that is first order in X is observed to have a rate constant of 1.8 10–2s–1. If the initial concentration of X is 1.0 M, what is the concentration of X after 195 s?

A) 33 M B) 0.65 M

C) 0.22 M D) 0.97 M E) 0.030 M

85. A particular first-order reaction has a rate constant of 0.0485 hr–1. What is the half-life for this reaction?

A) 1.00 hr B) 14.3 hr C) 20.6 hr D) 0.0699 hr E) 0.0485 hr

86. The reaction A ? products is first order. If the initial concentration of A is 0.631 M and, after 46.6 seconds have elapsed, the concentration of A has fallen to 0.0307 M, what is the rate constant of the reaction?

A) 0.0649 s–1 B) 0.0149 s–1 C) 0.0129 s–1 D) 0.665 s–1 E) 0.0215 s–1

87. The reaction A ? products is second order. If the initial concentration of A is 0.506 M and, after 16.7 seconds have elapsed, the concentration of A has fallen to 0.0528 M, what is the rate constant of the reaction?

A) 0.135 M–1 s–1 B) 1.02 M–1 s–1 C) 0.0415 M–1 s–1 D) 0.0271 M–1 s–1 E) 0.0599 M–1 s–1

88. The radioactive nuclide 185Ta undergoes first-order decay with a half-life of 49.4 min. If a quantity of 185Ta is produced, what fraction remains after 75.0 seconds?

A) 0.659 B) 0.349 C) 0.0253 D) 0.983 E) 0.0174

89. 63Ni decays by a first-order process via the emission of a beta particle. The 63Ni isotope has a half-life of 100. years. How long will it take for 83% of the nickel to undergo decay?

A) 27 years B) 1.2 years C) 110 years D) 12 years E) 260 years


Two isomers (A and B) of a given compound dimerize as follows:

2A A2

2B B2

Both processes are known to be second order in reactant, and k1 is known to be

0.25 L/mol·s at 25°C, where

Rate = – = k1[A]2

In a particular experiment, A and B were placed in separate containers at 25°, where

[A]0 = 1.0 10–2 M and [B]0 = 2.5 10–2 M. It was found that [A] = 3[B] after the reactions progressed for 3.0 minutes.

90. Calculate the concentration of A2 after 3.0 minutes. A) 2.8 10–22 M B) 6.9 10–3 M C) 3.1 10–3 M D) 1.6 10–3 M E) none of these

91. Calculate the value of k2 where Rate = – = k2[B]2

A) 2.2 L/mol·s B) 0.75 L/mol·s C) 1.9 L/mol·s D) 0.21 L/mol·s E) none of these

92. Two isomers (A and B) of a given compound dimerize as follows:2A A22B B2

Both processes are known to be second order in reactant, and k1 is known to be 0.29 L/mol·s at 25°C, where:

In a particular experiment, A and B were placed in separate containers at 25oC, where [A]0 = 1.0 10–2 M and [B]0 = 2.5 10–2 M. It was found that [A] = 3[B] after the reactions progressed for 3.0 minutes. Calculate the half-life for the reaction involving A.

A) 3.4 102 s B) 1.0 102 s C) 1.8 102 s D) 2.9 103 s E) none of these

93. The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is:

where k = 3.4 10–5 s–1 at 25°C, what is the initial rate of reaction at 25°C where [N2O5]0 = 6.4 10–2 M?

A) 3.4 10–5 mol/L·s B) 2.2 10-6 mol/L·s C) 5.3 10–4 mol/L·s D) 6.4 10–2 mol/L·s E) none of these

94. The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is:

where k = 3.4 10–5 s–1 at 25°C, what is the half-life for the reaction described? A) 2.9 104 s B) 2.0 104 s C) 8.7 108 s D) 4.9 10–5 s E) none of these

95. Consider a reaction of the type aA Products in which the rate law is found to be rate = k[A]3 (yes, a termolecular reaction is improbable but possible). If the first half-life of the reaction is found to be 40 seconds, what is the time for the second half-life?

A) 10 seconds B) 20 seconds C) 80 seconds D) 160 seconds E) 320 seconds

96. The reaction 2NO2 2NO + O2 obeys the rate law:at 500. K.

If the initial concentration of NO2 is 1.00 M, how long will it take for the [NO2] to decrease to 14.2% of its initial value?

A) 61.3 s B) 139 s C) 432 s D) 1.40 10–2 s E) cannot be determined from this data

97. If the reaction 2HI H2 + I2 is second order, which of the following will yield a linear plot?

A) log [HI] vs time B) 1/[HI] vs time C) [HI] vs time D) ln [HI] vs time E) None of these.

98. The reaction 3NO N2O + NO2 is found to obey the rate law, Rate = k[NO]2. If the first half-life of the reaction is found to be 2.0 s, what is the length of the fourth half-life?

A) 2.0 s B) 4.0 s C) 8.0 s D) 12.0 s E) 16.0 s

99. In 6 M HCl, the complex ion Ru(NH3)63+ decomposes to a variety of products. The reaction is first order in Ru(NH3)63+ and has a half-life of 14 hours at 25°C. Under these conditions, how long will it take for the [Ru(NH3)63+] to decrease to 13.4% of its initial value?

A) 2.9 hours B) 9.7 hours C) 1.9 hours D) 14 hours E) 41 hours

100. The elementary chemical reaction O + ClO Cl + O2 is made pseudo-first order in oxygen atoms by using a large excess of ClO radicals. The rate constant for the reaction is 2.6 cm3/molecules. If the initial concentration of ClO is 1.0 1011 molecules/cm3, how long will it take for the oxygen atoms to decrease to 10.% of

their initial concentration? A) 1.1 s B) 0.041 s C) 0.27 s D) 0.89 s E) 2.7 s

101. Determine the molecularity of the following elementary reaction: O3 O2 + O. A) unimolecular B) bimolecular C) termolecular D) quadmolecular E) molecularity cannot be determined

102. The decomposition of ozone may occur through the two-step mechanism shown:step 1 O3 Æ O2 + Ostep 2 O3 + O Æ 2O2

The oxygen atom is considered to be a(n) A) reactant B) product C) catalyst D) reaction intermediate E) activated complex

103. The rate law for a reaction is found to be Rate = k[A]2[B]. Which of the following mechanisms gives this rate law?

I. A + B E (fast)E + B Æ C + D (slow)

II. A + B E (fast)E + A Æ C + D (slow)

III. A + A Æ E (slow).E + B Æ C + D (fast)

A) I B) II C) III D) two of these E) none of these

104. The experimental rate law for the decomposition of nitrous oxide (N2O) to N2 and O2 is Rate = k[N2O]2. Two mechanisms are proposed:

I. N2O Æ N2 + ON2O + O Æ N2 + O2

II. 2N2O N4O2

N4O2 Æ 2N2 + O2

Which of the following could be a correct mechanism? A) Mechanism I, with the first step as the rate-determining step. B) Mechanism I, with the second step as the rate-determining step as long as the first

step is a fast equilibrium step. C) Mechanism II, with the second step as the rate-determining step if the first step is a

fast equilibrium step. D) None of the choices (A-C) could be correct. E) At least two of the above choices (A-C) could be correct.

105. Consider the reaction 2O3(g) 3O2(g). The following mechanism is proposed: O3 O2 + O

O3 + O 2O2If we assume the second step of the mechanism is the rate determining step and the first step is a fast equilibrium step, which of the following rate laws is predicted by this mechanism?

A) rate = k[O3] B) rate = k[O3]2[O2] C) rate = k[O3]2[O2]–1 D) rate = k[O3]2 E) none of these

106. Of what use is it to find a rate law for a reaction? A) We can use the rate law to directly determine coefficients in the balanced equation. B) From the rate law we can evaluate potential reaction mechanisms. C) The rate law gives us a good indication of the thermodynamic stability of the

products. D) The rate law can lead us to determine the equilibrium constant for the reaction. E) None of these.


The following questions refer to the reaction 2A2 + B2 2C. The following mechanism has been proposed:

step 1 (very slow) A2 + B2 R + Cstep 2 (slow) A2 + R C

107. What is the molecularity of step 2?

A) unimolecular B) bimolecular C) termolecular D) quadmolecular E) molecularity cannot be determined

108. Which step is rate determining? A) both steps B) step 1 C) step 2 D) a step that is intermediate to step 1 and step 2 E) none of these

109. According to collision theory, the activated complex that forms in step 1 could have which of the following structures? (The dotted lines represent partial bonds.)

A)

B)

C)

D)

E)

110. According to the proposed mechanism, what should the overall rate law be? A) rate = k[A2]2 B) rate = k[A2] C) rate = k[A2][B2] D) rate = k[A2][R] E) rate = k[R]2


Under certain conditions the reaction H2O2 + 3I– + 2H+ I3– + 2H2O occurs by the following series of steps:

k1

Step 1. H2O2 + H+ H3O2+

k–1

Step 2. H3O2+ + I– H2O + HOI (slow, rate constant k2)

Step 3. HOI + I– OH– + I2 (fast, rate constant k3)Step 4. OH– + H+ H2O (fast, rate constant k4)

Step 5. I2 + I– I3– (fast, rate constant k5)

111. Which of the steps would be called the rate-determining step? A) 1 B) 2 C) 3 D) 4 E) 5

112. The rate constant k for the reaction would be given by A) k = k2 B) k = k2k3 C) k = k2K D) k = k5 E) k = Kk2k3k4k5

113. The rate law for the reaction would be: A) [I3]/t = k[H2O2] B) [I3]/t = k[H2O2][H+][I–] C) [I3]/t = k[H2O2][H+] D) [I3]/t = k[H2O2][I–] E) [I3]/t = k[H2O2][H+]2[I–]–3

114. The reaction:2A + B Æ C

has the following proposed mechanism:Step 1: A + B D (fast equilibrium)Step 2: D + B Æ EStep 3: E + A Æ C + B

If step 2 is the rate-determining step, then the rate of formation of C should equal: A) k[A] B) k[A]2[B] C) k[A]2[B]2 D) k[A][B] E) k[A][B]2

115. The reaction 2NO + O2 2NO2 obeys the rate law – = kobsd[NO]2[O2].Which of the following mechanisms is consistent with the experimental rate law?

A) NO + NO Æ N2O2 (slow)N2O2 + O2 Æ 2NO2 (fast)

B) NO + O2 NO3 (fast equilibrium)NO3 + NO Æ 2NO2 (slow)

C) 2NO N2O2 (fast equilibrium)N2O2 Æ NO2 + O (slow)NO + O Æ NO2 (fast)

D) O2 + O2 O2 + O2 (slow)O2 + NO NO2 + O (fast)O + NO NO2 (fast)

E) none of these

116. The rate constant k is dependent onI. the concentration of the reactantII. the nature of the reactantsIII. the temperatureIV. the order of the reaction

A) none of these B) one of these C) two of these D) three of these E) all of these


The questions below refer to the following diagram:

117. Why is this reaction considered to be exothermic? A) Because energy difference B is greater than energy difference C. B) Because energy difference B is greater than energy difference A. C) Because energy difference A is greater than energy difference C. D) Because energy difference B is greater than energy difference C plus energy

difference A. E) Because energy difference A and energy difference C are about equal.

118. At what point on the graph is the activated complex present? A) point W B) point X C) point Y D) point Z E) none of these

119. If the reaction were reversible, would the forward or the reverse reaction have a higher activation energy?

A) The diagram shows no indication of any activation energy. B) The forward and reverse activation energies are equal. C) The forward activation energy would be greater. D) The reverse activation energy would be greater. E) None of these.

120. What would happen if the kinetic energy of the reactants was not enough to provide the needed activation energy?

A) The products would be produced at a lower energy state. B) The rate of the reaction would tend to increase. C) The activated complex would convert into products. D) The reactants would continue to exist in their present form. E) The products would form at an unstable energy state.

121. The rate constant for a reaction at 40.0°C is exactly 5 times that at 20.0°C. Calculate the Arrhenius energy of activation for the reaction.

A) 13.4 kJ/mol B) 7.38 kJ/mol C) 61.4 kJ/mol D) 5.00 kJ/mol E) none of these


Use the potential energy diagram shown to answer the following:

122. Which letter shows the activation energy (without use of a catalyst)? A) a B) b C) c

D) d E) e

123. Which letter shows the change in energy for the overall reaction? A) a B) b C) c D) d E) e

124. Which letter shows the activation energy using a catalyst? A) a B) b C) c D) d E) e


The questions below refer to the following information: The rate constant k for the reaction shown below is 2.6 10–8 L/mol s when the reaction proceeds at 300.0 K. The activation energy is 98000 J/mol. (The universal gas constant, R, is 8.314 J/mol·K)

2NOCl Æ 2NO + Cl2

125. Determine the magnitude of the frequency factor for the reaction. A) 1.2 108 B) 4.6 109 C) 3.0 109 D) 2.7 108 E) 9.1 109

126. If the temperature changed to 310 K, the rate constant k would change. The ratio of k at 310 K to k at 300.0 K is closest to what whole number?

A) 1 B) 2 C) 3 D) 4 E) 5

127. Use the following information to determine the activation energy for the reaction shown here:2NO N2 + O2

Temperature(K)

Rate Constant(L/mol·s)1400 0.1431500 0.703

A) 6.2 104 J/mol B) 1.3 101 J/mol C) 9.6 103 J/mol D) 3.3 104 J/mol E) 2.8 105 J/mol

128. When ethyl chloride, CH3CH2Cl, is dissolved in 1.0 M NaOH, it is converted into ethanol, CH3CH2OH, by the reaction:CH3CH2Cl + OH– CH3CH2OH + Cl–

At 25°C the reaction is first order in CH3CH2Cl, and the rate constant is 4.7 10–3 s–1. If the activation parameters are A = 3.4 1014 s–1 and Ea = 100.0 kJ/mol, what will the rate constant be at 40.°C?

A) 3.3 10–2 s–1 B) 6.8 10–4 s–1 C) 1.5 103 s–1 D) 9.1 10–3 s–1 E) 2.4 10–3 s–1

129. Which of the following statements best describes the condition(s) needed for a successful formation of a product according to the collision model?

A) The collision must involve a sufficient amount of energy, provided from the motion of the particles, to overcome the activation energy.

B) The relative orientation of the particles has little or no effect on the formation of the product.

C) The relative orientation of the particles has an effect only if the kinetic energy of the particles is below some minimum value.

D) The relative orientation of the particles must allow for formation of the new bonds in the product.

E) The energy of the incoming particles must be above a certain minimum value, and the relative orientation of the particles must allow for formation of new bonds in the product.

130. The rate constant for a reaction is 1.7 10–2 s–1 at 662 K and 5.0 10–2 s–1 at 848 K. What is the activation energy?

A) 12 kJ/mol B) 27 kJ/mol C) 640 kJ/mol D) 3300 kJ/mol E) This can't be solved without knowing the frequency factor.

131. For the second-order reaction NO(g) + O3(g) ? NO2(g) + O2(g), the rate constant has been measured to be 1.08 * 107 M–1 s–1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K. What is the rate constant at 281 K? (R = 8.3145 J K–1 mol–1)

A) 1.08 * 107 M–1 s–1 B) 1.08 * 109 M–1 s–1 C) 8.18 * 106 M–1 s–1 D) 1.43 * 107 M–1 s–1 E) 9.51 * 105 M–1 s–1

132. The reaction 2H2O2 2H2O + O2 has the following mechanism:H2O2 + I– Æ H2O + IO–

H2O2 + IO– Æ H2O + O2 + I–

The catalyst in the reaction is: A) H2O B) I– C) H2O2 D) IO– E) There is no catalyst in this reaction.

133. Which of the following statements is typically true for a catalyst?I. The concentration of the catalyst will go down as a reaction proceeds.II. The catalyst provides a new pathway in the reaction mechanism.III. The catalyst speeds up the reaction.

A) I only B) II only C) III only D) I and III E) II and III

134. The catalyzed pathway in a reaction mechanism has a __________ activation energy and thus causes a __________ reaction rate.

A) higher, lower

B) higher, higher C) lower, higher D) lower, steady E) higher, steady

135. Which of the following statements about enzymes is incorrect? A) They are proteins that catalyze specific biologic reactions. B) Several hundred are now known. C) The molecules they react with are called substrates. D) They are equal to inorganic catalysts in efficiency. E) All of these are correct.

136. Determine (a) the rate equation and (b) the rate constant for the hypothetical reaction A + B C given the following initial concentrations and initial rate data.

[A]0 [B]0 Initial RateRun # (mol/L) (mol/L) (mol/L·s)(1) 0.100 0.100 0.18(2) 0.100 0.200 0.36(3) 0.200 0.200 1.44


A reaction represented by the equation was studied at a specific temperature and the following data were collected:

3O2 (g) Æ 2O3 (g)

Time (seconds) Total pressure (atm) 0 1.000 46.89 0.9500 98.82 0.9033 137.9 0.8733 200.0 0.8333 286.9 0.7900 337.9 0.7700 511.3 0.7233

137. What is the rate law for this reaction?

138. What is the value of the rate constant?

139. How many seconds would it take for the total pressure to be 0.7133 atm?


For the reaction aA Products, use the following choicesa) zero order in Ab) first order in Ac) second order in Ad) a, b, ce) none of the above

140. The half-life is constant.

141. A plot of [A] vs. t is a straight line.

142. [A] is constant.

143. The rate is constant over time.

144. Which of the following is true about a system at equilibrium? A) The concentration(s) of the reactant(s) is equal to the concentration(s) of the

product(s). B) No new product molecules are formed. C) The concentration(s) of reactant(s) is constant over time. D) The rate of the reverse reaction is equal to the rate of the forward reaction and both

rates are equal to zero. E) None of the above (A-D) is true.

145. Which of the following is true about chemical equilibrium? A) It is microscopically and macroscopically static. B) It is microscopically and macroscopically dynamic. C) It is microscopically static and macroscopically dynamic. D) It is microscopically dynamic and macroscopically static. E) None of these are true about chemical equilibrium.

146. Equilibrium is reached in chemical reactions when:

A) The rates of the forward and reverse reactions become equal. B) The concentrations of reactants and products become equal. C) The temperature shows a sharp rise. D) All chemical reactions stop. E) The forward reaction stops.

147. For a particular system at a particular temperature there ______ equilibrium constant(s) and there _______ equilibrium position(s).

A) are infinite; is one B) is one; are infinite C) is one; is one D) are infinite; are infinite E) none of these

148. For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container.

At equilibrium, the concentration of A is 0.231 mol/L. What is the concentration of B at equilibrium?

A) 0.231 mol/L B) 0.295 mol/L C) 0.500 mol/L D) 0.462 mol/L E) none of these

149. The value of the equilibrium constant, K, is dependent on:I. the temperature of the systemII. the nature of the reactants and productsIII. the concentration of the reactantsIV. the concentration of the products

A) I, II B) II, III C) III, IV D) It is dependent on three of the above choices. E) It is not dependent on any of the above choices.

150. If the equilibrium constant for A + B C is 0.213, then the equilibrium constant for 2C 2A + 2B is

A) 0.574 B) 4.69 C) 0.426 D) 22.0

E) 0.213

151. Indicate the mass action expression for the following reaction: 2X(g) + Y(g) 3W(g) + V(g)

A) [X]2[Y][W]3[V] B) C) D) E) none of these

152. If, at a given temperature, the equilibrium constant for the reaction H2(g) + Cl2(g) 2HCl(g) is Kp, then the equilibrium constant for the reaction HCl(g) H2(g) + Cl2 (g) can be represented as:

A) B) Kp2 C) D) E) none of these

153. Apply the law of mass action to determine the equilibrium expression for 2NO2Cl(aq) 2NO2(aq) + Cl2(aq).

A) K = 2[NO2][Cl2]/2[NO2Cl] B) K = 2[NO2Cl]/2[NO2][Cl2] C) K = [NO2Cl]2/[NO2]2[Cl2] D) K = [NO2]2[Cl2]/[NO2Cl]2 E) K = [NO2Cl]2[NO2]2[Cl2]

154. At a given temperature, K = 0.030 for the equilibrium:PCl5(g) PCl3(g) + Cl2(g)What is K for:Cl2(g) + PCl3(g) PCl5(g)?

A) 0.030 B) 33 C) 0.00090 D) 30. E) 1100

155. Given the equilibrium constants for the following reactions:4Cu(s) + O2(g) 2Cu2O(s), K12CuO(s) Cu2O(s) + ?O2(g), K2what is K for the system

2Cu(s) + O2(g) 2CuO(s)equivalent to?

A) (K1)(K2) B) (K2)?/(K1) C) (K1)?/(K2) D) (K2)?/(K1) E) (K1)(K2)?

156. Which expression correctly describes the equilibrium constant for the following reaction?2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)

A) K = ( 2[C2H2] + 5[O2] ) / ( 4[CO2] + 2[H2O] ) B) K = ( 4[CO2] + 2[H2O] ) / (2[C2H2] + 5[O2] ) C) K = ( [CO2][H2O] ) / ( [C2H2][O2] ) D) K = ( [CO2]4[H2O]2 ) / ( [C2H2]2[O2]5 ) E) K = ( [C2H2]2[O2]5 ) / ( [CO2]4[H2O]2 )


Consider the chemical system CO + Cl2 COCl2; K = 4.6 109 L/mol.

157. How do the equilibrium concentrations of the reactants compare to the equilibrium concentration of the product?

A) They are much smaller. B) They are much bigger. C) They are about the same. D) They have to be exactly equal. E) You can't tell from the information given.

158. If the concentration of the product were to double, what would happen to the equilibrium constant?

A) It would double its value. B) It would become half its current value. C) It would quadruple its value. D) It would not change its value. E) It would depend on the initial conditions of the product.

159. Determine the equilibrium constant for the system N2O4 2NO2 at 25°C. The concentrations are shown here: [N2O4] = 2.93 10–2 M, [NO2] = 1.41 10–2 M.

A) 0.481

B) 2.08 C) 1.47 102 D) 0.232 E) 6.79 10–3

160. If K = 0.138 for A2 + 2B 2AB, then for 4AB 2A2 + 4B, K would equal: A) 0.276 B) 0.138 C) –0.138 D) 3.62 E) 52.5

161. Consider the gaseous reaction CO(g) + Cl2(g) COCl2(g). What is the expression for Kp in terms of K?

A) K(RT) B) K/(RT) C) K(RT)2 D) K/(RT)2 E) 1/K(RT)

162. For the reaction N2O4(g) 2NO2(g), Kp = 0.148 at a temperature of 298 K. What is Kp for the following reaction?4NO2(g) 2N2O4(g)

A) 6.76 B) 0.296 C) 3.38 D) 4.57 * 101 E) 2.19 * 10–2

163. For the reaction H2(g) + Cl2(g) 2HCl(g), Kc = 3.36 * 1023 at a temperature of 429 K. What is Kp at this temperature?

A) 3.36 * 1023 B) 1.18 * 1025 C) 9.55 * 1021 D) 4.17 * 1026 E) 2.71 * 1020

164. For the reaction NO(g) + ?O2(g) NO2(g) at 750°C, the equilibrium constant Kc equals:

A) 1.0 B) Kp

C) Kp(RT)–? D) Kp(RT)? E) Kp(RT)?

165. An equilibrium reaction, A2(g) + 3B2(g) 2C(g), has a Kp at 225ºC of 1.5 10–3 /atm2. What is K for this reaction at that temperature?

A) 9.0 10–7 B) 4.4 10–6 C) 2.5 D) 3.7 10–5 E) 0.51

166. Find the value of the equilibrium constant (K) (at 500 K) for N2(g) + 3H2(g) 2NH3(g). The value for Kp at 500 K is 1.5 10–5/atm2.

A) 7.5 10–2 B) 1.3 10–2 C) 9.6 10–2 D) 2.5 10–2 E) 6.0 10–2

167. Consider the following reaction: CS2(g) + 4H2(g) CH4(g) + 2H2S(g). The equilibrium constant K is about 0.26 at 900.°C. What is Kp at this temperature?

A) 2.4 103 B) 2.8 10–5 C) 2.8 10–5 D) 2.5 101 E) 1.1 10–3

168. Given the equation 2NOCl2(g) 2NO(g) + Cl2(g), the equilibrium constant is about 0.0290 at 115°C. Calculate Kp.

A) 0.0290 B) 0.923 C) 0.274 D) 29.4 E) none of these

169. Calculate Kp for using the following data:Kp = 2.4 106Kp = 1.8 1037

A) 4.3 1043 B) 2.2 1043

C) 3.2 10–25 D) 5.7 10–13 E) 1.0 10–12

170. Consider the reaction: CaCl2(s) + 2H2O(g) CaCl2·2H2O(s)

The equilibrium constant for the reaction as written is: A) K = B) C) D) K = [H2O]2 E) K =

171. Consider the reaction At 1273 K, the Kp value is 167.5. What is the at equilibrium if the is 0.25 atm at this temperature?

A) 3.2 atm B) 0.13 atm C) 13 atm D) 6.5 atm E) 9.2 atm


Consider the following equilibrium: H2(g) + I2(s) 2HI(g)

172. The proper Keq expression is: A) B) C) D) E)

173. Which of the following statements about the equilibrium is false? A) If the system is heated, the right side is favored. B) This is a heterogeneous equilibrium. C) If the pressure on the system is increased by changing the volume, the left side is

favored. D) Adding more H2(g) increases the equilibrium constant. E) Removing HI as it forms forces the equilibrium to the right.

174. Consider the reaction: 2SO2(g) + O2(g) 2SO3(g) at constant temperature. Initially a container is filled with pure SO3(g) at a pressure of 2 atm, after which equilibrium is reached. If y is the partial pressure of O2 at equilibrium, the value of Kp is:

A) B) C) D) E) none of these

175. Which of the following is true for a system whose equilibrium constant is relatively small?

A) It will take a short time to reach equilibrium. B) It will take a long time to reach equilibrium. C) The equilibrium lies to the left. D) The equilibrium lies to the right. E) Two of these.

176. The reaction quotient for a system is 7.2 102. If the equilibrium constant for the system is 36, what will happen as equilibrium is approached?

A) There will be a net gain in product. B) There will be a net gain in reactant. C) There will be a net gain in both product and reactant. D) There will be no net gain in either product or reactant. E) The equilibrium constant will decrease until it equals the reaction quotient.

177. Consider the following reaction:2HF(g) H2(g) + F2(g) (K = 1.00 10–2)

Given 1.00 mole of HF(g), 0.316 mole of H2(g), and 0.750 mole of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q.

A) Q = 0.0474 B) Q = 0.237 C) Q = 0.0593 D) Q = 2.07 E) none of these


Nitric oxide, an important pollutant in air, is formed from the elements nitrogen and oxygen at high temperatures, such as those obtained when gasoline burns in an automobile engine. At 2000°C, K for the reaction N2(g) + O2(g) 2NO(g) is 0.01.

178. Predict the direction in which the system will move to reach equilibrium at 2000°C if 0.4 moles of N2, 0.1 moles of O2, and 0.08 moles of NO are placed in a 1.0-liter container.

A) The system remains unchanged. B) The concentration of NO will decrease; the concentrations of N2 and O2 will

increase. C) The concentration of NO will increase; the concentrations of N2 and O2 will

decrease. D) The concentration of NO will decrease; the concentrations of N2 and O2 will remain

unchanged. E) More information is necessary.

179. A 1-L container originally holds 0.4 mol of N2, 0.1 mol of O2, and 0.08 mole of NO. If the volume of the container holding the equilibrium mixture of N2, O2, and NO is decreased to 0.5 L without changing the quantities of the gases present, how will their concentrations change?

A) The concentration of NO will increase; the concentrations of N2 and O2 will decrease.

B) The concentrations of N2 and O2 will increase; and the concentration of NO will decrease.

C) The concentrations of N2, O2, and NO will increase. D) The concentrations of N2, O2, and NO will decrease. E) There will be no change in the concentrations of N2, O2, and NO.

180. Consider the following equilibrated system: 2NO2(g) 2NO(g) + O2(g). If the Kp value is 0.884, find the equilibrium pressure of the O2 gas if the NO2 gas pressure is 0.520 atm and the PNO is 0.300 atm at equilibrium.

A) 1.53 atm B) 36.3 atm C) 0.510 atm D) 0.294 atm E) 2.66 atm

181. For the reaction given below, 2.00 moles of A and 3.00 moles of B are placed in a 6.00-L container.A(g) + 2B(g) C(g)

At equilibrium, the concentration of A is 0.235 mol/L. What is the value of K? A) 1.38 B) 1.07 C) 0.235 D) 4.55 E) 0.418

182. A 10.0-g sample of solid NH4Cl is heated in a 5.00-L container to 900.°C. At equilibrium the pressure of NH3(g) is 1.14 atm.NH4Cl(s) NH3(g) + HCl(g)

The equilibrium constant, Kp, for the reaction is: A) 1.14 B) 1.30 C) 2.28 D) 4.68 E) none of these

183. Consider the reaction H2 + I2 2HI for which K = 42.1 at a high temperature. If an equimolar mixture of reactants gives the concentration of the product to be 0.50 M at equilibrium, determine the equilibrium concentration of the hydrogen.

A) 1.1 10–1 M B) 7.7 10–2 M C) 3.9 10–2 M D) 1.3 101 M E) 5.9 10–3 M

184. Consider the equation A(aq) + 2B(aq) 3C(aq) + 2D(aq). In one experiment, 45.0 mL of 0.050 M A is mixed with 25.0 mL 0.100 M B. At equilibrium the concentration of C is 0.0410 M. Calculate K.


185. The reaction:H2(g) + I2(g) 2HI(g)

has Kp = 45.9 at 763 K. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 4.00 atm and hydrogen gas at a partial pressure of 0.215 atm. What is the partial pressure of I2?

A) 0.215 atm B) 0.405 atm C) 1.62 atm D) 10.9 atm E) 74.4 atm

186. For the equilibrium system:

CO2(g) + H2(g) CO(g) + H2O(g) H = +42 kJ/molK equals 1.6 at 1260 K. If 0.15 mol each of CO2, H2, CO, and H2O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then as the system came to equilibrium:

A) The temperature would decrease and the mass of CO2 would increase. B) The temperature would decrease and the mass of CO2 would decrease. C) The temperature would remain constant and the mass of CO2 would increase. D) The temperature would increase and the mass of CO2 would increase. E) The temperature would increase and the mass of CO2 would decrease.

187. CS2(g) + 3Cl2(g) CCl4(g) + S2Cl2(g)At a given temperature, the reaction above is at equilibrium when [CS2] = 0.050 M, [Cl2] = 0.25 M, [CCl4] = 0.15 M, and [S2Cl2] = 0.35 M. What would be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.14 M, Cl2 = 0.22 M, CCl4 = 0.28 M, and S2Cl2 = 0.37 M?

A) to the right B) to the left C) no change D) cannot predict unless we know the temperature E) cannot predict unless we know whether the reaction is endothermic or exothermic

188. A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature.3H2 + N2 2NH3An analysis of the mixture at equilibrium revealed 1.8 mol N2, 3.0 mol H2, and 1.8 mol NH3. How many moles of H2 were present at the beginning of the reaction?

A) 3.0 B) 4.5 C) 4.8 D) 5.7 E) 4.2

189. Carbon disulfide and chlorine react according to the following equation:CS2(g) + 3Cl2(g) S2Cl2(g) + CCl4(g)When 2.60 mol of CS2 and 4.25 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.400 mol of CCl4. How many moles of Cl2 are present at equilibrium?

A) 2.200 mol B) 0.400 mol C) 3.05 mol D) 3.45 mol E) 1.52 mol

190. Initially 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the following reaction then occurred:3H2(g) + N2(g) 2NH3(g)

The equilibrium concentration of NH3(g) = 0.62 moles/liter at 700.°C. The value for K at 700.°C for the formation of ammonia is:



Consider the following reaction (assume an ideal gas mixture): 2NOBr(g) 2NO(g) + Br2(g) A 1.0-liter vessel was initially filled with pure NOBr, at a pressure of 4.0 atm, at 300 K.

191. After equilibrium was established, the partial pressure of NOBr was 3.1 atm. What is Kp for the reaction?


192. After equilibrium was reached, the volume was increased to 2.0 liters, while the temperature was kept at 300 K. The result of this change was

A) an increase in Kp B) a decrease in Kp C) a shift in the equilibrium position to the right D) a shift in the equilibrium position to the left E) none of these

193. Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.0 atm of nitrogen gas is mixed with 2.0 atm of hydrogen gas. At equilibrium, the total pressure is 2.1 atm. Calculate the partial pressure of hydrogen gas at equilibrium.

A) 2.1 atm B) 0.65 atm C) 1.5 atm D) 0.0 atm

E) none of these

194. The following reaction is investigated (assume an ideal gas mixture):2N2O(g) + N2H4(g) 3N2(g) + 2H2O(g)

Initially there are 0.10 moles of N2O and 0.25 moles of N2H4, in a 10.0-L container. If there are 0.064 moles of N2O at equilibrium, how many moles of N2 are present at equilibrium?


195. A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B. Gas A decomposes according to the following reaction:3A 2B + C

The equilibrium concentration of gas C is 0.116 mol/L. Determine the equilibrium concentration of gas A.

A) 0.116 M B) 0.652 M C) 0.732 M D) 0.884 M E) 0.348 M


The equilibrium concentration of gas C is 0.120 mol/L. Determine the equilibrium concentration of gas B.

A) 0.120 M B) 0.620 M C) 0.740 M D) 0.260 M E) 0.240 M


The equilibrium concentration of gas C is 0.147 mol/L. Determine the value of the equilibrium constant, K.

A) 0.209 B) 0.166

C) 3.89 10–3 D) 0.531 E) none of these

198. A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation:NH4NO3(s) N2O(g) + 2H2O(g)

At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C. Calculate Kp.

A) 0.822 B) 1.64 C) 0.745 D) 2.98 E) 80.5


Given the equation 2A(g) 2B(g) + C(g). At a particular temperature, K = 1.6 104.

199. If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed?

A) To the left. B) To the right. C) The above mixture is the equilibrium mixture. D) Cannot tell from the information given. E) None of these (A-D).

200. Addition of chemical B to an equilibrium mixture of the above will A) cause [A] to increase B) cause [C] to increase C) have no effect D) cannot be determined E) none of the above

201. At a higher temperature, K = 1.8 10–5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will

A) cause [A] to increase B) cause [B] to increase C) have no effect D) cannot be determined E) none of the above

202. Raising the pressure by lowering the volume of the container will A) cause [A] to increase B) cause [B] to increase C) have no effect D) cannot be determined E) none of the above


Consider the following equilibrium: 2NOCl(g) 2NO(g) + Cl2(g) with K = 1.6 10–5. In an experiment, 1.00 mole of pure NOCl and 1.00 mole of pure Cl2 are placed in a 1.00-L container.

203. If x moles of NOCl react, what is the equilibrium concentration of NO? A) x B) 2x C) –x D) –2x E) x2

204. If x moles of NOCl react, what is the equilibrium concentration of Cl2? A) x B) ? x C) 1 + x D) 1 + ? x E) 1 + 2x

205. At a certain temperature K for the reaction 2NO2 N2O4 is 7.5 liters/mole. If 2.0 moles of NO2 are placed in a 2.0-liter container and permitted to react at this temperature, calculate the concentration of N2O4 at equilibrium.

A) 0.39 moles/liter B) 0.65 moles/liter C) 0.82 moles/liter D) 7.5 moles/liter E) none of these

206. Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and is allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g)If at equilibrium the N2O4 is 29% dissociated, what is the value of the equilibrium

constant, Kc, for the reaction under these conditions? A) 0.82 B) 0.47 C) 2.1 D) 0.34 E) 0.12

207. At 500.0 K, one mole of gaseous ONCl is placed in a one-liter container. At equilibrium it is 5.0% dissociated according to the equation shown here: 2ONCl 2NO + Cl2. Determine the equilibrium constant.

A) 6.9 10–5 B) 1.4 10–3 C) 5.3 10–2 D) 9.5 10–1 E) 1.4 104

208. Consider the following equilibrium:2NOCl(g) 2NO(g) + Cl2(g)

with K = 1.6 10–5. 1.00 mole of pure NOCl and 0.920 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of NO(g).

A) 2.09 10–3 M B) 9.20 10–1 M C) 1.09 M D) 5.90 10–3 M E) 4.17 10–3 M

209. Consider the following equilibrium:2NOCl(g) 2NO(g) + Cl2(g)

with K = 1.6 10–5. 1.00 mole of pure NOCl and 0.985 mole of pure Cl2 are placed in a 1.00-L container. Calculate the equilibrium concentration of Cl2(g).

A) 1.6 10–5 M B) 0.987 M C) 0.494 M D) 2.02 10–3 M E) 4.03 10–3 M

210. For the reaction below, Kp = 1.16 at 800.°C.CaCO3(s) CaO(s) + CO2(g)

If a 38.9-gram sample of CaCO3 is put into a 10.0-L container and heated to 800.°C, what percent of the CaCO3 will react to reach equilibrium?

A) 17.5% B) 33.9%

C) 45.5% D) 100.0% E) none of these

211. At –80°C, K for the reactionN2O4(g) 2NO2(g)

is 4.66 10–8. We introduce 0.042 mole of N2O4 into a 1.0-L vessel at –80°C and let equilibrium be established. The total pressure in the system at equilibrium will be:

A) 0.28 atm B) 0.67 atm C) 1.2 atm D) 0.042 atm E) none of these

212. The equilibrium system 2A 2B + C has a very small equilibrium constant: K = 2.6 10–6. Initially 3.0 moles of A are placed in a 1.5-L flask. Determine the concentration of C at equilibrium.

A) 0.011 M B) 0.024 M C) 0.032 M D) 0.048 M E) 2.0 M

213. Which of the following statements concerning equilibrium is not true? A) A system that is disturbed from an equilibrium condition responds in a manner to

restore equilibrium. B) Equilibrium in molecular systems is dynamic, with two opposing processes balancing

one another. C) The value of the equilibrium constant for a given reaction mixture is the same

regardless of the direction from which equilibrium is attained. D) A system moves spontaneously toward a state of equilibrium. E) The equilibrium constant is independent of temperature.


The questions below refer to the following system: Co(H2O)6

2+ + 4 Cl– CoCl42– + 6H2O

(pink) (blue)When cobalt(II) chloride is added to pure water, the Co2+ ions hydrate. The hydrated form then reacts with the Cl– ions to set up the equilibrium shown here.

214. Which statement below describes the change that the system will undergo if hydrochloric acid is added?

A) It should become more blue. B) It should become more pink. C) The equilibrium will shift to the right. D) The equilibrium will shift to the left. E) Two of these.

215. Which statement below describes the change that the system will undergo if water is added?

A) More chloride ions will be produced. B) More water will be produced. C) The equilibrium will shift to the right. D) The color will become more blue. E) There will be less of the hydrated cobalt ion at the new equilibrium position.

216. Which statement below describes the change that the system will undergo if silver nitrate is added?

A) It should become more blue. B) It should become more pink. C) Water will be produced. D) The silver ion will react with the CoCl42–. E) Nothing will change.


The following questions refer to the equilibrium shown here: 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)

217. What would happen to the system if oxygen were added? A) More ammonia would be produced. B) More oxygen would be produced. C) The equilibrium would shift to the right. D) The equilibrium would shift to the left. E) Nothing would happen.

218. What would happen to the system if the pressure were decreased? A) Nothing would happen. B) More oxygen would be produced.

C) The water vapor would become liquid water. D) The ammonia concentration would increase. E) The NO concentration would increase.

219. For a certain reaction at 25.0°C, the value of K is 1.2 10–3. At 50.0°C the value of K is 3.4 10–1. This means that the reaction is

A) exothermic B) endothermic C) never favorable D) more information needed E) none of these (A-D)

220. Ammonia is prepared industrially by the reaction: N2(g) + 3H2(g) 2NH3(g) for the reaction: H° = –92.2 kJ and K (at 25°C) = 4.0 108. When the temperature of the reaction is increased to 500°C, which of the following is true?

A) K for the reaction will be larger at 500°C than at 25°C. B) At equilibrium, more NH3 is present at 500°C than at 25°C. C) Product formation (at equilibrium) is not favored as the temperature is raised. D) The reaction of N2 with H2 to form ammonia is endothermic. E) None of the above is true.


Consider the following equilibrium: 2H2(g) + X2(g) 2H2X(g) + energy

221. Addition of X2 to a system described by the above equilibrium A) will cause [H2] to decrease B) will cause [X2] to decrease C) will cause [H2X] to decrease D) will have no effect E) cannot possibly be carried out

222. Addition of argon to the above equilibrium A) will cause [H2] to decrease B) will cause [X2] to increase C) will cause [H2X] to increase D) will have no effect E) cannot possibly be carried out

223. Increasing the pressure by decreasing the volume will cause

A) the reaction to occur to produce H2X B) the reaction to occur to produce H2 and X2 C) the reaction to occur to produce H2 but no more X2 D) no reaction to occur E) X2 to dissociate

224. Increasing the temperature will cause A) the reaction to occur to produce H2X B) the reaction to occur to produce H2 and X2 C) the reaction to occur to produce H2 but no more X2 D) no reaction to occur E) an explosion

225. Which of the following statements is true? A) When two opposing processes are proceeding at identical rates, the system is at

equilibrium. B) Catalysts are an effective means of changing the position of an equilibrium. C) The concentration of the products equals that of reactants and is constant at

equilibrium. D) An endothermic reaction shifts toward reactants when heat is added to the reaction. E) None of the above statements is true.

226. Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g) + 92.94 kJ Which of the following changes will shift the equilibrium to the right?I. increasing the temperatureII. decreasing the temperatureIII. increasing the volumeIV. decreasing the volumeV. removing some NH3

VI. adding some NH3

VII. removing some N2

VIII. adding some N2

A) I, IV, VI, VII B) II, III, V, VIII C) I, VI, VIII D) I, III, V, VII E) II, IV, V, VIII

227. Consider the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K:

A) increases, because by adding A more products are made, increasing the product to

reactant ratio B) decreases, because A is a reactant so the product to reactant ratio decreases C) does not change, because A does not figure into the product to reactant ratio D) does not change, as long as the temperature is constant E) depends on whether the reaction is endothermic or exothermic

228. Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is raised?

A) The equilibrium position is shifted to the right and the value for K increases. B) The equilibrium position is shifted to the right and the value for K decreases. C) The equilibrium position is shifted to the left and the value for K decreases. D) The equilibrium position is shifted to the left and the value for K increases. E) The equilibrium position is shifted but the value for K stays constant.

229. Consider the reaction represented by the equation 2SO2(g) + O2(g) 2SO3(g). For the system at chemical equilibrium, which of the following explains what happens after the addition of oxygen gas (assume constant temperature)?

A) The amount of SO3(g) increases and the value for K increases. B) The amount of SO3(g) decreases and the value for K increases. C) The amount of SO3(g) stays the same and the value for K decreases. D) The amount of SO3(g) decreases and the value for K stays the same. E) The amount of SO3(g) increases and the value for K stays the same.

230. Consider the reaction represented by the equation: N2(g) + 3H2(g) 2NH3(g). What happens to the equilibrium position when an inert gas is added to this system (as represented above) at equilibrium?

A) If the container is rigid, nothing happens to the equilibrium position. If the container is fitted with a moveable piston, the equilibrium position shifts.

B) If the container is rigid, the equilibrium position shifts. If the container is fitted with a moveable piston, nothing happens to the equilibrium position.

C) The equilibrium position shifts no matter what the container is like. D) Nothing happens to the equilibrium position no matter what the container is like. E) The value of the equilibrium constant must be known to answer this question.

chemistryhelprush.wikispaces.comchemistryhelprush.wikispaces.com/file/view/12+and+13+ap... · web...

Documents