Chemical Kinetics Test Bank Docx Chapter.13

Chemistry: Molecular Nature of Matter, 8e (Jespersen)

Chapter 13 Chemical Kinetics

1) Which of the following is a homogeneous reaction?

A) dissolving salt in water

B) neutralizing aqueous acid with solid sodium hydroxide

C) iron rusting

D) phosphorus igniting in air

E) titration of an unknown base with aqueous hydrochloric acid

Diff: 1

Section: 13.1

2) The fact that granulated sugar dissolves faster than a sugar cube of the same mass can best be explained by which of the following statements?

A) The ability of reacting or interacting molecules to come in contact with each other is greater for granulated sugar.

B) Dissolving the sugar increases the temperature of the solution.

C) Sugar cubes are coated to slow the dissolving process.

D) The concentration of granulated sugar is higher than that of a sugar cube.

E) None of the above

Diff: 1

Section: 13.1

3) Most heterogeneous reactions are slower than similar homogeneous reactions. Which of the following best explains why?

A) The temperature of the two phases is different.

B) Heterogeneous mixtures are not allowed to react, and therefore are heterogeneous.

C) Heterogeneous mixtures require the use of a catalyst.

D) The ability of reactants to come in contact with each other in heterogeneous mixtures is limited by the different phases.

E) The activation energy of heterogeneous reactions is always much higher.

Diff: 2

Section: 13.1

4) Nitrogen monoxide reacts with bromine at elevated temperatures, according to the equation:

2NO(g) + Br2(g) → 2NOBr(g)

In a certain reaction mixture, the rate of formation of NOBr(g) was 4.50 × 10-4 mol L-1 s-1. What was the rate of consumption of Br2(g)?

A) 4.50 × 10-4 mol L-1 s-1

B) 2.25 × 10-4 mol L-1 s-1

C) 9.00 × 10-4 mol L-1 s-1

D) 2.12 × 10-4 mol L-1 s-1

E) 2.03 × 10-3 mol L-1 s-1

Diff: 1

Section: 13.2

5) Nitrogen monoxide reacts with chlorine at high temperature, according to the equation:

2NO(g) + Cl2(g) → 2NOCl(g)

In a certain reaction mixture, the rate of formation of NOCl(g) was 4.50 × 10-4 mol L-1 s-1. What was the rate of consumption of NO(g)?

A) 4.50 × 10-4 mol L-1 s-1

B) 2.25 × 10-4 mol L-1 s-1

C) 9.00 × 10-4 mol L-1 s-1

D) 2.12 × 10-4 mol L-1 s-1

E) 2.03 × 10-3 mol L-1 s-1

Diff: 1

Section: 13.2

6) In a reaction described by the equation:

2CH4O(g) + 3O2(g) → 2CO2(g) + 4H2O(g),

the rate of consumption of O2(g) is 0.400 mol L-1 s-1. What is the rate of formation of H2O(g)?

A) 0.300 mol L-1 s-1

B) 0.400 mol L-1 s-1

C) 0.533 mol L-1 s-1

D) 0.800 mol L-1 s-1

E) 1.33 mol L-1 s-1

Diff: 1

Section: 13.2

7) In a reaction described by the equation:

2 CH4O(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g),

the rate of consumption of O2(g) is 0.400 mol L-1 s-1. What is the rate of consumption of CH4O(g)?

A) 0.200 mol L-1 s-1

B) 0.267 mol L-1 s-1

C) 0.333 mol L-1 s-1

D) 0.400 mol L-1 s-1

E) 0.600 mol L-1 s-1

Diff: 1

Section: 13.2

8) Cyclobutane, C4H8, decomposes as shown: C4H8(g) → 2 C2H4(g). In a study of this reaction, the rate of consumption of C4H8 at a certain point was 4.50 × 10-4 mol L-1 s-1. What is the rate at which C2H4(g) is being generated at this point?

A) 4.50 × 10-4 mol L-1 s-1

B) 2.25 × 10-4 mol L-1 s-1

C) 9.00 × 10-4 mol L-1 s-1

D) 2.12 × 10-4 mol L-1 s-1

E) 2.03 × 10-3 mol L-1 s-1

Diff: 1

Section: 13.2

9) A 10-mm cube of copper metal is placed in 250 mL of 12 M nitric acid at 25°C and the reaction below occurs:

Cu(s) + 4H+(aq) + 2NO3-(aq) → Cu2+(aq) + 2NO2(g) + 2H2O(l)

At a particular instant in time, nitrogen dioxide is being produced at the rate of . At this same instant, what is the rate at which hydrogen ions are being consumed?

A) 1.3 × 10-4 M/min

B) 5.2 × 10-4 M/min

C) 2.6 × 10-4 M/min

D) 1.0 × 10-3 M/min

E) 6.5 × 10-5 M/min

Diff: 1

Section: 13.2

10) The average reaction rate over a time period in graph b can be found by

A) taking the average of the rate every 100 s.

B) drawing a line tangent to the curve at the initial and final times, and then averaging.

C) drawing a line tangent to the curve at that point.

D) subtracting the final concentration from the initial concentration and dividing by the time interval.

E) subtracting the final time from the initial time and dividing by the concentration interval.

Diff: 1

Section: 13.2

11) The instantaneous rate at any point in graph b can be found by

A) taking the average of all rates found every 100 s.

B) drawing a line tangent to the curve at the initial and final times, and then averaging.

C) drawing a line tangent to the curve at that point.

D) subtracting the final concentration from the initial concentration and dividing by the time interval.

E) subtracting the final time from the initial time and dividing by the concentration.

Diff: 1

Section: 13.2

12) The rate of a chemical reaction in solution can be measured in the units

A) L2 mol-1 s-1.

B) mol L-1 s-1.

C) s-2.

D) mol s L-1.

E) sec L-1 mol-1.

Diff: 1

Section: 13.3

13) A reaction has the rate law, rate = k[A][B]2. Which change will cause the greatest increase in the reaction rate?

A) decreasing both concentrations by half

B) doubling the concentration of B

C) quadrupling the concentration of A

D) tripling the concentration of B

E) doubling the concentration of A

Diff: 1

Section: 13.3

14) A reaction has the rate law, rate = k[A]3[B]. Which change will cause the greatest increase in the reaction rate?

A) doubling the concentration of A and halving the concentration of B

B) quadrupling the concentration of B

C) tripling the concentration of A

D) doubling the concentration of A and tripling the concentration of B

E) tripling the concentration of B

Diff: 1

Section: 13.3

15) The reaction, 2NO(g) + O2(g) → 2NO2(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

A) rate = k[NO]2

B) rate = k[NO][O2]

C) rate = k[NO2]2[NO]2[O2]½

D) rate = k[NO]2[O2]2

E) rate = k([NO][O2])2

Diff: 1

Section: 13.3

16) The reaction, NO2Cl(g) + Cl(g) → NO2(g) + Cl2(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

A) rate = k[NO2]2

B) rate = k[Cl]

C) rate = k[NO2Cl][Cl][NO2][Cl2]

D) rate = k[NO2Cl][Cl]

E) rate = k[NO2][ Cl2]

Diff: 1

Section: 13.3

17) A reaction has the rate law: rate = k[A][B]2. What is the overall order of the reaction?

A) 2nd

B) 4th

C) 1st

D) 3rd

E) 0

Diff: 1

Section: 13.3

18) A reaction has the rate law, rate = k[A][B]3. What is the overall order of the reaction?

A) 0

B) 4th

C) 1st

D) 3rd

E) 2nd

Diff: 1

Section: 13.3

19) The reaction 2NO (g) + 2H2 (g) → N2 (g) + 2H2O (g) was found to follow the rate law:

rate = k[NO]2[H2]. By what factor will the rate of reaction increase if the pressure of NO gas is increased from 2.0 atm to 3.0 atm? Assume all other conditions are held constant.

A) 1.5

B) 1

C) 2.25

D) 2

E) 3

Diff: 2

Section: 13.3

20) A reaction has the rate law: rate = k[A][B]2. What is the order of the reaction, with respect to B?

A) 2nd

B) 4th

C) 1st

D) 3rd

E) 0

Diff: 1

Section: 13.3

21) A reaction has the rate law: rate = k[A]3[B]. What is the order of the reaction, with respect to A?

A) 2nd

B) 4th

C) 1st

D) 3rd

E) 0

Diff: 1

Section: 13.3

22) For the reaction, 2 XO + O2 → 2 XO2, data obtained from measurement of the initial rate of reaction at varying concentrations are given below.

Experiment [XO] (mol L-1) [O2] (mol L-1) Rate (mmol L-1 s-1 )

1 0.010 0.010 2.5

2 0.010 0.020 5.0

3 0.030 0.020 45.0

The rate law is therefore:

A) rate = k[XO]2 [O2]

B) rate = k[XO][O2]2

C) rate = k[XO][O2]

D) rate = k[XO]2 [O2]2

E) rate = k[XO]2/[O2]2

Diff: 1

Section: 13.3

23) The units of the rate constant for a particular reaction are min-1. What is the overall order of the reaction?

A) Zero

B) First

C) Second

D) Third

E) Fourth

Diff: 1

Section: 13.3

24) The units of the rate constant for a particular reaction are L mol-1 min-1. What is the overall order of the reaction?

A) Zero

B) First

C) Second

D) Third

E) Fourth

Diff: 1

Section: 13.3

25) Nitric oxide reacts with bromine at elevated temperatures according to the equation

2 NO(g) + Br2(g) → 2 NOBr(g)

The experimental rate law is rate = k[NO][Br2]. In a certain reaction mixture, the rate of formation of NOBr(g) was found to be 4.50 × 10-4 mol L-1 s-1. Which unit below is the correct unit for the rate constant?

A) mol L-1 s-1

B) s-1

C) mol2 L-2 s-1

D) L mol-1 s-1

E) L2 mol-2 s-1

Diff: 2

Section: 13.3

26) For the reaction, 3B + C → E + 2F, initial rate measurements were carried out and data from three trials are shown below:

Experiment [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 s-1)

1 0.100 0.250 0.000250

2 0.200 0.250 0.000500

3 0.100 0.500 0.00100

The rate law, therefore, is

A) rate = k[B]3[C]

B) rate = k[B][C]

C) rate = k[B]2[C]2

D) rate = k[B]2[C]

E) rate = k[B][C]2

Diff: 1

Section: 13.3

27) Given the reaction,

aA + bB → dD + eE

If we try rate = k[A]q[B]r for a generic rate law statement, which one of the statements below is false?

A) The exponents q and r are often integers.

B) The exponent q and r must be determined experimentally.

C) The exponents q and r are equal to the coefficients a and b, respectively.

D) The overall order of the reaction is q + r.

E) The symbol k represents the rate constant.

Diff: 1

Section: 13.3

28) The reaction, A + 2B products, was studied. A timer was started when reagents A and B were mixed, and stopped when a specific quantity of product C accumulated. The data contains initial amounts of reactants used and the time needed to reach the specific quantity of C. Based on the data below, we can conclude that

Experiment [A] (mol L-1) [B] (mol L-1) Time (secs)

1 0.100 0.140 25

2 0.050 0.140 50

3 0.100 0.070 100

Hint: Remember reaction rate is proportional to 1/time.

A) the reaction is first order with respect to substance A.

B) the reaction is zero order with respect to substance A.

C) the reaction is one-half order with respect to substance A.

D) the reaction is second order with respect to substance A.

E) the reaction is third order with respect to substance B

Diff: 2

Section: 13.3

29) For the reaction, 2M + 2N → 2P + Q, studies on how the initial rate of the reaction varied with concentration were carried out. Some data is given below.

Experiment [M] (mol L-1) [N] (mol L-1) Rate (mol L-1 s-1 )

1 0.100 0.100 0.000230

2 0.100 0.200 0.000920

3 0.200 0.200 0.000920

A) the rate law is therefore: rate = k[N]2

B) the rate law is therefore: rate = k[M][N]2

C) the rate law is therefore: rate = k[M][N]

D) the rate law is therefore: rate = k[M]2

E) the rate law is therefore: rate = k[M]2[N]2

Diff: 2

Section: 13.3

30) For the reaction, A + 2B → C + 2D, the following data were obtained .

Experiment [A] (mol L-1) [B] (mol L-1) Rate (mol L-1 s-1 )

1 0.100 0.200 0.000360

2 0.200 0.200 0.000720

3 0.100 0.400 0.000720

A) the rate law is therefore: rate = k[A][B]2

B) the rate law is therefore: rate = k[B]

C) the rate law is therefore: rate = k[A]

D) the rate law is therefore: rate = k[A][B]

E) the rate law is therefore: rate = k[A]2[B]

Diff: 2

Section: 13.3

31) For the reaction, A + 2B → C + 2D, some measurements of the initial rate of reaction at varying concentration gave the following data.

Experiment [A] (mol L-1) [B] (mol L-1) Rate (mol L-1 s-1 )

1 0.100 0.200 0.000360

2 0.150 0.200 0.000540

3 0.150 0.250 0.001055

A) the rate law is therefore: rate = k[A]2[B]

B) the rate law is therefore: rate = k[A][B]2

C) the rate law is therefore: rate = k[A]2[B]2

D) the rate law is therefore: rate = k[A][B]

E) the rate law is therefore: rate = k[A][B]3

Diff: 2

Section: 13.3

32) The reaction, 2A2X4(g) → 2A2X3(g) + X2(g), was found to be first order. The rate law, therefore, should be:

A) rate = k([A2X3]2[X2])/[A2X4]2

B) rate = k[A2X4]2

C) rate = k([A2X3][X2])/[A2X4]

D) rate = k[A2X4]

E) rate = k[A2X4]2/([A2X3]2[X2])

Diff: 2

Section: 13.3

33) The data below were obtained in a study on how the rate of a reaction was affected by the concentration of its reactants. The data indicate:

Experiment [A] (mol L-1) [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 hr-1)

1 0.200 0.100 0.600 5.0

2 0.200 0.400 0.400 80.0

3 0.600 0.100 0.200 15.0

4 0.200 0.100 0.200 5.0

5 0.200 0.200 0.400 20.0

A) the order of the reaction with respect to C cannot be determined.

B) the reaction is second order with respect to C.

C) the reaction is zero order with respect to C.

D) the reaction is first order with respect to C.

E) the order of the reaction with respect to C is minus one.

Diff: 2

Section: 13.3

34) Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants:

Experiment [A] (mol L-1) [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 hr-1)

1 0.200 0.100 0.600 5.0

2 0.200 0.400 0.400 80.0

3 0.600 0.100 0.200 15.0

4 0.200 0.100 0.200 5.0

5 0.200 0.200 0.400 20.0

A) the reaction is zero order with respect to B.

B) the reaction is first order with respect to B.

C) the reaction order for B cannot be determined.

D) the reaction is second order with respect to B.

E) the reaction order for B is minus one.

Hint: When you have three reactants, determine if any of them are 0 order.

Diff: 2

Section: 13.3

35) Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants:

Experiment [A] (mol L-1) [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 hr-1)

1 0.200 0.100 0.600 5.0

2 0.200 0.400 0.400 80.0

3 0.600 0.100 0.200 15.0

4 0.200 0.100 0.200 5.0

5 0.200 0.200 0.400 20.0

A) the reaction is first order with respect to A.

B) the reaction is second order with respect to A.

C) the reaction is zero order with respect to A.

D) the reaction order for A is minus one (Rate proportional to 1/[A]).

E) the reaction order for A cannot be determined from just this data alone.

Hint: When you have three reactants, determine if any of them are 0 order.

Diff: 2

Section: 13.3

36) Given these data in a study on how the rate of a reaction was affected by the concentration of the reactants, what is the numerical value of the rate constant, (k), for this reaction (where units match the data)?

Experiment [A] (mol L-1) [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 hr-1)

1 0.200 0.100 0.600 5.0

2 0.200 0.400 0.400 80.0

3 0.600 0.100 0.200 15.0

4 0.200 0.100 0.200 5.0

5 0.200 0.200 0.400 20.0

A) 2083

B) 694

C) 417

D) 2500

E) 83.3

Hint: When you have three reactants, determine if any of them are 0 order.

Diff: 2

Section: 13.3

37) What is the order of the reaction with respect to reactant A?

Determining A Rate Law From Experimental Data

The following data was found for the reaction:

A + B → Products

A) Zero

B) First

C) Second

D) Third

E) Fourth

Diff: 2

Section: 13.3

38) What is the order of the reaction with respect to reactant B?

Determining A Rate Law From Experimental Data

The following data was found for the reaction

A + B → Products

A) Zero

B) First

C) Second

D) Third

E) Fourth

Diff: 2

Section: 13.3

39) The data shown below was determined for the reaction A + B → Products.

Which of the following is the correct rate law for this reaction?

A) rate = k[A][B]

B) rate = k[A]

C) rate = k[B]2

D) rate = k[B]

E) rate = k[A][B]2

Diff: 2

Section: 13.3

40) The data shown below was determined for the reaction A + B → Products.

What is the numerical value of the rate constant, (k), for this reaction?

A) 258.2

B) 378.8

C) 1.72 × 104

D) 8.33

E) 1.125

Diff: 2

Section: 13.3

41) The data shown below was determined for the reaction A + B → Products.

What is the missing value in the table, for the initial rate of the reaction in Experiment 5?

A) 1.125

B) 0.500

C) 2.83

D) 1.53

E) 2.00

Diff: 2

Section: 13.3

42) The half-life of a chemical reaction was found to be independent of the quantity of reactant which was employed. The reaction is, therefore,

A) possibly first order.

B) definitely first order.

C) zero order.

D) possibly second order.

E) definitely second order.

Diff: 2

Section: 13.3

43) If a reaction involving a single reactant is first order, with a rate constant of 4.50 × 10-2 s-1, how much time is required for 75.0% of the initial quantity of reactant to be used up?

A) 16.7 seconds

B) 30.9 seconds

C) 23.1 seconds

D) 25.3 seconds

E) 11.6 seconds

Diff: 2

Section: 13.4

44) Graph b can best be described as

A) Zero-order rate process.

B) First-order rate process.

C) Second-order rate process.

D) B or C

E) A or C

Diff: 1

Section: 13.4

45) We should determine the reaction order from graph b by

A) plotting [A] vs. time.

B) plotting 1/[A] vs. time.

C) plotting ln[A] vs. time.

D) plotting the square root of concentration vs. time.

E) B and C

Diff: 1

Section: 13.4

46) Concentration vs. time data for a first-order reaction is shown in the graph below. What should be done to determine the half-life of the reaction?

A) Multiply [A] by k

B) Plot 1/[A] vs. time

C) Plot ln[A] vs. time

D) Plot the square root of concentration vs. time

E) B and C

Diff: 1

Section: 13.4

47) The initial concentration of a reactant in a first-order reaction is 0.620 M. What will be its concentration after 3 half-lives have passed?

A) 0.0865 M

B) 0.0775 M

C) 0.310 M

D) 0.207 M

E) 0.103 M

Diff: 2

Section: 13.4

48) The initial concentration of a reactant in a first-order reaction is 0.860 M. What will be its concentration after 4 half-lives have passed?

A) 0.215 M

B) 0.0538 M

C) 0.250 M

D) 0.125 M

E) 0.108 M

Diff: 2

Section: 13.4

49) The reaction A → Products is a zero-order reaction with a rate constant of 4.81 × 10-3 M s-1. If the reaction starts with a 33.1 M concentration of A, at what time will the concentration of A be 24.1 M?

A) 43.7 min

B) 72.8 min

C) 661 min

D) 1870 min

E) 31.2 min

Diff: 2

Section: 13.4

50) In a first-order reaction with only one reagent, the reaction was started with a concentration of reactant equal to 0.0800 M. After exactly two hours, the concentration had fallen to 0.0400 M. What is the molarity after exactly four hours?

A) 0.0000 M

B) 0.0100 M

C) 0.0150 M

D) 0.0200 M

E) 0.0300 M

Diff: 1

Section: 13.4

51) The decomposition of an aldehyde solution in carbon tetrachloride is a first-order reaction with a rate constant of 1.20 × 10-3 min-1. If we start with [aldehyde] = 0.0500 M, what will the concentration of aldehyde be 150 minutes later?

A) 0.00900 M

B) 0.0418 M

C) 0.00926 M

D) 0.00499 M

E) 0.000333 M

Diff: 1

Section: 13.4

52) The initial concentration of a reactant in a first order reaction is 0.620 M. What will be its concentration after 3 half-lives?

A) 0.0865 M

B) 0.310 M

C) 0.0775 M

D) 0.103 M

E) 0.207 M

Diff: 1

Section: 13.4

53) For the reaction, A → B + C, the rate law is rate = k[A]. If it takes 80.0 seconds for 70.0% of a 10.0 gram sample of A to be transformed into products, what is the value of the rate constant?

A) 0.00450 s-1

B) 0.0290 s-1

C) 0.00530 s-1

D) 0.0150 s-1

E) 5.40 s-1

Diff: 2

Section: 13.4

54) For the reaction, A → B + C, the rate law is rate = k[A] where k = 0.0175 s-1. How long will it take to reach 35.0 g from a 100.0 g sample?

A) 1.00 min

B) 7.77 min

C) 0.0184 s

D) 39.6 s

E) 1.06 s

Diff: 2

Section: 13.4

55) The reaction of substance A with substance C was carefully studied under conditions where the [C] remained essentially constant. The graph of [A] vs. time gave a straight line while the graph of ln[A] vs. time and that of 1/[A] vs. time both gave curves.

A) The reaction is therefore zero order with respect to A.

B) The reaction is therefore one-half order with respect to A.

C) The reaction is therefore first order with respect to A.

D) The reaction is therefore second order with respect to A.

E) The reaction is therefore third order with respect to A.

Diff: 1

Section: 13.4

56) A reaction is first-order overall. For a given sample, its initial rate is 0.0200 mol L-1 s-1, and 25.0 days later its rate dropped to 6.25 × 10-4 mol L-1 s-1. What is its half-life?

A) 25.0 days

B) 50.0 days

C) 12.5 days

D) 5.0 days

E) 37.5 days

Diff: 1

Section: 13.4

57) In a first-order reaction with only one reagent, the reaction was started with a concentration of reactant equal to 0.0800 M. After exactly two hours, the concentration had fallen to 0.0400 M. What is the molarity after exactly six hours?

A) 0.0000 M

B) 0.0100 M

C) 0.0150 M

D) 0.0200 M

E) 0.0300 M

Diff: 2

Section: 13.4

58) The rate constant for a first-order decomposition reaction is 0.0111 min-1. What is the half-life of the reaction?

A) 111 min

B) 62.4 min

C) 5000 sec

D) 31.25 min

E) 27.1 min

Diff: 1

Section: 13.4

59) Given a reaction, 2A + B → P, for which the rate law is rate = k[A]. Which equation or statement is true?

A) [A] = 1/kt

B) ln[A] = k/t

C) 1/[A] = kt

D) The half-life is 0.693/k.

E) e[A] = kt

Diff: 1

Section: 13.4

60) In a first-order reaction, what fraction of the reactant will remain after 4 half-lives?

A) 1/16

B) 1/8

C) 1/9

D) 1/4

E) 1/3

Diff: 2

Section: 13.4

61) In a first-order reaction, what fraction of the reactant will remain after 3 half-lives?

A) 1/16

B) 1/8

C) 1/9

D) 1/4

E) 1/3

Diff: 2

Section: 13.4

62) A first-order reaction has a rate constant of 0.00318 min1. The half-life of this reaction is, therefore,

A) 94.7 minutes.

B) 218 minutes.

C) 31.4 minutes.

D) 5.24 seconds.

E) 68.6 minutes.

Diff: 1

Section: 13.4

63) For the reaction

2A + B → Products

The rate equation was found to be rate = k[A]2. If the rate constant was found to be 0.045 M-1 min-1 and the reaction started with an initial concentration of A equal to 0.50 M, what is the concentration of A after 30.0 minutes?

A) 0.011 M

B) 0.13 M

C) 0.30 M

D) 1.54 M

E) 3.35 M

Diff: 2

Section: 13.4

64) For the reaction

2A + B → Products

The rate equation was found to be rate = k[A]2. If the rate constant was found to be 0.035 M-1 min-1 and the reaction started with an initial concentration of A equal to 0.50 M, how long will it take for the concentration of A to reach 0.25 M?

A) 4.2 sec

B) 57.1 min

C) 49.8 min

D) 1.05 sec

E) 53.5 min

Diff: 2

Section: 13.4

65) The reaction A → Products is a zero-order reaction with a rate constant of 2.56 × 10-3 M s-1. If the concentration of A is 75.6 M after 12.7 minutes, what was the initial concentration of A?

A) 838 M

B) 100 M

C) 75.6 M

D) 77.6 M

E) 73.6 M

Diff: 2

Section: 13.4

66) At a certain temperature the second-order reaction NOCl(g) → NO(g) + 1/2Cl2(g) is 50% complete after 6.23 hours when the initial concentration of NOCl is 4.78 mol/L. How long will it take for the reaction to be 75% complete?

A) 18.7 hr

B) 17.5 hr

C) 8.2 hr

D) 31.5 hr

E) 12.5 hr.

Diff: 2

Section: 13.4

67) Charcoal taken from the site of an ancient village was found to have a 14C to 12C ratio of one-third that is found in living plant life. Using this data, what is the age of the charcoal sample? The half-life of 14C is 5730 years.

A) 12,300 yrs.

B) 9,080 yrs.

C) 6,950 yrs.

D) 1,800 yrs.

E) 2510 yrs.

Diff: 2

Section: 13.4

68) For a first-order reaction with a single reactant, after 230.0 seconds, 10.0% of the reactant remains. The rate constant for the reaction is, therefore,

A) 0.000640 s-1

B) 0.0100 s-1

C) 100 s-1

D) 0.0510 s-1

E) 0.0915 s-1

Diff: 2

Section: 13.4

69) Graph a can best be described as a

A) Zero-order rate process.

B) First-order rate process.

C) Second-order rate process.

D) B or C

E) A or C

Diff: 1

Section: 13.4

70) The reaction of substance A with substance C was carefully studied under conditions where the [C] remained essentially constant. The graphs of [A] vs. time and that of ln[A] vs. time both gave curves, but the graph of 1/[A] vs. time gave a straight line.

A) The reaction is therefore zero order with respect to A.

B) The reaction is therefore one-half order with respect to A.

C) The reaction is therefore first order with respect to A.

D) The reaction is therefore second order with respect to A.

E) The reaction is therefore third order with respect to A.

Diff: 1

Section: 13.4

71) A sample of Peruvian corn was found to have a 14C to 12C ratio of 8.0 × 10-13. Similar corn samples taken present day have a 14C to 12C ratio of 1.2 × 10-12. Using this data, what is the age of the Peruvian corn sample?

Hint: The half-life of 14C is 5730 years.

A) 2.5 yrs.

B) 15,700 yrs.

C) 5,240 yrs.

D) 1,470 yrs.

E) 3,350 yrs.

Diff: 3

Section: 13.4

72) What two factors influence the effectiveness of molecular collisions in producing chemical change?

1. The molar masses of the reactants

2. The activation energy

3. The pressure

4. The orientation of the reactants

A) 3 and 4

B) 1 and 3

C) 1 and 2

D) 2 and 4

E) 2 and 3

Diff: 2

Section: 13.5

73) When there is an increase in temperature of a system the rate of reaction often increases. Which of the following best explains why this happens?

1. The concentrations increase with temperature.

2. The number of collisions with the sufficient kinetic energy increase with temperature.

3. The number of collisions per unit time increases with temperature.

4. The orientation of the molecules change with temperature.

A) 3 and 4

B) 1 and 3

C) 1 and 2

D) 2 and 4

E) 2 and 3

Diff: 2

Section: 13.5

74) For a one step reaction, the activation energy for the forward reaction is 40.0 kJ mol-1, and the heat of reaction is 20.0 kJ mol-1. Which statement below is true?

A) The activation energy of the forward reaction would be affected to a greater extent than the activation energy of the reverse reaction by addition of a catalyst.

B) The value for the heat of reaction would be decreased by addition of a catalyst.

C) The reaction is endothermic.

D) The reverse reaction has a higher activation energy than the forward reaction.

E) The reaction rate would be decreased by an increase in temperature.

Diff: 1

Section: 13.6

75) For a one-step reaction, the activation energy for the forward reaction is 40.0 kJ mol-1, and the heat of reaction is 20.0 kJ mol-1. Calculate the activation energy for the reverse reaction.

A) +60.0 kJ mol-1

B) -20.0 kJ mol-1

C) -1200 kJ mol-1

D) +20.0 kJ mol-1

E) +1200 kJ mol-1

Diff: 1

Section: 13.6

76) The reaction progress for a given reaction is shown below. Which corresponds to the activation energy of the forward reaction, Ea?

A) A

B) B

C) C

D) D

E) none of these

Diff: 1

Section: 13.6

77) The reaction progress for a given reaction is shown below. Which corresponds to the overall energy change of the reaction, ? (The heat of reaction)

A) A

B) B

C) C

D) D

E) none of these

Diff: 1

Section: 13.6

78) The reaction progress for a given reaction is shown below. The point on the diagram where the energy of the system is at a maximum is called the

A) transition state.

B) critical point.

C) formation energy of the reactants.

D) formation energy of the products.

E) rate determining state.

Diff: 1

Section: 13.6

79) The reaction progress for a given reaction is shown below. Which corresponds to the activation energy of the reverse reaction, Ea?

A) A

B) B

C) C

D) D

E) none of these

Diff: 1

Section: 13.6

80) The reaction A + 3B → D + F was studied, and the following mechanism was determined

A + B C (fast)

C + B → D + E (slow)

E + B → F (very fast)

The step with largest activation energy is

A) the first step.

B) the second step.

C) the third step.

D) None of the steps has an activation energy.

E) All of the steps have the same activation energy.

Diff: 1

Section: 13.6

81) For a given chemical reaction, the rate constant at 250.0 °C is 0.00383 s-1, and the activation energy is 22.40 kJ mol-1. Calculate the value of the rate constant at 335.0 °C.

A) 0.00513 s-1

B) 0.00946 s-1

C) 0.00787 s-1

D) 0.0224 s-1

E) 0.000640 s-1

Diff: 2

Section: 13.7

82) For a given chemical reaction, the rate constant at 42.0 °C is 0.00395 s-1, while the rate constant at 67.4 °C is 0.0133 s-1. Calculate the value of the activation energy, in kilojoules per mole.

A) 42.6

B) 1.13

C) 0.421

D) 18.5

E) 0.617

Diff: 2

Section: 13.7

83) The rate constant for a certain chemical reaction is 0.00250 L mol-1 s-1 at 25.0 °C and 0.0125 L mol-1 s-1 at 50.0 °C. What is the activation energy for the reaction?

A) 25.1 kJ mol-1

B) 51.6 kJ mol-1

C) 37.6 kJ mol-1

D) 45.3 kJ mol-1

E) 60.3 kJ mol-1

Diff: 2

Section: 13.7

84) For a particular chemical reaction, the rate constant at 30.0 °C is 1.38 × 10-4 L mol-1 s-1, while the value at 49.0 °C is 1.21 × 103 L mol-1 s-1. What is the activation energy for this reaction?

A) 92.8 kJ mol-1

B) 200 kJ mol-1

C) 40.4 kJ mol-1

D) 343 kJ mol-1

E) 56.4 kJ mol-1

Diff: 2

Section: 13.7

85) The activation energy for a reaction can be found by finding the slope of a plot of ln(k) vs. T-1 and

A) adding this slope to -R.

B) multiplying this slope by 2.303.

C) dividing this slope by -R.

D) multiplying this slope by 2.303R.

E) multiplying this slope by -R.

Diff: 2

Section: 13.7

86) The reaction: 2A + 2B → D + F was studied carefully and the following mechanism was determined.

A + A → C (slow)

C + B → D + E (fast)

E + B → F (very fast)

The rate law for the reaction would therefore be

A) rate = k[A]2

B) rate = k[A]2[B]2

C) rate = k[C][B]

D) rate = k[A][B]3

E) rate = k[A][B]

Diff: 1

Section: 13.8

87) Which statement about the slow step in the mechanism for a reaction mechanism is true?

A) It has a rate that is independent of the activation energy for the reaction.

B) It limits the effectiveness of a catalyst.

C) It controls the rate at which the products are produced.

D) It almost always involves the breaking of hydrogen bonds.

E) It determines the value of the standard enthalpy of reaction for the reaction.

Diff: 1

Section: 13.8

88) If the reaction H2(g) + Cl2(g) → 2 HCl(g) occurred in just two steps, what would the overall order of the reaction be?

A) 1st

B) 2nd

C) 3rd

D) 4th

E) It is impossible to determine the order from this limited information.

Diff: 1

Section: 13.8

89) The reaction mechanism proposed for the decomposition of H2O2 is

H2O2 + I- s H2O + IO (slow)

H2O2 + IO- → H2O + O2 + I- (fast)

Which statement is true?

A) The reaction is second order with respect to I-.

B) I is an intermediate.

C) The reaction is first order with respect to I-.

D) IO- is a catalyst.

E) The reaction is zero order with respect to I-.

Diff: 2

Section: 13.8

90) The reaction mechanism proposed for the decomposition of H2O2 is

NO2 + NO2 → NO3 + NO (slow)

NO3 + CO → NO2 + CO2 (fast)

Which statement is true?

A) The reaction is first order with respect to NO2.

B) NO2 is an intermediate.

C) The reaction is first order with respect to CO.

D) The reaction is second order with respect to NO2.

E) The reaction is zero order with respect to NO2.

Diff: 2

Section: 13.8

91) Suppose the reaction A + B → D followed the mechanism below. What would be the rate law for the reaction?

A + B C (fast)

C → D (slow)

A) rate = k[A]

B) rate = k[A]2

C) rate = k[A][B]

D) rate = k[A][B]/[D]

E) rate = k[A][B][C]

Diff: 3

Section: 13.8

92) The reaction: A + 3B → D + F was studied carefully and the mechanism below was determined. What is the rate law for the reaction?

A + B C (fast)

C + B → D + E (slow)

E + B → F (very fast)

Hint: Express the rate limiting step in terms of reactants present in the overall reaction.

A) rate = k[A]2[B]

B) rate = k[A][B]2

C) rate = k[C][B]

D) rate = k[A][B]3

E) rate = k[A][B]

Diff: 3

Section: 13.8

93) The reaction: A + 3B → D + F was studied carefully and the mechanism below was determined. What is the rate law for the reaction?

A + B → C (slow)

C + B → D + E (fast)

E + B → F (very fast)

A) rate = k[A]2[B]

B) rate = k[A][B]2

C) rate = k[C][B]

D) rate = k[A][B]3

E) rate = k[A][B]

Diff: 2

Section: 13.8

94) A variable which has no effect on the rate of a chemical reaction is

A) energy of activation.

B) a catalyst.

C) the concentration of the reactants.

D) the temperature.

E) the standard heat of reaction for the system.

Diff: 2

Section: 13.9

95) Which statement concerning the rate of a chemical reaction is false?

A) It will be very rapid if the activation energy is large.

B) It will be slow if one or more of the steps is slow.

C) It may be inhibited sometimes by certain catalytic agents.

D) It is dependent on temperature.

E) It often increases when the concentrations of one of the reactants is increased.

Diff: 1

Section: 13.9

96) A chemical reaction has been the subject of intense study, and a rate law, rate = k[A][B]2, was developed which summarized the mechanistic findings. Which change to the system will not cause an increase in the rate constant under any circumstances?

A) raising the temperature by 25 degrees

B) adding a positive catalyst

C) tripling the concentration of A

D) doubling the concentration of B

E) lowering the temperature by 0.5 degrees

Diff: 1

Section: 13.9

97) The reaction, A + 3B → D + F was studied, and the following mechanism was established:

A + B C (fast)

C + B → D + E (slow)

E + B → F (very fast)

The species, E, is properly described as

A) an intermediate.

B) a cofactor.

C) a catalyst.

D) an inhibitor.

E) an enzyme.

Diff: 1

Section: 13.9

98) The reaction: A + 3 B → D + F was studied and the following mechanism was determined.

A + B C (fast)

C + B → D + E (slow)

E + B → F (very fast)

The species, C, is properly described as

A) a cofactor.

B) an inhibitor.

C) a catalyst.

D) an enzyme.

E) an intermediate.

Diff: 1

Section: 13.9

99) A catalyst alters the rate of a chemical reaction by

A) providing an alternate pathway that has a different activation energy.

B) changing the products formed in the reaction.

C) changing the frequency of collisions between molecules.

D) always providing a surface on which molecules react.

E) changing the enthalpy of reaction for the reaction.

Diff: 1

Section: 13.9

100) Which statement is true concerning a negative catalyst (inhibitor)?

A) It lowers the energy of activation of the rate determining step.

B) It increases the heat of reaction.

C) It never undergoes a chemical change at any time during a chemical reaction.

D) It blocks the path with the highest energy of activation for the rate determining step.

E) It blocks the path with the lowest energy of activation for the rate determining step.

Diff: 2

Section: 13.9

101) Which statement describes the situation when a catalyst is used in a reaction? Remember that the book says that the term 'catalyst' will be used to mean a positive catalyst.

A) The forward reaction rate is increased while the reverse reaction rate is slowed.

B) The heat change for the reaction becomes more exothermic.

C) The final (equilibrium) amounts of reactants and products are not affected.

D) The activation energy for the reverse reaction is increased.

E) The activation energy for the forward reaction is not altered.

Diff: 1

Section: 13.9

102) A reaction has the following proposed mechanism:

A2(g) + B(s) → A2B(s) (fast)

A2B(s) → A(g) + AB(s) (slow)

AB(s) + C(g) → AC(g) + B(s) (fast)

A(g) + C(g) → AC(g) (fast)

For this mechanism, the species B would best be classified as a(n)

A) product.

B) homogeneous catalyst.

C) intermediate.

D) heterogeneous catalyst.

E) transition state structure.

Diff: 1

Section: 13.9

103) List the five factors that can affect the rate at which reactions proceed.

Diff: 1

Section: 13.1

104) Heterogeneous catalysis often takes place at transition metal surfaces. Which would be a better choice for a catalyst–a gold sphere with a radius of 18Å, or 15 gold spheres, each with a radius of 5 Å?

Hint: The surface area of a sphere is given by: A = 4πr2.

Diff: 1

Section: 13.1

105) What is the difference between the average and instantaneous rates of a reaction?

Diff: 2

Section: 13.1

106) One reaction that can be used to remove NO gas from power plant emission is its reaction with methane.

CH4(g) + 4NO(g) → 2N2(g) + CO2(g) + H2O(g)

If NO is being removed at a rate of 1.18 × 10-2 mol L-1 s-1, at what rate is N2 gas being formed?

Diff: 2

Section: 13.2

107) The units of the rate constant for a particular reaction are L mol-1 min-1. What is the overall order of the reaction?

Diff: 1

Section: 13.3

108) The reaction:

A + 2B → products

has the rate law:

rate = k[A][B]3

For this reaction, the overall reaction order would be ________.

Diff: 1

Section: 13.3

109) If a reaction was found to be 4th order overall, what would be the units for the rate constant, in terms of M and s?

Diff: 1

Section: 13.3

110) The reaction A + 2B → products was found to follow the rate law, rate = k[A]2[B]. The rate of reaction will increase by a factor of ________ when the concentration of A is tripled, the concentration of B is doubled, and the temperature remains constant.

Diff: 1

Section: 13.3

111) The reaction A + 2B → products was found to follow the rate law, rate = k[A][B]3. The rate of reaction will increase by a factor of ________ when the concentration of A is unchanged, the concentration of B is doubled, and the temperature remains constant.

Diff: 1

Section: 13.3

112) The decomposition of a compound is known to be a first-order reaction. If the half-life of the reaction is 6.25 minutes at 65 °C, what is the value of the rate constant for the reaction at this temperature?

Diff: 1

Section: 13.4

113) A first-order reaction begins with 176 g of reactant. After 2.6 days, the amount of reactant that remains is 88 g. How much reactant will remain after 5.2 days?

Diff: 1

Section: 13.4

114) A first-order reaction has a rate constant of 3.51 × 10-3 s-1. The time required for the reaction to be 63% complete is ________.

Diff: 1

Section: 13.4

115) The nuclear transmutation reaction of X is a first-order reaction. If the half-life of X is 188.5 hours, how much would a sample weighing 14.55 mg today weigh at the same time tomorrow?

Diff: 2

Section: 13.4

116) An isomerization reaction of a substance, A, is first order. In a laboratory class, one student group found that 28.5% of A had isomerized after a period of 15.0 minutes, when the temperature was maintained at 84.5 °C. What is the half-life of substance A at that temperature?

Diff: 2

Section: 13.4

117) A reaction is hypothesized to be a second-order reaction with respect to reactant A. What should be plotted and what would you expect to see in that plot to if the reaction is second order with respect to reactant A?

Diff: 1

Section: 13.4

118) A certain reaction A → products is second order in A. If this reaction is 20% complete in 13 minutes, how long would it take, in hours, for the reaction to be 85% complete?

Diff: 2

Section: 13.4

119) Concentration vs. time data for a first order reaction is shown in the graph below. The best estimate of the half-life of the reaction, as deduced from the figure, is:

Diff: 1

Section: 13.4

120) Why does increasing the temperature of a reaction mixture increase the reaction rate?

Diff: 1

Section: 13.6

121) For the reaction A + B → products, the rate law was determined experimentally to be:

Rate = k[B]2

Using this information, could the reaction happen in a single step, or would it require multiple steps? Explain.

Diff: 2

Section: 13.7

122) What effect does the magnitude of the standard enthalpy of reaction have on the rate constant for a reaction, if the temperature is kept constant?

Diff: 2

Section: 13.7

123) A reaction has the following proposed mechanism:

A2(g) + B(s) → A2B(s) (fast)

A2B(s) → A(g) + AB(s) (slow)

AB(s) + C(g) → AC(g) + B(s) (fast)

A(g) + C(g) → AC(g) (fast)

Identify any intermediate(s) in this mechanism.

Diff: 1

Section: 13.8

124) For a reaction involving NO and Br2, the following mechanism has been proposed:

NO + Br2 → NOBr2 (slow)

NOBr2 + NO → NOBr + NOBr (fast)

Write the rate law for the formation of NOBr implied by this mechanism.

Diff: 1

Section: 13.8

125) The reaction A + B → products is determined to be an elementary process. If this is true can you determine the rate law for this reaction and if so what is it?

Diff: 2

Section: 13.8

126) The decomposition of ozone to oxygen has the following proposed mechanism:

O3(g) O2(g) + O(g) (fast)

O(g) + O3(g) → 2O2(g) (slow)

What is the rate determining step?

Diff: 2

Section: 13.8

127) What is the difference between homogenous and heterogeneous catalysis?

Diff: 1

Section: 13.9

128) A reaction has the following proposed mechanism:

A2(g) + B(s) → A2B(s) (fast)

A2B(s) → A(g) + AB(s) (slow)

AB(s) + C(g) → AC(g) + B(s) (fast)

A(g) + C(g) → AC(g) (fast)

Using this mechanism, what is the overall reaction?

Diff: 1

Section: 13.9

129) Describe, in words, the effects of a catalyst on a chemical reaction.

Diff: 1

Section: 13.9

130) What effect does a negative catalyst have on the value of the rate constant for a particular reaction?

Diff: 2

Section: 13.9

131) A catalyst used by a biological system is given a special name called a(n)

Diff: 2

Section: 13.9

132) One reaction that can be used to remove NO gas from power plant emission is its reaction with methane.

CH4(g) + 4NO(g) → 2N2(g) + CO2(g) + H2O(g)

In this reaction, CH4 is being removed at the same rate that CO2 is being produced.

Diff: 2

Section: 13.2

133) One reaction that can be used to remove NO gas from power plant emission is its reaction with methane.

CH4(g) + 4NO(g) → 2N2(g) + CO2(g) + H2O(g)

In this reaction, NO is being removed at the same rate that CO2 is being produced.

Diff: 2

Section: 13.2

134) If increasing the concentration of a particular reactant in a reaction mixture by a factor of three fails to cause any measurable change in the rate of a chemical reaction, the order of reaction with respect to that particular reactant is zero.

Diff: 1

Section: 13.3

135) Nitric oxide reacts with bromine at elevated temperatures according to the equation,

2 NO(g) + Br2(g) → 2 NOBr(g).

The experimental rate law is: rate = k[NO][Br2]. The half-life of either of the reactant species is independent of its concentration and is equal to 0.693/k.

Diff: 1

Section: 13.4

136) The activation energy of a reaction is equal to the difference between the potential energy of the reactants and the potential energy of the products.

Diff: 2

Section: 13.6

137) The activation energy of a reaction is equal to the difference between the activation energy for the forward step of the reaction and the potential energy of the reactants.

Diff: 2

Section: 13.6

138) The activation energy is the energy required to initiate a reaction, and the reaction will continue without additional outside energy.

Diff: 2

Section: 13.7

139) The coefficients of the balanced equation for an elementary step give the exponents in the rate law of that step.

Diff: 2

Section: 13.8

140) The fastest step in a multistep reaction mechanism is the net reaction.

Diff: 1

Section: 13.8

141) In order to carry out chemical kinetics studies, all reactants must be in a catalyzed form so that they will form products at the regular rate.

Diff: 1

Section: 13.8

142) The final step in a multistep reaction mechanism is always the rate-determining step.

Diff: 2

Section: 13.8

143) The step in a multistep reaction mechanism that has the highest activation energy is the rate-determining step.

Diff: 2

Section: 13.8

144) A catalyst that lowers the activation energy of the forward reaction in a system to one-half its uncatalyzed value will also lower the activation energy of the reverse reaction in the system to one-half its uncatalyzed value.

Diff: 1

Section: 13.9

145) The reaction rates for similar reactants are often much faster when they take place in a homogeneous reaction environment than when they take place in a heterogeneous reaction environment. An example of this would be the rate at which a log burns in comparison to a suspension of sawdust in air. The sawdust suspension will erupt in a large ball of fire very quickly, while the log burns at a much slower rate. Give an explanation of this, based on any of the five factors that may affect reaction rate.

Diff: 2

Section: 13.1

146) Given this data from a study on how the rate of a reaction was affected by the concentration of the reactants, determine the rate constant for the reaction.

Experiment [A] (mol L-1) [B] (mol L-1) [C] (mol L-1) Rate (mol L-1 hr-1)

1 0.200 0.100 0.600 5.0

2 0.200 0.400 0.400 80.0

3 0.600 0.100 0.200 15.0

4 0.200 0.100 0.200 5.0

5 0.200 0.200 0.400 20.0

A) 2500 L2 mol-2 hr-1

B) 208 L2 mol-2 hr-1

C) 139 L2 mol-2 hr-1

D) 2083 L2 mol-2 hr-1

E) 6667 L2 mol-2 hr-1

Diff: 2

Section: 13.3

147) The reaction A + 2B → products was found to follow the rate law, rate = k[A][B]3. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Diff: 2

Section: 13.3

148) A nuclear transmutation reaction is a first-order reaction. The mass of a sample was taken on three successive days at the same time. First day: 14.554 mg. Second day: 14.193 mg. Third day: 13.841 mg. What should the mass be at the same time on the fifth day?

Diff: 2

Section: 13.4

149) The reaction, 2 NO2(g) → 2 NO(g) + O2(g), has a rate constant of 0.110 L mol-1 s-1 when the temperature is 450 °C. How long, in seconds, would it take for a sample of NO2, whose concentration is initially 0.355 M, to decrease to 25.0% of its original concentration at this temperature?

Hint: use the units of the rate constant to determine the order of the reaction.

Diff: 2

Section: 13.4

150) The half-life of a first order chemical reaction is 24.0 minutes at 55.0°C and 16.4 minutes at 63.5°C. What will be the half-life, in minutes, at 70.0°C?________

Hint: Use the given information to solve for activation energy, then find the missing equilibrium constant. Remember t1/2 = .

Diff: 3

Section: 13.4

151) Suppose the reaction, 2A + 2B → 2D + F followed the mechanism:

A + B C + D (fast)

A + C → E (slow)

E + B → D + F (very fast)

The rate law for the reaction would be

A) rate = k[A]2[B]/[D]

B) rate = k[A][B][C]

C) rate = k[A][B]/[D]

D) rate = k[A]2[B]2

E) rate = k[A][B]2

Diff: 2

Section: 13.7

152) The decomposition of hydrogen peroxide in solution was studied in the laboratory, and the following mechanism was proposed based on the experimental data.

H2O2 + I- s H2O + IO- (slow)

H2O2 + IO- → H2O + O2 + I- (fast)

Which one of the following statements is false?

A) The reaction is first order with respect to H2O2.

B) The reaction is first order with respect to I-.

C) I- is a catalyst.

D) IO- is an intermediate.

E) The reaction is first order with respect to IO-.

Diff: 1

Section: 13.8

153) Many reactions require that the initial reactant become 'activated'. This activation often comes from the transfer of energy from a wall or other gas molecule. After the molecule is activated, it then proceeds to a reaction, such as the following decomposition:

A + M A* + M (fast)

A* → B + C (slow)

What is the overall rate law for this process?

Diff: 1

Section: 13.9

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