Chemistry: Structure and Properties

Nivaldo Tro

Chapter 14 Chemical Kinetics - all with Video Answers

Educators

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Chapter Questions

01:49

Problem 1

Explain why lizards become sluggish in cold weather. How is this phenomenon related to chemistry?

Allison Krajewski

Numerade Educator

01:43

Problem 2

Why are reaction rates important (both practically and theoretically)?

Eugene Schneider

University of Minnesota - Twin Cities

02:40

Problem 3

Using the idea that reactions occur as a result of collisions between particles, explain why reaction rates depend on the concentration of the reactants.

Allison Krajewski

Numerade Educator

00:46

Problem 4

Using the idea that reactions occur as a result of collisions between particles, explain why reaction rates depend on the temperature of the reaction mixture.

Eugene Schneider

University of Minnesota - Twin Cities

01:39

Problem 5

What units are typically used to express the rate of a reaction?

Allison Krajewski

Numerade Educator

00:39

Why is the reaction rate for reactants defined as the negative of the change in reactant concentration with respect to time, whereas for products it is defined as the change in reactant concentration with respect to time (with a positive sign)?

Eugene Schneider

University of Minnesota - Twin Cities

04:37

Problem 7

Explain the difference between the average rate of reaction and the instantaneous rate of reaction.

Allison Krajewski

Numerade Educator

02:28

Problem 8

Consider a simple reaction in which a reactant A forms products: What is the rate law if the reaction is zero order with respect to A? First order? Second order? For each case, explain how a doubling of the concentration of A would affect the rate of reaction.

Eugene Schneider

University of Minnesota - Twin Cities

01:45

Problem 9

How is the order of a reaction generally determined?

Allison Krajewski

Numerade Educator

01:11

Problem 10

For a reaction with multiple reactants, how is the overall order of the reaction defined?

Eugene Schneider

University of Minnesota - Twin Cities

02:57

Problem 11

Explain the difference between the rate law for a reaction and the integrated rate law for a reaction. What relationship does each kind of rate law express?

Ricajoy Montero

Numerade Educator

01:14

Problem 12

Write integrated rate laws for zero-order, first-order, and
second-order reactions of the form A products.

Eugene Schneider

University of Minnesota - Twin Cities

03:07

Problem 13

What does the term half-life mean? Write the expressions for the
half-lives of zero-order, first-order, and second-order reactions.

Ricajoy Montero

Numerade Educator

00:48

Problem 14

How do reaction rates typically depend on temperature? What
part of the rate law is temperature dependent?

Eugene Schneider

University of Minnesota - Twin Cities

05:49

Problem 15

Explain the meaning of each term within the Arrhenius
equation: activation energy, frequency factor, and exponential
factor. Use these terms and the Arrhenius equation to explain
why small changes in temperature can result in large changes in
reaction rates.

Ricajoy Montero

Numerade Educator

01:01

Problem 16

What is an Arrhenius plot? Explain the significance of the slope
and intercept of an Arrhenius plot.

Eugene Schneider

University of Minnesota - Twin Cities

02:42

Problem 17

Explain the meaning of the orientation factor in the collision model.

Ricajoy Montero

Numerade Educator

00:54

Problem 18

Explain the difference between a normal chemical equation for a
chemical reaction and the mechanism of that reaction.

Eugene Schneider

University of Minnesota - Twin Cities

04:02

Problem 19

In a reaction mechanism, what is an elementary step? Write
down the three most common elementary steps and the corresponding
rate law for each one.

Ricajoy Montero

Numerade Educator

00:56

Problem 20

What are the two requirements for a proposed mechanism to be
valid for a given reaction?

Eugene Schneider

University of Minnesota - Twin Cities

02:06

Problem 21

What is an intermediate within a reaction mechanism?

Ricajoy Montero

Numerade Educator

01:34

Problem 22

What is a catalyst? How does a catalyst increase the rate of a
chemical reaction?

Eugene Schneider

University of Minnesota - Twin Cities

01:58

Problem 23

Explain the difference between homogeneous catalysis and
heterogeneous catalysis.

Ricajoy Montero

Numerade Educator

01:55

Problem 24

What are the four basic steps involved in heterogeneous catalysis?

Eugene Schneider

University of Minnesota - Twin Cities

03:30

Problem 25

What are enzymes? What is the active site of an enzyme? What is
a substrate?

Ricajoy Montero

Numerade Educator

01:07

Problem 26

What is the general two-step mechanism by which most enzymes
work?

Eugene Schneider

University of Minnesota - Twin Cities

05:55

Problem 27

Consider the reaction.
a. Express the rate of the reaction in terms of the change in
concentration of each of the reactants and products.
b. In the first 25.0 s of this reaction, the concentration of HBr
drops from 0.600 M to 0.512 M. Calculate the average rate of
the reaction during this time interval.
c. If the volume of the reaction vessel in part b is 1.50 L, what
amount of Br2 (in moles) forms during the first 15.0 s of the
reaction?

Allison Krajewski

Numerade Educator

03:37

Problem 28

Consider the reaction.
a. Express the rate of the reaction in terms of the change in
concentration of each of the reactants and products.
b. In the first 15.0 s of the reaction, 0.015 mol of O2 is produced
in a reaction vessel with a volume of 0.500 L. What is the
average rate of the reaction during this time interval?
c. Predict the rate of change in the concentration of N2O during
this time interval. In other words, what is [N2O]>t?

Eugene Schneider

University of Minnesota - Twin Cities

04:42

Problem 29

For the reaction 2 A(g) + B(g)->3 C(g),
a. determine the expression for the rate of the reaction in terms
of the change in concentration of each of the reactants and
products.
b. when A is decreasing at a rate of 0.100 M>s, how fast is B
decreasing? How fast is C increasing?

Allison Krajewski

Numerade Educator

01:40

Problem 30

For the reaction A(g) + 12
B(g)->2 C(g),
a. determine the expression for the rate of the reaction in terms
of the change in concentration of each of the reactants and
products.
b. when C is increasing at a rate of 0.0025 M>s, how fast is B
decreasing? How fast is A decreasing?

Eugene Schneider

University of Minnesota - Twin Cities

04:58

Problem 31

Consider the reaction.
Complete the table.

Allison Krajewski

Numerade Educator

03:36

Problem 32

Consider the reaction.
Complete the table.

Eugene Schneider

University of Minnesota - Twin Cities

06:36

Problem 33

Consider the reaction:
The tabulated data were collected for the concentration of C4H8
as a function of time.
a. What is the average rate of the reaction between 0 and 10 s?
Between 40 and 50 s?
b. What is the rate of formation of C2H4 between 20 and 30 s?

Allison Krajewski

Numerade Educator

02:34

Problem 34

Consider the reaction.
The tabulated data were collected for the concentration of NO2 as
a function of time.
a. What is the average rate of the reaction between 10 and 20 s?
Between 50 and 60 s?
b. What is the rate of formation of O2 between 50 and 60 s?

Eugene Schneider

University of Minnesota - Twin Cities

08:19

Problem 35

Consider the reaction.
The graph shows the concentration of Br2 as a function of time.
a. Use the graph to calculate each quantity.
(i) the average rate of the reaction between 0 and 25 s
(ii) the instantaneous rate of the reaction at 25 s
(iii) the instantaneous rate of formation of HBr at 50 s
b. Make a rough sketch of a curve representing the concentration
of HBr as a function of time. Assume that the initial
concentration of HBr is zero.

Allison Krajewski

Numerade Educator

02:53

Problem 36

Consider the reaction.
The graph shows the concentration of H2O2 as a function of time.
a. Use the graph to calculate each quantity.
(i) the average rate of the reaction between 10 and 20 s
(ii) the instantaneous rate of the reaction at 30 s
(iii) the instantaneous rate of formation of O2 at 50 s
b. If the initial volume of the H2O2 is 1.5 L, what total amount of
O2 (in moles) is formed in the first 50 s of reaction?

Eugene Schneider

University of Minnesota - Twin Cities

03:15

Problem 37

This graph shows a plot of the rate of a reaction versus the
concentration of the reactant A for the reaction A->products.
a. What is the order of the reaction with respect to A?
b. Make a rough sketch of a plot of [A] versus time.
c. Write a rate law for the reaction including an estimate for the
value of k.

Allison Krajewski

Numerade Educator

02:10

Problem 38

This graph shows a plot of the rate of a reaction versus the
concentration of the reactant.
a. What is the order of the reaction with respect to A?
b. Make a rough sketch of a plot of [A] versus time.
c. Write a rate law for the reaction including the value of k.

Eugene Schneider

University of Minnesota - Twin Cities

02:47

Problem 39

What are the units of k for each type of reaction?
a. first-order reaction
b. second-order reaction
c. zero-order reaction

Allison Krajewski

Numerade Educator

02:11

Problem 40

This reaction is first order in N2O5:
The rate constant for the reaction at a certain temperature is
0.053>s.
a. Calculate the rate of the reaction when [N2O5] = 0.055 M.
b. What is the rate of the reaction at the concentration indicated
in part a if the reaction is second order? Zero order? (Assume
the same numerical value for the rate constant with the appropriate
units.)

Eugene Schneider

University of Minnesota - Twin Cities

05:13

Problem 41

A reaction in which A, B, and C react to form products is first
order in A, second order in B, and zero order in C.
a. Write a rate law for the reaction.
b. What is the overall order of the reaction?
c. By what factor does the reaction rate change if [A] is doubled
(and the other reactant concentrations are held constant)?
d. By what factor does the reaction rate change if [B] is doubled
(and the other reactant concentrations are held constant)?
e. By what factor does the reaction rate change if [C] is doubled
(and the other reactant concentrations are held constant)?
f. By what factor does the reaction rate change if the concentrations
of all three reactants are doubled?

Allison Krajewski

Numerade Educator

05:06

Problem 42

A reaction in which A, B, and C react to form products is zero
order in A, one-half order in B, and second order in C.
a. Write a rate law for the reaction.
b. What is the overall order of the reaction?
c. By what factor does the reaction rate change if [A] is doubled
(and the other reactant concentrations are held constant)?
d. By what factor does the reaction rate change if [B] is doubled
(and the other reactant concentrations are held constant)?
e. By what factor does the reaction rate change if [C] is doubled
(and the other reactant concentrations are held constant)?
f. By what factor does the reaction rate change if the concentrations
of all three reactants are doubled?

Eugene Schneider

University of Minnesota - Twin Cities

06:14

Problem 43

Consider the tabulated data showing the initial rate of a reaction
(A->products) at several different concentrations of A. What
is the order of the reaction? Write a rate law for the reaction
including the value of the rate constant, k.

Allison Krajewski

Numerade Educator

00:59

Problem 44

Eugene Schneider

University of Minnesota - Twin Cities

07:09

Problem 45

The tabulated data were collected for this reaction:
Write an expression for the reaction rate law and calculate the
value of the rate constant, k. What is the overall order of the
reaction?

Allison Krajewski

Numerade Educator

04:35

Problem 46

The tabulated data were collected for this reaction:
Write an expression for the reaction rate law and calculate the
value of the rate constant, k. What is the overall order of the
reaction?

Eugene Schneider

University of Minnesota - Twin Cities

03:46

Problem 47

Indicate the order of reaction consistent with each observation.
a. A plot of the concentration of the reactant versus time yields a
straight line.
b. The reaction has a half-life that is independent of initial
concentration.
c. A plot of the inverse of the concentration versus time yields a
straight line.

Ricajoy Montero

Numerade Educator

02:05

Problem 48

Indicate the order of reaction consistent with each observation.
a. The half-life of the reaction gets shorter as the initial concentration
is increased.
b. A plot of the natural log of the concentration of the reactant
versus time yields a straight line.
c. The half-life of the reaction gets longer as the initial concentration
is increased.

Eugene Schneider

University of Minnesota - Twin Cities

06:15

Problem 49

The tabulated data show the concentration of AB versus time for
this reaction:
Determine the order of the reaction and the value of the rate
constant. Predict the concentration of AB at 25 s.

David Collins

Numerade Educator

01:58

Problem 50

The tabulated data show the concentration of N2O5 versus time
for this reaction:
Determine the order of the reaction and the value of the rate
constant. Predict the concentration of N2O5 at 250 s.

Eugene Schneider

University of Minnesota - Twin Cities

04:45

Problem 51

The tabulated data show the concentration of cyclobutane (C4H8)
versus time for this reaction:
Determine the order of the reaction and the value of the rate
constant. What is the rate of reaction when [C4H8] = 0.25 M?

David Collins

Numerade Educator

01:04

Problem 52

A reaction in which A->products is monitored as a function
of time. The results are tabulated here.
Determine the order of the reaction and the value of the rate
constant. What is the rate of reaction when [A] = 0.10 M?

Eugene Schneider

University of Minnesota - Twin Cities

03:42

Problem 53

This reaction was monitored as a function of time:
A plot of ln[A] versus time yields a straight line with slope
-0.0045>s.
a. What is the value of the rate constant (k) for this reaction at
this temperature?
b. Write the rate law for the reaction.
c. What is the half-life?
d. If the initial concentration of A is 0.250 M, what is the
concentration after 225 s?

Oluwapelumi Kolawole

Numerade Educator

03:07

Problem 54

This reaction was monitored as a function of time:
A plot of 1>[AB] versus time yields a straight line with slope
-0.055>M # s.
a. What is the value of the rate constant (k) for this reaction at
this temperature?
b. Write the rate law for the reaction.
c. What is the half-life when the initial concentration is 0.55 M?
d. If the initial concentration of AB is 0.250 M, and the reaction
mixture initially contains no products, what are the concentrations
of A and B after 75 s?

Eugene Schneider

University of Minnesota - Twin Cities

01:46

Problem 55

The decomposition of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ is first order in $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ and has a rate constant of $1.42 \times 10^{-4} \mathrm{~s}^{-1}$ at a certain temperature.
a. What is the half-life for this reaction?
b. How long will it take for the concentration of $\$ O_{2} C l_{2}$ to decrease to $25 \%$ of its initial concentration?
c. If the initial concentration of $\$ O_{2} C l_{2}$ is $1.00 \mathrm{M}$, how long will it take for the concentration to decrease to $0.78 \mathrm{M} ?$
d. If the initial concentration of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ is $0.150 \mathrm{M}$, what is the concentration of $\$ \mathrm{SO}_{2} \mathrm{Cl}_{2}$ after $2.00 \times 10^{2} \mathrm{~s}$ ? After $5.00 \times 10^{2} \mathrm{~s}$ ?

David Collins

Numerade Educator

05:54

Problem 56

The decomposition of XY is second order in XY and has a rate
constant of 7.02 * 10-3 M-1 # s-1 at a certain temperature.
a. What is the half-life for this reaction at an initial concentration
of 0.100 M?
b. How long will it take for the concentration of XY to decrease
to 12.5% of its initial concentration when the initial concentration
is 0.100 M? When the initial concentration is 0.200 M?
c. If the initial concentration of XY is 0.150 M, how long will it
take for the concentration to decrease to 0.062 M?
d. If the initial concentration of XY is 0.050 M, what is the concentration
of XY after 5.0 * 101 s? After 5.50 * 102 s?

Eugene Schneider

University of Minnesota - Twin Cities

04:28

Problem 57

The half-life for the radioactive decay of U-238 is 4.5 billion years
and is independent of initial concentration. How long will it take
for 10% of the U-238 atoms in a sample of U-238 to decay? If a
sample of U-238 initially contained 1.5 * 1018 atoms when the
universe was formed 13.8 billion years ago, how many U-238
atoms does it contain today?

Ronald Prasad

Numerade Educator

04:35

Problem 58

The half-life for the radioactive decay of C-14 is 5730 years and is
independent of the initial concentration. How long does it take
for 25% of the C-14 atoms in a sample of C-14 to decay? If a
sample of C-14 initially contains 1.5 mmol of C-14, how many
millimoles are left after 2255 years?

Eugene Schneider

University of Minnesota - Twin Cities

02:26

Problem 59

The diagram shows the energy of a reaction as the reaction
progresses. Label each blank box in the diagram.
a. reactants b. products
c. activation energy (Ea) d. enthalpy of reaction (Hrxn)

Ricajoy Montero

Numerade Educator

01:07

Problem 60

A chemical reaction is endothermic and has an activation energy
that is twice the value of the enthalpy change of the reaction.
Draw a diagram depicting the energy of the reaction as it
progresses. Label the position of the reactants and products and
indicate the activation energy and enthalpy of reaction.

Eugene Schneider

University of Minnesota - Twin Cities

02:45

Problem 61

The activation energy of a reaction is 56.8 kJ>mol and the
frequency factor is 1.5 * 1011>s. Calculate the rate constant of
the reaction at 25 C.

Ricajoy Montero

Numerade Educator

02:36

Problem 62

The rate constant of a reaction at 32 C is 0.055>s. If the
frequency factor is 1.2 * 1013>s, what is the activation barrier?

Eugene Schneider

University of Minnesota - Twin Cities

03:03

Problem 63

The rate constant (k) for a reaction is measured as a function of
temperature. A plot of ln k versus 1>T (in K) is linear and has a
slope of -7445 K. Calculate the activation energy for the reaction.

Ricajoy Montero

Numerade Educator

01:55

Problem 64

The rate constant (k) for a reaction is measured as a function of
temperature. A plot of ln k versus 1>T (in K) is linear and has a slope of -1.01 * 104 K. Calculate the activation energy for the
reaction.

Eugene Schneider

University of Minnesota - Twin Cities

05:07

Problem 65

The tabulated data shown here were collected for the first-order
reaction:
Use an Arrhenius plot to determine the activation barrier and
frequency factor for the reaction.

David Collins

Numerade Educator

02:33

Problem 66

The tabulated data show the rate constant of a reaction measured at several different temperatures. Use an Arrhenius plot to determine the activation barrier and frequency factor for the reaction.

Eugene Schneider

University of Minnesota - Twin Cities

05:10

Problem 67

The tabulated data were collected for the second-order reaction:
Use an Arrhenius plot to determine the activation barrier and
frequency factor for the reaction.

David Collins

Numerade Educator

02:57

Problem 68

The tabulated data show the rate constant of a reaction measured
at several different temperatures. Use an Arrhenius plot to determine
the activation barrier and frequency factor for the reaction.

Eugene Schneider

University of Minnesota - Twin Cities

09:32

Problem 69

A reaction has a rate constant of 0.0117>s at 400.0 K and 0.689>s
at 450.0 K.
a. Determine the activation barrier for the reaction.
b. What is the value of the rate constant at 425 K?

Ricajoy Montero

Numerade Educator

03:32

Problem 70

A reaction has a rate constant of 0.000122>s at 27 C and 0.228>s
at 77 C.
a. Determine the activation barrier for the reaction.
b. What is the value of the rate constant at 17 C?

Eugene Schneider

University of Minnesota - Twin Cities

04:48

Problem 71

If a temperature increase from 10.0 C to 20.0 C doubles the rate
constant for a reaction, what is the value of the activation barrier
for the reaction?

Ricajoy Montero

Numerade Educator

02:05

Problem 72

If a temperature increase from 20.0 C to 35.0 C triples the rate
constant for a reaction, what is the value of the activation barrier
for the reaction?

Eugene Schneider

University of Minnesota - Twin Cities

02:57

Problem 73

Consider these two gas-phase reactions:
a. AA(g) + BB(g)->2 AB(g)
b. AB(g) + CD(g)->AC(g) + BD(g)
If the reactions have identical activation barriers and are carried
out under the same conditions, which one would you expect to
have the faster rate?

Ricajoy Montero

Numerade Educator

03:21

Problem 74

Which of these two reactions would you expect to have the
smaller orientation factor? Explain.
a. O(g) + N2(g)->NO(g) + N(g)
b. NO(g) + Cl2(g)->NOCl(g) + Cl(g)

Eugene Schneider

University of Minnesota - Twin Cities

03:45

Problem 75

Consider this overall reaction, which is experimentally observed
to be second order in AB and zero order in C:

Is the following mechanism valid for this reaction?

Ricajoy Montero

Numerade Educator

06:39

Problem 76

Consider this overall reaction, which is experimentally observed
to be second order in X and first order in Y:
a. Does the reaction occur in a single step in which X and Y
collide?
b. Is this two-step mechanism valid?

Eugene Schneider

University of Minnesota - Twin Cities

08:42

Problem 77

Consider this three-step mechanism for a reaction:
a. What is the overall reaction?
b. Identify the intermediates in the mechanism.
c. What is the predicted rate law?

Ricajoy Montero

Numerade Educator

02:16

Problem 78

Consider this two-step mechanism for a reaction:
a. What is the overall reaction?
b. Identify the intermediates in the mechanism.
c. What is the predicted rate law?

Eugene Schneider

University of Minnesota - Twin Cities

02:41

Problem 79

Many heterogeneous catalysts are deposited on high surface-area
supports. Why?

Ricajoy Montero

Numerade Educator

01:32

Problem 80

Suppose that the reaction A->products is exothermic and
has an activation barrier of 75 kJ>mol. Sketch an energy diagram
showing the energy of the reaction as a function of the progress
of the reaction. Draw a second energy curve showing the effect of
a catalyst.

Eugene Schneider

University of Minnesota - Twin Cities

04:14

Problem 81

Suppose that a catalyst lowers the activation barrier of a reaction
from 125 kJ >mol to 55 kJ >mol. By what factor would you
expect the reaction rate to increase at 25 C? (Assume that the
frequency factors for the catalyzed and uncatalyzed reactions
are identical.)

Ricajoy Montero

Numerade Educator

02:42

Problem 82

The activation barrier for the hydrolysis of sucrose into glucose
and fructose is 108 kJ>mol. If an enzyme increases the rate of the
hydrolysis reaction by a factor of 1 million, how much lower
must the activation barrier be when sucrose is in the active site of
the enzyme? (Assume that the frequency factors for the catalyzed
and uncatalyzed reactions are identical and a temperature of
25 C.)

Eugene Schneider

University of Minnesota - Twin Cities

06:16

Problem 83

The tabulated data were collected for this reaction at 500 C:
a. Determine the order of the reaction and the value of the rate
constant at this temperature.
b. What is the half-life for this reaction (at the initial
concentration)?
c. How long will it take for 90% of the CH3CN to convert to
CH3NC?

David Collins

Numerade Educator

04:04

Problem 84

The tabulated data were collected for this reaction at a certain
temperature:
a. Determine the order of the reaction and the value of the rate
constant at this temperature.
b. What is the half-life for this reaction (at the initial
concentration)?
c. What is the concentration of X after 10.0 hours?

Eugene Schneider

University of Minnesota - Twin Cities

03:45

Problem 85

Consider the reaction:
The rate law for this reaction is:
Suppose the rate of the reaction at certain initial concentrations
of A, B, and C is 0.0115 M>s. What is the rate of the reaction if
the concentrations of A and C are doubled and the concentration
of B is tripled?

Ricajoy Montero

Numerade Educator

04:04

Problem 86

Consider the reaction:
The rate law for this reaction is:
Suppose that a 1.0 L reaction vessel initially contains 1.0 mol of
O3 and 1.0 mol of O2. What fraction of the O3 has reacted when
the rate falls to one-half of its initial value?

Eugene Schneider

University of Minnesota - Twin Cities

08:37

Problem 87

At 700 K acetaldehyde decomposes in the gas phase to methane
and carbon monoxide. The reaction is:
A sample of CH3CHO is heated to 700 K, and the pressure is
measured as 0.22 atm before any reaction takes place. The
kinetics of the reaction are followed by measurements of total
pressure, and these data are obtained:
Determine the rate law, the rate constant, and the total pressure
after 2.00 * 104 s.

David Collins

Numerade Educator

02:46

Problem 88

At 400 K oxalic acid decomposes according to the reaction:
In three separate experiments, the initial pressure of oxalic acid
and the final total pressure after 20,000 s are measured.
Find the rate law of the reaction and its specific rate constant.

Eugene Schneider

University of Minnesota - Twin Cities

04:35

Problem 89

Dinitrogen pentoxide decomposes in the gas phase to form
nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen
pentoxide and has a half-life of 2.81 h at 25 C. If a 1.5 L
reaction vessel initially contains 745 torr of N2O5 at 25 C, what
partial pressure of O2 is present in the vessel after 215 minutes?

David Collins

Numerade Educator

02:46

Problem 90

Cyclopropane (C3H6) reacts to form propene (C3H6) in the gas
phase. The reaction is first order in cyclopropane and has a rate
constant of 5.87 * 10-4>s at 485 C. If a 2.5 L reaction vessel
initially contains 722 torr of cyclopropane at 485 C, how long will
it take for the partial pressure of cyclopropane to drop to below
1.00 * 102 torr?

Eugene Schneider

University of Minnesota - Twin Cities

01:16

Problem 91

Iodine atoms combine to form I2 in liquid hexane solvent with a
rate constant of 1.5 * 1010 L>mol # s. The reaction is second
order in I. Since the reaction occurs so quickly, the only way to
study the reaction is to create iodine atoms almost instantaneously,
usually by photochemical decomposition of I2. Suppose
a flash of light creates an initial [I] concentration of 0.0100 M.
How long will it take for 95% of the newly created iodine atoms
to recombine to form I2?

David Collins

Numerade Educator

03:35

Problem 92

The hydrolysis of sucrose (C12H22O11) into glucose and fructose
in acidic water has a rate constant of 1.8 * 10-4 s-1 at 25 C.
Assuming the reaction is first order in sucrose, determine the
mass of sucrose that is hydrolyzed when 2.55 L of a 0.150 M
sucrose solution is allowed to react for 195 minutes.

Eugene Schneider

University of Minnesota - Twin Cities

05:26

Problem 93

The reaction AB(aq)->A(g) + B(g) is second order in AB and
has a rate constant of 0.0118 M-1 # s-1 at 25.0 C. A reaction vessel
initially contains 250.0 mL of 0.100 M AB that is allowed to react
to form the gaseous product. The product is collected over water
at 25.0 C. How much time is required to produce 200.0 mL of
the products at a barometric pressure of 755.1 mmHg? (The vapor
pressure of water at this temperature is 23.8 mmHg.)

David Collins

Numerade Educator

04:21

Problem 94

The reaction 2 H2O2(aq)->2 H2O(l) + O2(g) is first order
in H2O2 and under certain conditions has a rate constant of
0.00752 s-1 at 20.0 C. A reaction vessel initially contains
150.0mL of 30.0% H2O2 by mass solution (the density of the
solution is 1.11 g >mL). The gaseous oxygen is collected over
water at 20.0 C as it forms. What volume of O2 forms in
85.0 seconds at a barometric pressure of 742.5 mmHg? (The
vapor pressure of water at this temperature is 17.5 mmHg.)

Eugene Schneider

University of Minnesota - Twin Cities

03:57

Problem 95

Consider this energy diagram:
a. How many elementary steps are involved in this reaction?
b. Label the reactants, products, and intermediates.
c. Which step is rate limiting?
d. Is the overall reaction endothermic or exothermic?

Ricajoy Montero

Numerade Educator

02:53

Problem 96

Consider the reaction in which HCl adds across the double bond
of ethene:
The following mechanism, with the accompanying energy
diagram, has been suggested for this reaction:
a. Based on the energy diagram, determine which step is rate
limiting.
b. What is the expected order of the reaction based on the
proposed mechanism?
c. Is the overall reaction exothermic or endothermic?

Eugene Schneider

University of Minnesota - Twin Cities

02:43

Problem 97

The desorption of a single molecular layer of n-butane from a
single crystal of aluminum oxide is found to be first order with a
rate constant of 0.128>s at 150 K.
a. What is the half-life of the desorption reaction?
b. If the surface is initially completely covered with n-butane at
150 K, how long will it take for 25% of the molecules to
desorb? For 50% to desorb?
c. If the surface is initially completely covered, what fraction
will remain covered after 10 s? After 20 s?

David Collins

Numerade Educator

01:42

Problem 98

The evaporation of a 120-nm film of n-pentane from a single
crystal of aluminum oxide is zero order with a rate constant of
1.92 * 1013 molecules>cm2 # s at 120 K.
a. If the initial surface coverage is 8.9 * 1016 molecules>cm2,
how long will it take for one-half of the film to evaporate?
b. What fraction of the film is left after 10 s? Assume the same
initial coverage as in part a.

Eugene Schneider

University of Minnesota - Twin Cities

06:10

Problem 99

The kinetics of this reaction were studied as a function of temperature.
(The reaction is first order in each reactant and second
order overall.)
a. Determine the activation energy and frequency factor for the
reaction.
b. Determine the rate constant at 15 C.
c. If a reaction mixture is 0.155 M in C2H5Br and 0.250 M in
OH-, what is the initial rate of the reaction at 75 C?

David Collins

Numerade Educator

02:12

Problem 100

The reaction 2 N2O5->2 N2O4 + O2 takes place at around
room temperature in solvents such as CCl4. The rate constant at
293 K is 2.35 * 10-4 s-1, and at 303 K the rate constant is
9.15 * 10-4 s-1. Calculate the frequency factor for the reaction.

Eugene Schneider

University of Minnesota - Twin Cities

04:48

Problem 101

This reaction has an activation energy of zero in the gas phase:
a. Would you expect the rate of this reaction to change very
much with temperature?
b. Why might the activation energy be zero?
c. What other types of reactions would you expect to have little
or no activation energy?

Ricajoy Montero

Numerade Educator

02:04

Problem 102

Consider the two reactions:
a. Why is the activation barrier for the first reaction so much
higher than that for the second?
b. The frequency factors for these two reactions are very close
to each other in value. Assuming that they are the same,
calculate the ratio of the reaction rate constants for these two
reactions at 25 C.

Eugene Schneider

University of Minnesota - Twin Cities

05:36

Problem 103

Anthropologists can estimate the age of a bone or other sample of
organic matter by its carbon-14 content. The carbon-14 in a living
organism is constant until the organism dies, after which carbon-14
decays with first-order kinetics and a half-life of 5730 years.
Suppose a bone from an ancient human contains 19.5% of the C-14
found in living organisms. How old is the bone?

Ricajoy Montero

Numerade Educator

02:18

Problem 104

Geologists can estimate the age of rocks by their uranium-238
content. The uranium is incorporated in the rock as it hardens
and then decays with first-order kinetics and a half-life of
4.5 billion years. A rock contains 83.2% of the amount of
uranium-238 that it contained when it was formed. (The amount
that the rock contained when it was formed can be deduced from
the presence of the decay products of U-238.) How old is the rock?

Eugene Schneider

University of Minnesota - Twin Cities

03:53

Problem 105

Consider the gas-phase reaction:
The reaction was experimentally determined to be first order in
H2 and first order in I2. Consider the proposed mechanisms.
Proposed mechanism I:
Proposed mechanism II:
a. Show that both of the proposed mechanisms are valid.
b. What kind of experimental evidence might lead you to favor
mechanism II over mechanism I?

Ricajoy Montero

Numerade Educator

04:42

Problem 106

Consider the reaction:
This three-step mechanism is proposed:
a. Show that the mechanism sums to the overall reaction.
b. What is the rate law predicted by this mechanism?

Eugene Schneider

University of Minnesota - Twin Cities

07:18

Problem 107

The proposed mechanism for the formation of hydrogen bromide
can be written in a simplified form as:
What rate law corresponds to this mechanism?

Ricajoy Montero

Numerade Educator

03:37

Problem 108

A proposed mechanism for the formation of hydrogen iodide can
be written in simplified form as:
What rate law corresponds to this mechanism?

Eugene Schneider

University of Minnesota - Twin Cities

03:25

Problem 109

A certain substance X decomposes. Fifty percent of X remains
after 100 minutes. How much X remains after 200 minutes if the
reaction order with respect to X is (a) zero order, (b) first order,
(c) second order?

Prashant Bana

Numerade Educator

01:58

Problem 110

The half-life for radioactive decay (a first-order process) of
plutonium-239 is 24,000 years. How many years does it take for
one mole of this radioactive material to decay until just one atom
remains?

Eugene Schneider

University of Minnesota - Twin Cities

05:25

Problem 111

The energy of activation for the decomposition of 2 mol of HI to
H2 and I2 in the gas phase is 185 kJ. The heat of formation of
HI(g) from H2(g) and I2(g) is -5.68 kJ>mol. Find the energy of
activation for the reaction of 1 mol of H2 and 1 mol of I2 to form
2mol of HI in the gas phase.

Ricajoy Montero

Numerade Educator

03:29

Problem 112

Ethyl chloride vapor decomposes by the first-order reaction:
The activation energy is 249 kJ>mol, and the frequency factor is
1.6 * 1014 s-1. Find the value of the specific rate constant at
710K. What fraction of the ethyl chloride decomposes in
15minutes at this temperature? Find the temperature at which
the rate of the reaction would be twice as fast.

Eugene Schneider

University of Minnesota - Twin Cities

05:09

Problem 113

In this chapter we have seen a number of reactions in which a
single reactant forms products. For example, consider the following
first-order reaction:
However, we also learned that gas-phase reactions occur through
collisions.
a. One possible explanation is that two molecules of CH3NC
collide with each other and form two molecules of the product
in a single elementary step. If that is the case, what reaction
order would you expect?
b. Another possibility is that the reaction occurs through more
than one step. For example, a possible mechanism involves
one step in which the two CH3NC molecules collide, resulting
in the 'activation' of one of them. In a second step, the activated
molecule goes on to form the product. Write down this
mechanism and determine which step must be rate determining
in order for the kinetics of the reaction to be first order.
Show explicitly how the mechanism predicts first-order
kinetics.

David Collins

Numerade Educator

03:55

Problem 114

The first-order integrated rate law for a reaction A->products
is derived from the rate law using calculus:
The equation just given is a first-order, separable differential
equation that can be solved by separating the variables and
integrating:
In the integral just given, [A]0 is the initial concentration of A.
We then evaluate the integral:
a. Use a procedure similar to the one just shown to derive an
integrated rate law for a reaction A->products, which is
one-half-order in the concentration of A (that is,
Rate = k[A]1>2).
b. Use the result from part a to derive an expression for the halflife
of a one-half-order reaction.

Eugene Schneider

University of Minnesota - Twin Cities

05:09

Problem 115

The previous exercise shows how the first-order integrated rate
law is derived from the first-order differential rate law. Begin
with the second-order differential rate law and derive the
second-order integrated rate law.

Ricajoy Montero

Numerade Educator

05:20

Problem 116

The rate constant for the first-order decomposition of N2O5(g) to
NO2(g) and O2(g) is 7.48 * 10-3 s-1 at a given temperature.
a. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.100 atm to
rise to 0.145 atm.
b. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.100 atm to
rise to 0.200 atm.
c. Find the total pressure after 100 s of reaction.

David Collins

Numerade Educator

05:14

Problem 117

Phosgene (Cl2CO), a poison gas used in World War I, is formed
by the reaction of Cl2 and CO. The proposed mechanism for the
reaction is:
What rate law is consistent with this mechanism?

Nicholas Mogoi

Numerade Educator

02:06

Problem 118

The rate of decomposition of N2O3(g) to NO2(g) and NO(g) is
monitored by measuring [NO2] at different times. The following
tabulated data are obtained.
The reaction follows a first-order rate law. Calculate the rate
constant. Assume that after 50,000 s all the N2O3(g) had
decomposed.

Eugene Schneider

University of Minnesota - Twin Cities

05:02

Problem 119

At 473 K, for the elementary reaction 2 NOCl(g) k1
k-1
2 NO(g) + Cl2(g)
A sample of NOCl is placed in a container and heated to 473 K.
When the system comes to equilibrium, [NOCl] is found to be
0.12 mol>L. What are the concentrations of NO and Cl2?

David Collins

Numerade Educator

01:49

Problem 120

Consider the reaction:
The reaction is first order in CHCl3 and one-half order in Cl2. Which
reaction mixture would you expect to have the fastest initial rate?

Eugene Schneider

University of Minnesota - Twin Cities

03:25

Problem 121

The accompanying graph shows the concentration of a reactant as
a function of time for two different reactions. One of the reactions
is first order and the other is second order. Which of the two
reactions is first order? Second order? How would you change
each plot to make it linear?

Ricajoy Montero

Numerade Educator

02:34

Problem 122

A particular reaction, A->products, has a rate that slows down
as the reaction proceeds. The half-life of the reaction is found to
depend on the initial concentration of A. Determine whether each
statement is likely to be true or false for this reaction.
a. A doubling of the concentration of A doubles the rate of the
reaction.
b. A plot of 1>[A] versus time is linear.
c. The half-life of the reaction gets longer as the initial
concentration of A increases.
d. A plot of the concentration of A versus time has a constant
slope.

Eugene Schneider

University of Minnesota - Twin Cities

02:14

Problem 123

A student says, 'The initial concentration of a reactant was doubled,
and the rate doubled. Therefore, the reaction is second
order in that reactant.'Why might the student say that? What is
wrong with the statement? What is the actual order with respect
to the reactant? Explain your reasoning clearly.

Prashant Bana

Numerade Educator

04:48

Problem 124

A certain compound, A, reacts to form products according to the
reaction A->P. The amount of A is measured as a function of
time under a variety of different conditions and the tabulated
results are shown here:
Have one group member make a graph of [A] versus t, one group
member make a graph of ln[A] versus t, and one group member
make a graph of 1>[A] versus t using the data for 25 C.
Additional group members can make similar graphs for the other
temperatures. What is the order of the reaction with respect to
A? Explain your answer.
a. Use the data to determine the rate constant at each
temperature.
b. What is the activation energy for this reaction?
c. The same reaction is conducted in the presence of a catalyst,
and the following data are obtained:
What effect does a catalyst have on the rate of the reaction? What
is the activation energy for this reaction in the presence of the
catalyst? How does it compare with the activation energy for the
reaction when the catalyst isn"t present?

Eugene Schneider

University of Minnesota - Twin Cities

09:39

Problem 125

Methane (CH4) is a greenhouse gas emitted by industry, agriculture,
and waste systems. It is the second most prevalent greenhouse
gas (after carbon dioxide). Methane plays an important
role in climate change because it absorbs infrared radiation more
efficiently than carbon dioxide. Methane is broken down in the
atmosphere by ozone (O3), making its atmospheric lifetime
shorter than that of carbon dioxide.
A research group studied the rate of the reaction by which
methane reacts with ozone and gets the data shown in the tables
shown here. Study the data and answer the questions that follow.
a. Use the data in the first table to determine the order of the
reaction with respect to each reactant.
b. Use the data in the second table to determine the activation
barrier and pre-exponential factor for the reaction.
c. Atmospheric concentrations of methane and ozone can vary
depending on the location and altitude. Calculate the rate of
the reaction at 273 K for a methane concentration of 1.8 ppm
(by volume) and an ozone concentration of 5.0 ppm (by
volume). Note that 1 ppm of CH4 by volume means 1 L
CH4>106 L air. Assume STP (standard temperature and
pressure) so that 1 mol gas occupies 22.4 L.
d. What is the half-life of methane in the atmosphere in years at
323 K? (Assume that [CH4] = [O3] = [A]0 = 5.0 * 10-7 M.)

David Collins

Numerade Educator