Question 1

The half-life of a second-order reaction under a given set of reaction conditions is a constant.

Accepted Answer

A) True 
 B)False  False

Question 2

A _____ order reaction is one whose rate is independent of concentration.

Accepted Answer

A)  first 
B)  third 
C)  last 
D)  second 
E)  zeroth 
A)  first 
B)  third 
C)  last 
D)  second 
E)  zeroth E

Question 3

Calculate the reaction rate of SO2(g) in the following reaction, using the data provided in the following table. $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})$$\rightarrow$$2 \mathrm{SO}_{3}(\mathrm{~g})$

$\begin{array}{|l|l|l|l|}
\hline   \text { Time(s) } &{\left[\mathrm{SO}_{2}\right](\mathrm{M})} & {\left[\mathrm{O}_{2}\right](\mathrm{M})} & {\left[\mathrm{SO}_{3}\right](\mathrm{M})} \
\hline 200 & 0.0235 & 0.0520 & 0.0100 \
\hline 520 & 0.0146 & 0.0410 & 0.0208 \
\hline
\end{array}$

Accepted Answer

A)  5.7 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
B)  2.5 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
C)  4.3 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
D)  1.3 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
E)  3.8 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
A)  5.7 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
B)  2.5 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
C)  4.3 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
D)  1.3 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ 
E)  3.8 $\times 10 ^ { - 6 } \mathrm { M } / \mathrm { S }$ D

Question 4

Radicals are species that have one or more unpaired valence electrons.

Accepted Answer

A) True 
 B)False

Question 5

Which of the following is true of zeroth-order reactions?

Accepted Answer

A)  The rate is dependent on the reactant concentration. 
B)  The differential rate law is rate = k. 
C)  The graph of the reactant concentration as a function of time is a straight line with slope of k. 
D)  It can be written in a form such that the exponent of the reactant in the rate law is 1. 
E)  The graph of the product concentration as a function of time is a straight line with slope of -k. 
A)  The rate is dependent on the reactant concentration. 
B)  The differential rate law is rate = k. 
C)  The graph of the reactant concentration as a function of time is a straight line with slope of k. 
D)  It can be written in a form such that the exponent of the reactant in the rate law is 1. 
E)  The graph of the product concentration as a function of time is a straight line with slope of -k.

Question 6

The following graph represents the straight-line plot to determine the rate constant of a _____-order reaction.

Accepted Answer

A)  first 
B)  fourth 
C)  second 
D)  zeroth 
E)  third 
A)  first 
B)  fourth 
C)  second 
D)  zeroth 
E)  third

Question 7

A graph of the concentration of any reactant as a function of time is a straight line with a slope of k.

Accepted Answer

A) True 
 B)False

Question 8

The general rate law for a unimolecular elementary reaction (A → products) is rate = k[A].

Accepted Answer

A) True 
 B)False

Question 9

The rate of radioactive decay is dependent on temperature.

Accepted Answer

A) True 
 B)False

Question 10

A(n)_____ rate law describes the reaction rate in terms of the initial concentration and the measured concentration of one or more reactants after a given amount of time.

Accepted Answer

A)  homogeneous 
B)  degenerate 
C)  differential 
D)  heterogeneous 
E)  integrated 
A)  homogeneous 
B)  degenerate 
C)  differential 
D)  heterogeneous 
E)  integrated

Question 11

The rate law for a reaction can be obtained from the overall balanced chemical equation alone.

Accepted Answer

A) True 
 B)False

Question 12

Irreversible inhibitors are therefore the equivalent of _____ in heterogeneous catalysis.

Accepted Answer

The answer of Irreversible inhibitors are therefore the equivalent of...

Question 13

Which heterogeneous catalyst is used in steam reforming?

Accepted Answer

A)  Ni 
B)  Fe 
C)  Cu 
D)  Pd 
E)  Rh 
A)  Ni 
B)  Fe 
C)  Cu 
D)  Pd 
E)  Rh

Question 14

The following is an example of a first-order reaction involving the _____.

Accepted Answer

A)  reaction of t-butyl bromide with water to give t-butanol 
B)  hydrolysis of the anticancer drug cisplatin 
C)  oxidation of ethanol to acetaldehyde in the liver 
D)  decomposition of N2O on a platinum surface 
E)  hydrolysis of aspirin 
A)  reaction of t-butyl bromide with water to give t-butanol 
B)  hydrolysis of the anticancer drug cisplatin 
C)  oxidation of ethanol to acetaldehyde in the liver 
D)  decomposition of N2O on a platinum surface 
E)  hydrolysis of aspirin

Question 15

Differential rate laws are generally used to describe what is occurring on a molecular level during a reaction.

Accepted Answer

A) True 
 B)False

Question 16

The reaction rate of a heterogeneous reaction depends on the surface area of the more condensed phase.

Accepted Answer

A) True 
 B)False

Question 17

Which of the following best describes chemical kinetics?

Accepted Answer

A)  It is the enthalpy change that occurs when a solid ionic compound is transformed into gaseous ions. 
B)  It is the process of converting one element to another. 
C)  It is a methodology that combines chemical reactions and stoichiometric calculations to determine the concentrations of substances present in a sample. 
D)  It is the study of reaction rates, the changes in the concentrations of reactants and products with time. 
E)  It is a complete description of the system at a given time, including its temperature and pressure, the amount of matter it contains, its chemical composition, and the physical state of the matter. 
A)  It is the enthalpy change that occurs when a solid ionic compound is transformed into gaseous ions. 
B)  It is the process of converting one element to another. 
C)  It is a methodology that combines chemical reactions and stoichiometric calculations to determine the concentrations of substances present in a sample. 
D)  It is the study of reaction rates, the changes in the concentrations of reactants and products with time. 
E)  It is a complete description of the system at a given time, including its temperature and pressure, the amount of matter it contains, its chemical composition, and the physical state of the matter.

Question 18

Reaction rates generally decrease with time as reactant concentrations increase.

Accepted Answer

A) True 
 B)False

Question 19

A compound hydrolyzes in water with a rate constant of $1.9 \times 10 ^ { - 3 } \mathrm {~min} ^ { - 1 }$ at pH 6.0 and $26 ^{?}\mathrm { C }$ . The half-life for this reaction is _____ min.

Accepted Answer

A)  $3.6 \times 10 ^ { 2 }$ 
B)  $5.1 \times 10 ^ { 2 }$ 
C)  $4.8 \times 10 ^ { 2 }$ 
D)  $6.5 \times 10 ^ { 2 }$ 
E)  $2.9 \times 10 ^ { 2 }$ 
A)  $3.6 \times 10 ^ { 2 }$ 
B)  $5.1 \times 10 ^ { 2 }$ 
C)  $4.8 \times 10 ^ { 2 }$ 
D)  $6.5 \times 10 ^ { 2 }$ 
E)  $2.9 \times 10 ^ { 2 }$

Question 20

Which of the following feature is true about catalysts?

Accepted Answer

A)  Catalysts appear in the overall stoichiometry of the reaction being catalyzed. 
B)  The reaction rate of a catalyzed reaction is slower than the reaction rate of the uncatalyzed reaction at the same temperature. 
C)  Catalysts increase the reaction rate of a chemical reaction by being consumed in the process. 
D)  The net change in energy that results from a reaction is affected by the presence of a catalyst. 
E)  Catalysts increase the reaction rates of both the forward and the reverse reactions by the same amount. 
A)  Catalysts appear in the overall stoichiometry of the reaction being catalyzed. 
B)  The reaction rate of a catalyzed reaction is slower than the reaction rate of the uncatalyzed reaction at the same temperature. 
C)  Catalysts increase the reaction rate of a chemical reaction by being consumed in the process. 
D)  The net change in energy that results from a reaction is affected by the presence of a catalyst. 
E)  Catalysts increase the reaction rates of both the forward and the reverse reactions by the same amount.

Exam 14: Chemical Kinetics

The half-life of a second-order reaction under a given set of reaction conditions is a constant.

A _____ order reaction is one whose rate is independent of concentration.

Radicals are species that have one or more unpaired valence electrons.

Which of the following is true of zeroth-order reactions?

The following graph represents the straight-line plot to determine the rate constant of a _____-order reaction.

A graph of the concentration of any reactant as a function of time is a straight line with a slope of k.

The general rate law for a unimolecular elementary reaction (A → products) is rate = k[A].

The rate of radioactive decay is dependent on temperature.

A(n)_____ rate law describes the reaction rate in terms of the initial concentration and the measured concentration of one or more reactants after a given amount of time.

The rate law for a reaction can be obtained from the overall balanced chemical equation alone.

Irreversible inhibitors are therefore the equivalent of _____ in heterogeneous catalysis.

Which heterogeneous catalyst is used in steam reforming?

The following is an example of a first-order reaction involving the _____.

Differential rate laws are generally used to describe what is occurring on a molecular level during a reaction.

The reaction rate of a heterogeneous reaction depends on the surface area of the more condensed phase.

Which of the following best describes chemical kinetics?

Reaction rates generally decrease with time as reactant concentrations increase.

A compound hydrolyzes in water with a rate constant of 1.9×10−3 min−11.9 \times 10 ^ { - 3 } \mathrm {~min} ^ { - 1 }1.9×10−3 min−1 at pH 6.0 and 26?C26 ^{?}\mathrm { C }26?C . The half-life for this reaction is _____ min.

Which of the following feature is true about catalysts?

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Gases

Liquids

Solids

Solutions

Chemical Equilibrium

Aqueous Acidbase Equilibriums

Solubility and Complexation Equilibriums

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Periodic Trends and the S-Block Elements

The P-Block Elements

The D-Block Elements

Organic Compounds

Filters

A compound hydrolyzes in water with a rate constant of $1.9 \times 10 ^ { - 3 } \mathrm {~min} ^ { - 1 }$ at pH 6.0 and $26 ^{?}\mathrm { C }$ . The half-life for this reaction is _____ min.