Question 1

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if Ea = 55.3 kJ/mol?

Accepted Answer

A) 2.24 × 104 
B) 3.34 × 103 
C) 433 
D) 2.49 × 106 
E) 1.35 × 102 
A) 2.24 × 104 
B) 3.34 × 103 
C) 433 
D) 2.49 × 106 
E) 1.35 × 102

Question 2

The data in the table below were obtained for the reaction:
A + B → P  
-The rate law for this reaction is rate = ________.

Accepted Answer

A) k[A][B] 
B) k[P] 
C) k[A]2[B] 
D) k[A]2[B]2 
E) k[A]2 
A) k[A][B] 
B) k[P] 
C) k[A]2[B] 
D) k[A]2[B]2 
E) k[A]2

Question 3

The rate law of a reaction is rate = k[D][X]. The units of the rate constant are ________.

Accepted Answer

A) mol L-1s-1 
B) L mol-1s-1 
C) mol2 L-2s-1 
D) mol L-1s-2 
E) L2 mol-2s-1 
A) mol L-1s-1 
B) L mol-1s-1 
C) mol2 L-2s-1 
D) mol L-1s-2 
E) L2 mol-2s-1

Question 4

A burning splint will burn more vigorously in pure oxygen than in air because ________.

Accepted Answer

A) oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than is in air 
B) oxygen is a catalyst for combustion 
C) oxygen is a product of combustion 
D) nitrogen is a product of combustion and the system reaches equilibrium at a lower temperature 
E) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the combustion 
A) oxygen is a reactant in combustion and concentration of oxygen is higher in pure oxygen than is in air 
B) oxygen is a catalyst for combustion 
C) oxygen is a product of combustion 
D) nitrogen is a product of combustion and the system reaches equilibrium at a lower temperature 
E) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the combustion

Question 5

One difference between first- and second-order reactions is that ________.

Accepted Answer

A) the half-life of a first-order reaction does not depend on [A]0; the half-life of a second-order reaction does depend on [A]0 
B) the rate of both first-order and second-order reactions do not depend on reactant concentrations 
C) the rate of a first-order reaction depends on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations 
D) a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed 
E) None of the above are true. 
A) the half-life of a first-order reaction does not depend on [A]0; the half-life of a second-order reaction does depend on [A]0 
B) the rate of both first-order and second-order reactions do not depend on reactant concentrations 
C) the rate of a first-order reaction depends on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations 
D) a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed 
E) None of the above are true.

Question 6

Which of the following is true?

Accepted Answer

A) If we know that a reaction is an elementary reaction, then we know its rate law. 
B) The rate-determining step of a reaction is the rate of the fastest elementary step of its mechanism. 
C) Since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process. 
D) In a reaction mechanism, an intermediate is identical to an activated complex. 
E) All of the above statements are true. 
A) If we know that a reaction is an elementary reaction, then we know its rate law. 
B) The rate-determining step of a reaction is the rate of the fastest elementary step of its mechanism. 
C) Since intermediate compounds can be formed, the chemical equations for the elementary reactions in a multistep mechanism do not always have to add to give the chemical equation of the overall process. 
D) In a reaction mechanism, an intermediate is identical to an activated complex. 
E) All of the above statements are true.

Question 7

As the temperature of a reaction is increased, the rate of the reaction increases because the ________.

Accepted Answer

A) reactant molecules collide less frequently 
B) reactant molecules collide more frequently and with greater energy per collision 
C) activation energy is lowered 
D) reactant molecules collide less frequently and with greater energy per collision 
E) reactant molecules collide more frequently with less energy per collision 
A) reactant molecules collide less frequently 
B) reactant molecules collide more frequently and with greater energy per collision 
C) activation energy is lowered 
D) reactant molecules collide less frequently and with greater energy per collision 
E) reactant molecules collide more frequently with less energy per collision

Question 8

The reaction A → B is first order in [A]. Consider the following data.  
-The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1.

Accepted Answer

A) 0.693 
B) 1.65 × 10-2 
C) 1.98 
D) 0.198 
E) 3.30 ×10-3 
A) 0.693 
B) 1.65 × 10-2 
C) 1.98 
D) 0.198 
E) 3.30 ×10-3

Question 9

In the energy profile of a reaction, the species that exists at the maximum on the curve is called the ________.

Accepted Answer

A) product 
B) activated complex 
C) activation energy 
D) enthalpy of reaction 
E) atomic state 
A) product 
B) activated complex 
C) activation energy 
D) enthalpy of reaction 
E) atomic state

Question 10

The active site of nitrogenase is a cofactor that contains two transition metals. These transition metals are ________.

Accepted Answer

A) Cr and Mg 
B) Mn and V 
C) Os and Ir 
D) Fe and Zn 
E) Fe and Mo 
A) Cr and Mg 
B) Mn and V 
C) Os and Ir 
D) Fe and Zn 
E) Fe and Mo

Question 11

The data in the table below were obtained for the reaction:
A + B → P  
-The magnitude of the rate constant is ________.

Accepted Answer

A) 38.0 
B) 0.278 
C) 13.2 
D) 42.0 
E) 2.21 
A) 38.0 
B) 0.278 
C) 13.2 
D) 42.0 
E) 2.21

Question 12

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by ________.

Accepted Answer

The answer of The relationship of absorbed light to the...

Question 13

A compound decomposes by a first-order process. If 13% of the compound decomposes in 60 minutes, the half-life of the compound is ________.

Accepted Answer

A) 299 
B) 20 
C) 12 
D) -18 
E) -5 
A) 299 
B) 20 
C) 12 
D) -18 
E) -5

Question 14

The mechanism for formation of the product X is: A + B → C + D (slow)
B + D → X (fast)
The intermediate reactant in the reaction is ________.

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) X 
A) A 
B) B 
C) C 
D) D 
E) X

Question 15

The rate constant of a first-order process that has a half-life of 462 s is ________ s-1.

Accepted Answer

A) 1.50 × 10-3 
B) 3.20 × 102 
C) 6.67 × 102 
D) -1.08 × 10-3 
E) 2.16 × 10-3 
A) 1.50 × 10-3 
B) 3.20 × 102 
C) 6.67 × 102 
D) -1.08 × 10-3 
E) 2.16 × 10-3

Question 16

Elementary reactions involving the simultaneous collision of three molecules are ________.

Accepted Answer

The answer of Elementary reactions involving the simultaneous collision of...

Question 17

The rate of a reaction depends on ________.

Accepted Answer

A) collision frequency 
B) collision energy 
C) collision orientation 
D) all of the above 
E) none of the above 
A) collision frequency 
B) collision energy 
C) collision orientation 
D) all of the above 
E) none of the above

Question 18

The reaction A → B is first order in [A]. Consider the following data.  
-The concentration of A is ________ M after 40.0 s.

Accepted Answer

A) 1.3 × 10-2 
B) 1.2 
C) 0.17 
D) 3.5 × 10-4 
E) 0.025 
A) 1.3 × 10-2 
B) 1.2 
C) 0.17 
D) 3.5 × 10-4 
E) 0.025

Question 19

If a rate law is second order (reactant), doubling the reactant ________ the reaction rate.

Accepted Answer

The answer of If a rate law is second order...

Question 20

A reaction was found to be zero order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to ________.

Accepted Answer

A) remain constant 
B) increase by a factor of 27 
C) increase by a factor of 9 
D) triple 
E) decrease by a factor of the cube root of 3 
A) remain constant 
B) increase by a factor of 27 
C) increase by a factor of 9 
D) triple 
E) decrease by a factor of the cube root of 3

Exam 14: Chemical Kinetics

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if Ea = 55.3 kJ/mol?

The data in the table below were obtained for the reaction: A + B → P -The rate law for this reaction is rate = ________.

The rate law of a reaction is rate = k[D][X]. The units of the rate constant are ________.

A burning splint will burn more vigorously in pure oxygen than in air because ________.

One difference between first- and second-order reactions is that ________.

Which of the following is true?

As the temperature of a reaction is increased, the rate of the reaction increases because the ________.

The reaction A → B is first order in [A]. Consider the following data. -The rate constant of a first-order process that has a half-life of 3.50 min is ________ s-1.

In the energy profile of a reaction, the species that exists at the maximum on the curve is called the ________.

The active site of nitrogenase is a cofactor that contains two transition metals. These transition metals are ________.

The data in the table below were obtained for the reaction: A + B → P -The magnitude of the rate constant is ________.

The relationship of absorbed light to the concentration of the substance absorbing the light is governed by ________.

A compound decomposes by a first-order process. If 13% of the compound decomposes in 60 minutes, the half-life of the compound is ________.

The mechanism for formation of the product X is: A + B → C + D (slow) B + D → X (fast) The intermediate reactant in the reaction is ________.

The rate constant of a first-order process that has a half-life of 462 s is ________ s-1.

Elementary reactions involving the simultaneous collision of three molecules are ________.

The rate of a reaction depends on ________.

The reaction A → B is first order in [A]. Consider the following data. -The concentration of A is ________ M after 40.0 s.

If a rate law is second order (reactant), doubling the reactant ________ the reaction rate.

A reaction was found to be zero order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to ________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

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Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

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A particular first-order reaction has a rate constant of 1.35 × 10² s^-1 at 25.0 °C. What is the magnitude of k at 75.0 °C if E_a = 55.3 kJ/mol?

The reaction A → B is first order in [A]. Consider the following data. -The rate constant of a first-order process that has a half-life of 3.50 min is ________ s^-1.

The rate constant of a first-order process that has a half-life of 462 s is ________ s^-1.