Question 1

If the rate law for the reaction 2A + 3B → products
Is second order in A and first order in B, then the rate law is rate = __________.

Accepted Answer

A) k[A][B] 
B) k[A]2[B]3 
C) k[A][B]2 
D) k[A]2[B] 
E) k[A]2[B]2 
A) k[A][B] 
B) k[A]2[B]3 
C) k[A][B]2 
D) k[A]2[B] 
E) k[A]2[B]2

Question 2

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 3

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 4

The average rate of disappearance of A between 10 s and 20 s is __________ mol/s.

Accepted Answer

A) 2.2 × 10-3 
B) 1.1 × 10-3 
C) 4.4 × 10-3 
D) 454 
E) 9.90 × 10-3 
A) 2.2 × 10-3 
B) 1.1 × 10-3 
C) 4.4 × 10-3 
D) 454 
E) 9.90 × 10-3

Question 5

Which one of the following is not a valid expression for the rate of the reaction below? 4NH3 + 7O2 → 4NO2 + 6H2O

Accepted Answer

A)    
B)    
C)    
D)    
E) All of the above are valid expressions of the reaction rate. 
A)    
B)    
C)    
D)    
E) All of the above are valid expressions of the reaction rate.

Question 6

The number of molecules that participate as reactants defines the __________ of the reaction.

Accepted Answer

The answer of The number of molecules that participate as...

Question 7

A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M. The rate constant for this reaction is __________ M-1s-1.

Accepted Answer

A) 12 
B) 2.0 x 10-2 
C) 8.5 × 10-2 
D) 4.3 x 10-2 
E) 4.3 
A) 12 
B) 2.0 x 10-2 
C) 8.5 × 10-2 
D) 4.3 x 10-2 
E) 4.3

Question 8

The following reaction occurs in aqueous solution: NH4+ (aq)+ NO2- → N2 (g)+ 2H2O (l)
The data below is obtained at 25°C.   The order of the reaction in NH4+ is __________.

Accepted Answer

A) -2 
B) -1 
C) +2 
D) +1 
E) 0 
A) -2 
B) -1 
C) +2 
D) +1 
E) 0

Question 9

The order of the reaction in B is __________.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 0 
A) 1 
B) 2 
C) 3 
D) 4 
E) 0

Question 10

The minimum energy to initiate a chemical reaction is the __________.

Accepted Answer

The answer of The minimum energy to initiate a chemical...

Question 11

The primary source of the specificity of enzymes is __________.

Accepted Answer

A) their polarity, which matches that of their specific substrate 
B) their delocalized electron cloud 
C) their bonded transition metal, which is specific to the target substrate 
D) their locations within the cell 
E) their shape, which relates to the lock-and-key model 
A) their polarity, which matches that of their specific substrate 
B) their delocalized electron cloud 
C) their bonded transition metal, which is specific to the target substrate 
D) their locations within the cell 
E) their shape, which relates to the lock-and-key model

Question 12

The rate limiting step in a reaction is the slowest step in the reaction sequence.

Accepted Answer

A) True 
 B)False

Question 13

Consider the following reaction: 3A → 2B
The average rate of appearance of B is given by Δ[B]/Δt. Comparing the rate of appearance of B and the rate of disappearance of A, we get Δ[B]/Δt = __________ × (-Δ[A]/Δt).

Accepted Answer

A) -2/3 
B) +2/3 
C) -3/2 
D) +1 
E) +3/2 
A) -2/3 
B) +2/3 
C) -3/2 
D) +1 
E) +3/2

Question 14

A second-order reaction has a half-life of 18 s when the initial concentration of reactant is 0.71 M. The rate constant for this reaction is __________ M-1s-1.

Accepted Answer

A) 7.8 × 10-2 
B) 3.8 × 10-2 
C) 2.0 × 10-2 
D) 1.3 
E) 18 
A) 7.8 × 10-2 
B) 3.8 × 10-2 
C) 2.0 × 10-2 
D) 1.3 
E) 18

Question 15

The following reaction is second order in [A] and the rate constant is 0.025 M-1s-1: A → B
The concentration of A was 0.65 M at 33 s. The initial concentration of A was __________ M.

Accepted Answer

A) 2.4 
B) 0.27 
C) 0.24 
D) 1.4 
E) 1.2 × 10-2 
A) 2.4 
B) 0.27 
C) 0.24 
D) 1.4 
E) 1.2 × 10-2

Question 16

The average rate of disappearance of I- between 400.0 s and 800.0 s is __________ M/s.

Accepted Answer

A) 2.8 × 10-5 
B) 1.4 × 10-5 
C) 5.8 × 10-5 
D) 3.6 × 104 
E) 2.6 × 10-4 
A) 2.8 × 10-5 
B) 1.4 × 10-5 
C) 5.8 × 10-5 
D) 3.6 × 104 
E) 2.6 × 10-4

Question 17

The overall order of the reaction is __________.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 0 
A) 1 
B) 2 
C) 3 
D) 4 
E) 0

Question 18

The rate law of the overall reaction A + B → C
Is rate = k[A]2. Which of the following will not increase the rate of the reaction?

Accepted Answer

A) increasing the concentration of reactant A 
B) increasing the concentration of reactant B 
C) increasing the temperature of the reaction 
D) adding a catalyst for the reaction 
E) All of these will increase the rate. 
A) increasing the concentration of reactant A 
B) increasing the concentration of reactant B 
C) increasing the temperature of the reaction 
D) adding a catalyst for the reaction 
E) All of these will increase the rate.

Question 19

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 20

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

Exam 14: Chemical Kinetics

If the rate law for the reaction 2A + 3B → products Is second order in A and first order in B, then the rate law is rate = __________.

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

The rate of a reaction depends on __________.

The average rate of disappearance of A between 10 s and 20 s is __________ mol/s.

Which one of the following is not a valid expression for the rate of the reaction below? 4NH3 + 7O2 → 4NO2 + 6H2O

The number of molecules that participate as reactants defines the __________ of the reaction.

A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M. The rate constant for this reaction is __________ M-1s-1.

The following reaction occurs in aqueous solution: NH4+ (aq)+ NO2- → N2 (g)+ 2H2O (l) The data below is obtained at 25°C. The order of the reaction in NH4+ is __________.

The order of the reaction in B is __________.

The minimum energy to initiate a chemical reaction is the __________.

The primary source of the specificity of enzymes is __________.

The rate limiting step in a reaction is the slowest step in the reaction sequence.

Consider the following reaction: 3A → 2B The average rate of appearance of B is given by Δ[B]/Δt. Comparing the rate of appearance of B and the rate of disappearance of A, we get Δ[B]/Δt = __________ × (-Δ[A]/Δt).

A second-order reaction has a half-life of 18 s when the initial concentration of reactant is 0.71 M. The rate constant for this reaction is __________ M-1s-1.

The following reaction is second order in [A] and the rate constant is 0.025 M-1s-1: A → B The concentration of A was 0.65 M at 33 s. The initial concentration of A was __________ M.

The average rate of disappearance of I- between 400.0 s and 800.0 s is __________ M/s.

The overall order of the reaction is __________.

The rate law of the overall reaction A + B → C Is rate = k[A]2. Which of the following will not increase the rate of the reaction?

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

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

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

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Which one of the following is not a valid expression for the rate of the reaction below? 4NH₃ + 7O₂ → 4NO₂ + 6H₂O

A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M. The rate constant for this reaction is __________ M^-1s^-1.

The following reaction occurs in aqueous solution: NH₄⁺(aq)+ NO₂^- → N₂(g)+ 2H₂O (l) The data below is obtained at 25°C. The order of the reaction in NH₄⁺ is __________.

A second-order reaction has a half-life of 18 s when the initial concentration of reactant is 0.71 M. The rate constant for this reaction is __________ M^-1s^-1.

The following reaction is second order in [A] and the rate constant is 0.025 M^-1s^-1: A → B The concentration of A was 0.65 M at 33 s. The initial concentration of A was __________ M.

The average rate of disappearance of I^- between 400.0 s and 800.0 s is __________ M/s.

The rate law of the overall reaction A + B → C Is rate = k[A]². Which of the following will not increase the rate of the reaction?