Question 1

What is the order of reaction for the following reaction: Rate = k[A]-1/2 [B]1/2?

Accepted Answer

A) first order 
B) zero order 
C) 1/2 order 
D) -1/2 order 
E) second order 
A) first order 
B) zero order 
C) 1/2 order 
D) -1/2 order 
E) second order B

Question 2

Energy of activation has no effect on reaction rate.

Accepted Answer

A) True 
 B)False  False

Question 3

The decomposition of dinitrogen pentoxide is described by the chemical equation
2 N2O5(g)→ 4 NO2(g)+ O2(g).
If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

Accepted Answer

A) 0.800 mol min-1 
B) 1.60 mol min-1 
C) 3.20 mol min-1 
D) 6.40 mol min-1 
A) 0.800 mol min-1 
B) 1.60 mol min-1 
C) 3.20 mol min-1 
D) 6.40 mol min-1 C

Question 4

Data for the reaction A + B → C are given below.Find the rate constant for this system.

Accepted Answer

A) 2.8 × 10-2 M-1s-1  
B) 2.8 × 10-2 Ms-1  
C) 2.8 × 10-2 M2s-1  
D) 1.7 × 10-3 M-1s-1  
E) 1.7 × 10-3 Ms-1  
A) 2.8 × 10-2 M-1s-1  
B) 2.8 × 10-2 Ms-1  
C) 2.8 × 10-2 M2s-1  
D) 1.7 × 10-3 M-1s-1  
E) 1.7 × 10-3 Ms-1

Question 5

A reaction is first order.If its initial rate is 0.0200 M/s and 25.0 days later its rate is 6.25 × 10-4 M/s,then its half-life is ________.

Accepted Answer

A) 12.5 days 
B) 5.0 days 
C) 25.0 days 
D) 50.0 days 
E) 2.5 days 
A) 12.5 days 
B) 5.0 days 
C) 25.0 days 
D) 50.0 days 
E) 2.5 days

Question 6

Activation energy is:
I.the minimum kinetic energy required for each molecule in a collision to produce a reaction.
II.the minimum total kinetic energy required for the molecules in a collision to produce a reaction.
III.a factor in determining the rate of a reaction.
IV.high for fast reactions.

Accepted Answer

A) I and III 
B) I,III,and IV 
C) II,III 
D) II and IV 
E) II,III,and IV 
A) I and III 
B) I,III,and IV 
C) II,III 
D) II and IV 
E) II,III,and IV

Question 7

According to the collision theory in gaseous molecules,collision frequency is ________ and the rate of reaction is ________ because ________.

Accepted Answer

A) low,low,molecules are so far apart 
B) high,high,each collision results in a reaction 
C) low,low,molecules must collide before they can react 
D) high,relatively low,only a fraction of the collisions lead to a reaction 
E) low,high,molecules are moving so fast that each reaction causes many others 
A) low,low,molecules are so far apart 
B) high,high,each collision results in a reaction 
C) low,low,molecules must collide before they can react 
D) high,relatively low,only a fraction of the collisions lead to a reaction 
E) low,high,molecules are moving so fast that each reaction causes many others

Question 8

The rate of disappearance of HBr in the gas phase reaction
2 HBr(g)→   (g)+   (g) Is 0.130 mol L-1  
At 150 °C.The rate of reaction is ________ mol L-1  
.

Accepted Answer

A) 3.85 
B) 0.0650 
C) 0.0169 
D) 0.260 
E) 0.0860 
A) 3.85 
B) 0.0650 
C) 0.0169 
D) 0.260 
E) 0.0860

Question 9

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl ][N]2?

Accepted Answer

A) zero order 
B) first order 
C) second order 
D) third order 
A) zero order 
B) first order 
C) second order 
D) third order

Question 10

Define activation energy.

Accepted Answer

A) the difference between the energy of the products and reactants 
B) the energy difference between the maximum energy of reaction and the energy of the products 
C) the minimum total kinetic energy that molecules must bring to their collisions for a chemical reaction to occur 
D) the total kinetic energy of molecules in collisions 
E) the total kinetic energy of molecules in a system 
A) the difference between the energy of the products and reactants 
B) the energy difference between the maximum energy of reaction and the energy of the products 
C) the minimum total kinetic energy that molecules must bring to their collisions for a chemical reaction to occur 
D) the total kinetic energy of molecules in collisions 
E) the total kinetic energy of molecules in a system

Question 11

For a reaction Rate = k[A][B]2,what factor will keep k unchanged?

Accepted Answer

A) raising temperature 
B) adding inhibitor 
C) increasing [A] 
D) adding catalyst 
A) raising temperature 
B) adding inhibitor 
C) increasing [A] 
D) adding catalyst

Question 12

For the second order reaction A → products,the following data are obtained:
[A] = 3.024 M,t = 0 min
[A] = 2.935 M,t = 1.0 min
[A] = 2.852 M,t = 2.0 min
What is the rate constant,k?

Accepted Answer

A) 3.6 × 10-3 M-1 min-1  
B) 1.4 × 10-2 M-1 min-1  
C) 2.2 × 10-2 M-1 min-1  
D) 9.7 × 10-3 M-1 min-1  
E) 1.0 × 10-2 M-1 min-1  
A) 3.6 × 10-3 M-1 min-1  
B) 1.4 × 10-2 M-1 min-1  
C) 2.2 × 10-2 M-1 min-1  
D) 9.7 × 10-3 M-1 min-1  
E) 1.0 × 10-2 M-1 min-1

Question 13

In a second order reaction:
I.the sum of the exponents in the rate law is equal to two.
II.at least one of the exponents in the rate law is a two.
III.the half-life is dependent on the initial concentration of the reactant species.
IV.the half-life is independent of the initial concentration of the reactant species.
V.k can be expressed as M-2s-1 or M-2min-1.

Accepted Answer

A) I and IV 
B) II and IV 
C) I,III,and V 
D) I and III 
E) II and III 
A) I and IV 
B) II and IV 
C) I,III,and V 
D) I and III 
E) II and III

Question 14

For the second order reaction A → products,the following data are obtained:
[A] = 1.512 M,t = 0 min
[A] = 1.490 M,t = 1.0 min
[A] = 1.469 M,t = 2.0 min
What is the rate constant,k,for the reaction?

Accepted Answer

A) 3.6 × 10-3 M-1 min-1  
B) 1.4 × 10-2 M-1 min-1  
C) 2.2 × 10-2 M-1 min-1  
D) 1.0 × 10-2 M-1 min-1  
E) 9.7 × 10-3 M-1 min-1  
A) 3.6 × 10-3 M-1 min-1  
B) 1.4 × 10-2 M-1 min-1  
C) 2.2 × 10-2 M-1 min-1  
D) 1.0 × 10-2 M-1 min-1  
E) 9.7 × 10-3 M-1 min-1

Question 15

What is the rate law for the following reaction and its mechanism?
2 O3 → 3 O2 (overall reaction)
O3 → O2 + O∙ (slow)
O∙ + O3 → 2 O2 (fast)

Accepted Answer

A) Rate = k[O3] 
B) Rate = k[O3]2  
C) Rate = k[O3]2/[O2] 
D) Rate = k[O3]/[O2] 
E) Rate = k[O3][O2] 
A) Rate = k[O3] 
B) Rate = k[O3]2  
C) Rate = k[O3]2/[O2] 
D) Rate = k[O3]/[O2] 
E) Rate = k[O3][O2]

Question 16

In the Arrhenius equation,ln k = -Ea/RT + ln A,the symbol A denotes:

Accepted Answer

A) the initial concentration of A 
B) the activation energy 
C) the rate constant 
D) a constant that represents the frequency of collisions with the proper orientation and other steric conditions favorable for a reaction 
E) the absolute temperature 
A) the initial concentration of A 
B) the activation energy 
C) the rate constant 
D) a constant that represents the frequency of collisions with the proper orientation and other steric conditions favorable for a reaction 
E) the absolute temperature

Question 17

The isomerization of methylisonitrile to acetonitrile 
  NC(g)→   CN(g)
Is first order in   NC.The half-life of the reaction is 5.20 × 101 s at 545 K.The rate constant when the initial [   NC] is 0.030 mol L-1 is ________  
.

Accepted Answer

A) 75.1 
B) 0.641 
C) 0.0133 
D) 1.56 
E) 2.84 × 104 
A) 75.1 
B) 0.641 
C) 0.0133 
D) 1.56 
E) 2.84 × 104

Question 18

The rate constant at 160 °C for the first order decomposition of ore is 0.032/min.The half-life of the reaction is ________.

Accepted Answer

A) 62.5 s 
B) 31.25 s 
C) 5000 s 
D) 111 s 
E) 1300 s 
A) 62.5 s 
B) 31.25 s 
C) 5000 s 
D) 111 s 
E) 1300 s

Question 19

For the second-order reaction A → products,the following data are obtained:
[A] = 3.024 M,t = 0 min
[A] = 2.935 M,t = 1.0 min
[A] = 2.852 M,t = 2.0 min
What is the concentration of [A] after 4 min?

Accepted Answer

A) 2.70 M 
B) 2.66 M 
C) 0.76 M 
D) 2.76 M 
E) 2.62 M 
A) 2.70 M 
B) 2.66 M 
C) 0.76 M 
D) 2.76 M 
E) 2.62 M

Question 20

Given the following initial rate data,write the rate law expression.

Accepted Answer

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

Exam 20: Chemical Kinetics

What is the order of reaction for the following reaction: Rate = k[A]-1/2 [B]1/2?

Energy of activation has no effect on reaction rate.

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N2O5(g)→ 4 NO2(g)+ O2(g). If the rate of disappearance of N2O5 is equal to 1.60 mol min-1 at a particular moment,what is the rate of appearance of NO2 at that moment?

Data for the reaction A + B → C are given below.Find the rate constant for this system.

A reaction is first order.If its initial rate is 0.0200 M/s and 25.0 days later its rate is 6.25 × 10-4 M/s,then its half-life is ________.

Activation energy is: I.the minimum kinetic energy required for each molecule in a collision to produce a reaction. II.the minimum total kinetic energy required for the molecules in a collision to produce a reaction. III.a factor in determining the rate of a reaction. IV.high for fast reactions.

According to the collision theory in gaseous molecules,collision frequency is ________ and the rate of reaction is ________ because ________.

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g)→ (g)+ (g) Is 0.130 mol L-1 At 150 °C.The rate of reaction is ________ mol L-1 .

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl ][N]2?

Define activation energy.

For a reaction Rate = k[A][B]2,what factor will keep k unchanged?

For the second order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the rate constant,k?

For the second order reaction A → products,the following data are obtained: [A] = 1.512 M,t = 0 min [A] = 1.490 M,t = 1.0 min [A] = 1.469 M,t = 2.0 min What is the rate constant,k,for the reaction?

What is the rate law for the following reaction and its mechanism? 2 O3 → 3 O2 (overall reaction) O3 → O2 + O∙ (slow) O∙ + O3 → 2 O2 (fast)

In the Arrhenius equation,ln k = -Ea/RT + ln A,the symbol A denotes:

The isomerization of methylisonitrile to acetonitrile NC(g)→ CN(g) Is first order in NC.The half-life of the reaction is 5.20 × 101 s at 545 K.The rate constant when the initial [ NC] is 0.030 mol L-1 is ________ .

The rate constant at 160 °C for the first order decomposition of ore is 0.032/min.The half-life of the reaction is ________.

For the second-order reaction A → products,the following data are obtained: [A] = 3.024 M,t = 0 min [A] = 2.935 M,t = 1.0 min [A] = 2.852 M,t = 2.0 min What is the concentration of [A] after 4 min?

Given the following initial rate data,write the rate law expression.

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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What is the order of reaction for the following reaction: Rate = k[A]^-1/2 [B]^1/2?

The decomposition of dinitrogen pentoxide is described by the chemical equation 2 N₂O₅(g)→ 4 NO₂(g)+ O₂(g). If the rate of disappearance of N₂O₅ is equal to 1.60 mol min^-1 at a particular moment,what is the rate of appearance of NO₂ at that moment?

A reaction is first order.If its initial rate is 0.0200 M/s and 25.0 days later its rate is 6.25 × 10^-4 M/s,then its half-life is ________.

According to the collision theory in gaseous molecules,collision frequency is and the rate of reaction is because .

The rate of disappearance of HBr in the gas phase reaction 2 HBr(g)→ (g)+ (g) Is 0.130 mol L^-1 At 150 °C.The rate of reaction is ________ mol L^-1 .

What is the overall reaction order for the reaction that has the rate law Rate = k[Cl][N]²?

For a reaction Rate = k[A][B]²,what factor will keep k unchanged?

What is the rate law for the following reaction and its mechanism? 2 O₃ → 3 O₂ (overall reaction) O₃ → O₂ + O∙ (slow) O∙ + O₃ → 2 O₂ (fast)

In the Arrhenius equation,ln k = ^-^E_a/RT + ln A,the symbol A denotes:

The isomerization of methylisonitrile to acetonitrile NC(g)→ CN(g) Is first order in NC.The half-life of the reaction is 5.20 × 10¹ s at 545 K.The rate constant when the initial [ NC] is 0.030 mol L^-1 is ________ .