Question 1

"Instantaneous rate" is defined as the

Accepted Answer

A) change in concentration per g. 
B) equation showing how the rate depends on the concentration of each product. 
C) rate of reaction at a particular time. 
D) rate of reaction during at time zero. 
A) change in concentration per g. 
B) equation showing how the rate depends on the concentration of each product. 
C) rate of reaction at a particular time. 
D) rate of reaction during at time zero. C

Question 2

In aqueous solution,hypobromite ion,BrO-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation. 3 BrO-(aq)→ BrO3-(aq)+ 2 Br-(aq)
A plot of 1/[BrO-] vs.time is linear and the slope is equal to 0.056 M-1s-1.If the initial concentration of BrO- is 0.65 M,how long will it take one-half of the BrO- ion to react?

Accepted Answer

A) 3.6 × 10-2 s 
B) 7.1 s 
C) 12 s 
D) 27 
A) 3.6 × 10-2 s 
B) 7.1 s 
C) 12 s 
D) 27 D

Question 3

The following reaction is first order in A and first order in B: A + B → Products Rate = k[A][B]
What is the initial rate of this reaction in vessel (b)relative to the initial rate of this reaction in vessel (a)? Each vessel has the same volume.Shaded spheres represent A molecules,and unshaded spheres represent B molecules present at the beginning of the reaction.

Accepted Answer

A) rate in vessel (b)/rate in vessel (a)= 1:2 
B) rate in vessel (b)/rate in vessel (a)= 1:1 
C) rate in vessel (b)/rate in vessel (a)= 2:1 
D) rate in vessel (b)/rate in vessel (a)= 4:1 
A) rate in vessel (b)/rate in vessel (a)= 1:2 
B) rate in vessel (b)/rate in vessel (a)= 1:1 
C) rate in vessel (b)/rate in vessel (a)= 2:1 
D) rate in vessel (b)/rate in vessel (a)= 4:1 A

Question 4

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq)→ 2 H2O(l)+ O2(g)
Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Accepted Answer

A) [H2O2] versus time 
B) [H2O2]2 versus time 
C) 1/[H2O2] versus time 
D) ln[H2O2] versus time 
A) [H2O2] versus time 
B) [H2O2]2 versus time 
C) 1/[H2O2] versus time 
D) ln[H2O2] versus time

Question 5

Consider a reaction that occurs by the following one-step mechanism:
AS1U1B12S1U1B0 + BS1U1B12S1U1B0 → 2 AB
The potential energy profile for this reaction is shown below.  
-The activation energy for the forward reaction is given by the difference in energy between which two reaction stages?

Accepted Answer

A) reaction stage 2 - reaction stage 1 
B) reaction stage 2 - reaction stage 3 
C) reaction stage 1 - reaction stage 3 
D) reaction stage 3 - reaction stage 1 
A) reaction stage 2 - reaction stage 1 
B) reaction stage 2 - reaction stage 3 
C) reaction stage 1 - reaction stage 3 
D) reaction stage 3 - reaction stage 1

Question 6

Consider a reaction that occurs by the following one-step mechanism:
AS1U1B12S1U1B0 + BS1U1B12S1U1B0 → 2 AB
The potential energy profile for this reaction is shown below.  
-What is the species present at reaction stage 1?

Accepted Answer

A) an intermediate 
B) a product 
C) a reactant 
D) a transition state 
A) an intermediate 
B) a product 
C) a reactant 
D) a transition state

Question 7

Consider a reaction that occurs by the following one-step mechanism:
AS1U1B12S1U1B0 + BS1U1B12S1U1B0 → 2 AB
The potential energy profile for this reaction is shown below.  
-What is the species present at reaction stage 3?

Accepted Answer

A) an intermediate 
B) a product 
C) a reactant 
D) a transition state 
A) an intermediate 
B) a product 
C) a reactant 
D) a transition state

Question 8

-Which of the elementary reactions shown above has a molecularity of one?

Accepted Answer

A) elementary reaction (a) 
B) elementary reaction (b) 
C) elementary reaction (c) 
D) elementary reactions (a), (b),and (c) 
A) elementary reaction (a) 
B) elementary reaction (b) 
C) elementary reaction (c) 
D) elementary reactions (a), (b),and (c)

Question 9

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 300 seconds?

Accepted Answer

A) picture a) 
B) picture b) 
C) picture c) 
D) picture d) 
A) picture a) 
B) picture b) 
C) picture c) 
D) picture d)

Question 10

The reaction A + B C + D occurs in one step.The activation energy is 132 kJ/mol and ΔE = -236 kJ/mol.What is the activation energy for the reverse reaction?

Accepted Answer

A) -104 
B) 368 
C) -368 
D) 104 
A) -104 
B) 368 
C) -368 
D) 104

Question 11

-Which of the elementary reactions shown above has a molecularity of two?

Accepted Answer

A) elementary reaction (a) 
B) elementary reaction (b) 
C) elementary reaction (c) 
D) elementary reactions (a), (b),and (c) 
A) elementary reaction (a) 
B) elementary reaction (b) 
C) elementary reaction (c) 
D) elementary reactions (a), (b),and (c)

Question 12

A concentration-time study of the gas phase reaction 2 A3 → 3 A2 produced the data in the table below. Time (s)[A3] (M)[A2] (M)
0 4.00 × 10-4 0
10 2.00 × 10-4 3.00 × 10-4
20 1.00 × 10-4 4.50 × 10-4
30 5.00 × 10-5 ?
What is the average rate of decomposition of A3 in the time interval 20-30 seconds?

Accepted Answer

A) 4.00 × 10-4 M/s 
B) 3.50 × 10-5 M/s 
C) 5.00 × 10-6 M/s 
D) 4.00 × 10-6 M/s 
A) 4.00 × 10-4 M/s 
B) 3.50 × 10-5 M/s 
C) 5.00 × 10-6 M/s 
D) 4.00 × 10-6 M/s

Question 13

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Accepted Answer

A) activation energy 
B) net energy 
C) potential energy 
D) rate limiting energy 
A) activation energy 
B) net energy 
C) potential energy 
D) rate limiting energy

Question 14

Shown is a concentration versus time plot for a reaction involving gases A,B,and C.  
-Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10-5 M/s.What is the rate of reaction with respect to A over the time interval 0 to 100 seconds?

Accepted Answer

A) 0 M/s 
B) less than 3.7 × 10-5 M/s 
C) 3.7 × 10-5 M/s 
D) greater than 3.7 × 10-5 M/s 
A) 0 M/s 
B) less than 3.7 × 10-5 M/s 
C) 3.7 × 10-5 M/s 
D) greater than 3.7 × 10-5 M/s

Question 15

The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]2. BrO3-(aq)+ 5 Br-(aq)+ 6 H+(aq)→ 3 Br2(aq)+ 3 H2O(l)
What is the order of reaction with respect to Br -?

Accepted Answer

A) first 
B) second 
C) fifth 
D) sixth 
A) first 
B) second 
C) fifth 
D) sixth

Question 16

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 2.00? The rate will

Accepted Answer

A) decrease by a factor of 1/4.00. 
B) decrease by a factor of 1/2.00. 
C) increase by a factor of 2.00. 
D) increase by a factor of 4.00. 
A) decrease by a factor of 1/4.00. 
B) decrease by a factor of 1/2.00. 
C) increase by a factor of 2.00. 
D) increase by a factor of 4.00.

Question 17

A reaction with an activation energy,Ea = 103 kJ/mol has a rate constant,k = 3.5 × 10-5 s-1 at 25°C.For this reaction the rate constant at 45°C is ________.

Accepted Answer

Question 18

For the reaction shown below,if the rate of formation of Br2 is 1.5 × 10-6 M/s,over the same time period the rate of consumption of H+ is ________ M/s.
ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

Accepted Answer

Question 19

At 300°C decomposition of NO2(g)occurs with a rate law: Rate = - k[NO2]x.If the initial rate of decomposition is 3.2 × 10-5 M/s when [NO2]o = 8.0 × 10-3 M and the initial rate of decomposition is 8.0 × 10-6 M/s when [NO2]o = 4.0 × 10-3 M,then the order of reaction with respect to NO2,x = ________.

Accepted Answer

Question 20

Consider a reaction that occurs by the following mechanism:
A + BC → AC + B
AC + D → A + CD
The potential energy profile for this reaction is shown below.  
-Intermediates occur at which reaction stages?

Accepted Answer

A) reaction stages 1 and 5 
B) reaction stages 2,3,and 4 
C) reaction stages 2 and 4 
D) reaction stage 3 
A) reaction stages 1 and 5 
B) reaction stages 2,3,and 4 
C) reaction stages 2 and 4 
D) reaction stage 3

"Instantaneous rate" is defined as the

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -The activation energy for the forward reaction is given by the difference in energy between which two reaction stages?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 3?

-Which of the elementary reactions shown above has a molecularity of one?

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 300 seconds?

The reaction A + B C + D occurs in one step.The activation energy is 132 kJ/mol and ΔE = -236 kJ/mol.What is the activation energy for the reverse reaction?

-Which of the elementary reactions shown above has a molecularity of two?

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10^-5 M/s.What is the rate of reaction with respect to A over the time interval 0 to 100 seconds?

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]². BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l) What is the order of reaction with respect to Br^-?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 2.00? The rate will

A reaction with an activation energy,E_a = 103 kJ/mol has a rate constant,k = 3.5 × 10^-5 s^-1 at 25°C.For this reaction the rate constant at 45°C is ________.

For the reaction shown below,if the rate of formation of Br₂ is 1.5 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)

Consider a reaction that occurs by the following mechanism: A + BC → AC + B AC + D → A + CD The potential energy profile for this reaction is shown below. -Intermediates occur at which reaction stages?

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Exam 13: Chemical Kinetics

"Instantaneous rate" is defined as the

The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H2O2(aq)→ 2 H2O(l)+ O2(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Consider a reaction that occurs by the following one-step mechanism: A2 + B2 → 2 AB The potential energy profile for this reaction is shown below. -The activation energy for the forward reaction is given by the difference in energy between which two reaction stages?

Consider a reaction that occurs by the following one-step mechanism: A2 + B2 → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

Consider a reaction that occurs by the following one-step mechanism: A2 + B2 → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 3?

-Which of the elementary reactions shown above has a molecularity of one?

Consider the first-order reaction A → B in which A molecules (unshaded spheres)are converted to B molecules (shaded spheres).Given the following pictures at t = 0 seconds and t = 100 seconds,which picture represents the number of A and B molecules remaining at 300 seconds?

The reaction A + B C + D occurs in one step.The activation energy is 132 kJ/mol and ΔE = -236 kJ/mol.What is the activation energy for the reverse reaction?

-Which of the elementary reactions shown above has a molecularity of two?

What is the minimum energy barrier that must be overcome for a chemical reaction to occur?

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10-5 M/s.What is the rate of reaction with respect to A over the time interval 0 to 100 seconds?

The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]2. BrO3-(aq)+ 5 Br-(aq)+ 6 H+(aq)→ 3 Br2(aq)+ 3 H2O(l) What is the order of reaction with respect to Br -?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 2.00? The rate will

A reaction with an activation energy,Ea = 103 kJ/mol has a rate constant,k = 3.5 × 10-5 s-1 at 25°C.For this reaction the rate constant at 45°C is ________.

For the reaction shown below,if the rate of formation of Br2 is 1.5 × 10-6 M/s,over the same time period the rate of consumption of H+ is ________ M/s. ClO2-(aq)+ 4 Br-(aq)+ 4 H+(aq)→ Cl-(aq)+ 2 Br2(aq)+2 H2O(l)

Consider a reaction that occurs by the following mechanism: A + BC → AC + B AC + D → A + CD The potential energy profile for this reaction is shown below. -Intermediates occur at which reaction stages?

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Covalent Compounds: Bonding Theories and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids, solids, and Phase Changes

Solutions and Their Properties

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Applications of Aqueous Equilibria

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

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Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

The Main-Group Elements

Connections to Organic and Biological Chemistry

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The first-order decomposition of hydrogen peroxide occurs according to the equation 2 H₂O₂(aq)→ 2 H₂O(l)+ O₂(g) Using data from a concentration-time study of this reaction,which plot will produce a straight line?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -The activation energy for the forward reaction is given by the difference in energy between which two reaction stages?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 1?

Consider a reaction that occurs by the following one-step mechanism: A₂ + B₂ → 2 AB The potential energy profile for this reaction is shown below. -What is the species present at reaction stage 3?

Shown is a concentration versus time plot for a reaction involving gases A,B,and C. -Over the time interval 300 to 400 seconds,the rate of reaction with respect to A is Δ[A]/Δt = 3.7 × 10^-5 M/s.What is the rate of reaction with respect to A over the time interval 0 to 100 seconds?

The reaction shown below has the rate law: Rate = k[BrO₃^-][Br^-][H⁺]². BrO₃^-(aq)+ 5 Br^-(aq)+ 6 H⁺(aq)→ 3 Br₂(aq)+ 3 H₂O(l) What is the order of reaction with respect to Br^-?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 2.00? The rate will

A reaction with an activation energy,E_a = 103 kJ/mol has a rate constant,k = 3.5 × 10^-5 s^-1 at 25°C.For this reaction the rate constant at 45°C is ________.

For the reaction shown below,if the rate of formation of Br₂ is 1.5 × 10^-6 M/s,over the same time period the rate of consumption of H⁺ is ________ M/s. ClO₂^-(aq)+ 4 Br^-(aq)+ 4 H⁺(aq)→ Cl^-(aq)+ 2 Br₂(aq)+2 H₂O(l)