Question 1

What is the difference between average reaction rate and instantaneous reaction rate?

Accepted Answer

An average reaction rate is determined u...

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 0.80 M,how long will it take one-half of the BrO- ion to react?

Accepted Answer

A)   4.5 × 10-2 s
B)   7.1 s
C)   12 s
D)   22 s

Question 3

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0,what is the new rate if the concentration of [A] is increased to 0.200 M?

Accepted Answer

A)   0.0200 M/s
B)   0.0400 M/s
C)   0.0600 M/s
D)   0.0800 M/s
E)   0.100 M/s

Question 4

Given the following balanced equation,determine the rate of reaction with respect to [H2]. N2(g) + 3 H2(g) → 2 NH3(g)

Accepted Answer

A)   Rate = + 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
B)   Rate = + 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
C)   Rate = + 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
D)   Rate = - 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = +     
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
E)   It is not possible to determine without more information.

Question 5

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 1010 s-1,what is the rate constant for this reaction at 298 K?

Accepted Answer

A)   2.9 × 10-4 s-1
B)   7.4 × 10-4 s-1
C)   1.4 × 109 s-1
D)   4.6 × 105 s-1
E)   3.5 × 103 s-1

Question 6

Which of the following represents the equation for a first-order half-life?

Accepted Answer

A)   t 1/2 = 1/2 =   
B)   t 1/2 =   
C)   t 1/2 =   
D)   t 1/2 =   
E)   t 1/2 = [A]o" class="answers-bank-image d-inline" rel="preload" >
B)   t 1/2 = 1/2 =   
B)   t 1/2 =   
C)   t 1/2 =   
D)   t 1/2 =   
E)   t 1/2 = [A]o" class="answers-bank-image d-inline" rel="preload" >
C)   t 1/2 = 1/2 =   
B)   t 1/2 =   
C)   t 1/2 =   
D)   t 1/2 =   
E)   t 1/2 = [A]o" class="answers-bank-image d-inline" rel="preload" >
D)   t 1/2 = 1/2 =   
B)   t 1/2 =   
C)   t 1/2 =   
D)   t 1/2 =   
E)   t 1/2 = [A]o" class="answers-bank-image d-inline" rel="preload" >
E)   t 1/2 = [A]o

Question 7

The following reaction is first order,C2H6 → 2 CH3.If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K,how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

Accepted Answer

A)   4.5 min
B)   17 min
C)   53 min
D)   65 min

Question 8

Given the following balanced equation,determine the rate of reaction with respect to [N2]. N2(g) + 3 H2(g) → 2 NH3(g)

Accepted Answer

A)   Rate = + 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
B)   Rate = - 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
C)   Rate = + 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
D)   Rate = - 2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. N2(g) + 3 H2(g) → 2 NH3(g)  
A)   Rate = +   
B)   Rate = -   
C)   Rate = +     
D)   Rate = -     
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
E)   It is not possible to determine without more information.

Question 9

Define activation energy.

Accepted Answer

Activation energy is the energ...

Question 10

Given the following balanced equation,determine the rate of reaction with respect to [O2]. 2 SO2(g) + O2(g) → 2 SO3(g)

Accepted Answer

A)   Rate = - 2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
B)   Rate = + 2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
C)   Rate = - 2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
D)   Rate = - 2]. 2 SO2(g) + O2(g) → 2 SO3(g)  
A)   Rate = -     
B)   Rate = +     
C)   Rate = -   
D)   Rate = -   
E)   It is not possible to determine without more information." class="answers-bank-image d-inline" rel="preload" >
E)   It is not possible to determine without more information.

Question 11

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 95.0°C if Ea = 55.5 kJ/mol?

Accepted Answer

A)   9.56 × 103 s-1
B)   2.85 × 104 s-1
C)   576 s-1
D)   4.33 × 1087 s-1
E)   1.36 × 2 s-1 at 25.0°C.What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol? 
A)   9.56 × 103 s-1 
B)   2.85 × 104 s-1 
C)   576 s-1 
D)   4.33 × 1087 s-1 
E)   1.36 ×   s-1" class="answers-bank-image d-inline" rel="preload" > s-1

Question 12

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Accepted Answer

A)   4.55 M
B)   0.258 M
C)   3.87 M
D)   2.20 M
E)   2.39 M

Question 13

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0[B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

Accepted Answer

A)   0.0200 M/s
B)   0.0400 M/s
C)   0.0600 M/s
D)   0.0800 M/s
E)   0.100 M/s

Question 14

Define the frequency factor.

Accepted Answer

The frequency factor...

Question 15

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 5.00? The rate will

Accepted Answer

A)   decrease by a factor of 1/25.0.
B)   decrease by a factor of 1/5.00.
C)   increase by a factor of 5.00.
D)   increase by a factor of 25.00.

Question 16

Which of the following statements is FALSE?

Accepted Answer

A)   The half-life of a zero-order reaction is dependent on concentration.
B)   The half-life of a second-order reaction is not dependent on concentration.
C)   The rate of second-order reactions is dependent on concentration.
D)   The rate of a first-order reaction is dependent on concentration.
E)   None of the statements is FALSE.

Question 17

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of disappearance of Cl2 is 4.24 × 10-2 M/s,what is the rate of formation of NO? 2 NO(g) + Cl2(g) → 2 NOCl(g)

Accepted Answer

A)   4.24 × 10-2 M/s
B)   2.12 × 10-2 M/s
C)   1.06 × 10-1 M/s
D)   8.48 × 10-2 M/s
E)   1.61 × 10-2 M/s

Question 18

Determine the rate law and the value of k for the following reaction using the data provided. NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate (M-1s-1) 
0) 10 0.33 1.42
0) 10 0.66 2.84
0) 25 0.66 7.10

Accepted Answer

A)   Rate = 1360 M-2.5s-1[NO2]2.5[O3]
B)   Rate = 227 M-2.5s-1[NO2][O3]2.5
C)   Rate = 43 M-1s-1[NO2][O3]
D)   Rate = 430 M-2s-1[NO2]2[O3]
E)   Rate = 130 M-2s-1[NO2][O3]2

Question 19

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Accepted Answer

A)   0.143 hr
B)   2.28 hr
C)   6.99 hr
D)   22.7 hr

Question 20

Give the characteristic of a first-order reaction having only one reactant.

Accepted Answer

A)   The rate of the reaction is not proportional to the concentration of the reactant.
B)   The rate of the reaction is proportional to the square of the concentration of the reactant.
C)   The rate of the reaction is proportional to the square root of the concentration of the reactant.
D)   The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.
E)   The rate of the reaction is directly proportional to the concentration of the reactant.

Exam 14: Chemical Kinetics

Give the characteristic of a first-order reaction having only one reactant.

Correct Answer
verified

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [N₂]. N₂(g) + 3 H₂(g) → 2 NH₃(g)

Correct Answer
verified

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

Correct Answer
verified

Define activation energy.

Correct Answer
verified
Activation energy is the energ...
View Answer

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Correct Answer
verified

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 5.00? The rate will

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [H₂]. N₂(g) + 3 H₂(g) → 2 NH₃(g)

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided. NO₂(g) + O₃(g) → NO₃(g) + O₂(g) [NO₂]_i(M) [O₃]_i (M) Initial Rate (M^-1s^-1) 0) 10 0.33 1.42 0) 10 0.66 2.84 0) 25 0.66 7.10

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of disappearance of Cl₂ is 4.24 × 10^-2 M/s,what is the rate of formation of NO? 2 NO(g) + Cl₂(g) → 2 NOCl(g)

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2 SO₂(g) + O₂(g) → 2 SO₃(g)

Correct Answer
verified

What is the difference between average reaction rate and instantaneous reaction rate?

Correct Answer
verified
An average reaction rate is determined u...
View Answer

Correct Answer
verified

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 95.0°C if E_a = 55.5 kJ/mol?

Correct Answer
verified

Define the frequency factor.

Correct Answer
verified
The frequency factor...
View Answer

Which of the following statements is FALSE?

Correct Answer
verified

Which of the following represents the equation for a first-order half-life?

Correct Answer
verified

The following reaction is first order,C₂H₆ → 2 CH₃.If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K,how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0.20 mol in the same container?

Correct Answer
verified

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰[B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct Answer
verified

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

Correct Answer
verified

Exam 14: Chemical Kinetics

Give the characteristic of a first-order reaction having only one reactant.

Correct AnswerverifiedShow Answer

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [N2]. N2(g) + 3 H2(g) → 2 NH3(g)

Correct AnswerverifiedShow Answer

The first-order reaction,SO2Cl2 → SO2 + Cl2,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Correct AnswerverifiedShow Answer

Define activation energy.

Correct AnswerverifiedActivation energy is the energ...View AnswerShow Answer

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Correct AnswerverifiedShow Answer

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 5.00? The rate will

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [H2]. N2(g) + 3 H2(g) → 2 NH3(g)

Correct AnswerverifiedShow Answer

Determine the rate law and the value of k for the following reaction using the data provided. NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate (M-1s-1) 0) 10 0.33 1.42 0) 10 0.66 2.84 0) 25 0.66 7.10

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of disappearance of Cl2 is 4.24 × 10-2 M/s,what is the rate of formation of NO? 2 NO(g) + Cl2(g) → 2 NOCl(g)

Correct AnswerverifiedShow Answer

Given the following balanced equation,determine the rate of reaction with respect to [O2]. 2 SO2(g) + O2(g) → 2 SO3(g)

Correct AnswerverifiedShow Answer

What is the difference between average reaction rate and instantaneous reaction rate?

Correct AnswerverifiedAn average reaction rate is determined u...View AnswerShow Answer

Correct AnswerverifiedShow Answer

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 95.0°C if Ea = 55.5 kJ/mol?

Correct AnswerverifiedShow Answer

Define the frequency factor.

Correct AnswerverifiedThe frequency factor...View AnswerShow Answer

Which of the following statements is FALSE?

Correct AnswerverifiedShow Answer

Which of the following represents the equation for a first-order half-life?

Correct AnswerverifiedShow Answer

The following reaction is first order,C2H6 → 2 CH3.If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K,how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.20 mol in the same container?

Correct AnswerverifiedShow Answer

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0[B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct AnswerverifiedShow Answer

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 1010 s-1,what is the rate constant for this reaction at 298 K?

Correct AnswerverifiedShow Answer

Correct Answer
verified

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [N₂]. N₂(g) + 3 H₂(g) → 2 NH₃(g)

Correct Answer
verified

The first-order reaction,SO₂Cl₂ → SO₂ + Cl₂,has a half-life of 8.75 hours at 593 K.How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

Correct Answer
verified

Correct Answer
verified
Activation energy is the energ...
View Answer

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Correct Answer
verified

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 5.00? The rate will

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [H₂]. N₂(g) + 3 H₂(g) → 2 NH₃(g)

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided. NO₂(g) + O₃(g) → NO₃(g) + O₂(g) [NO₂]_i(M) [O₃]_i (M) Initial Rate (M^-1s^-1) 0) 10 0.33 1.42 0) 10 0.66 2.84 0) 25 0.66 7.10

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of disappearance of Cl₂ is 4.24 × 10^-2 M/s,what is the rate of formation of NO? 2 NO(g) + Cl₂(g) → 2 NOCl(g)

Correct Answer
verified

Given the following balanced equation,determine the rate of reaction with respect to [O₂]. 2 SO₂(g) + O₂(g) → 2 SO₃(g)

Correct Answer
verified

Correct Answer
verified
An average reaction rate is determined u...
View Answer

Correct Answer
verified

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 95.0°C if E_a = 55.5 kJ/mol?

Correct Answer
verified

Correct Answer
verified
The frequency factor...
View Answer

Correct Answer
verified

Correct Answer
verified

The following reaction is first order,C₂H₆ → 2 CH₃.If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K,how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0.20 mol in the same container?

Correct Answer
verified

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰[B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

Correct Answer
verified

If the activation energy for a given compound is found to be 42.0 kJ/mol,with a frequency factor of 8.0 × 10¹⁰ s^-1,what is the rate constant for this reaction at 298 K?

Correct Answer
verified