Question 1

A reaction is found to have an activation energy of 108 kJ mol-1. If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K, what is the rate constant at 366 K?

Accepted Answer

A)  12 s-1
B)  1.7 s-1
C)  0.58 s-1
D)  5.4 × 10-5 s-1
E)  1.9 × 10-4 s-1

Question 2

Identify a heterogeneous catalyst.

Accepted Answer

A)  CFCs with ozone
B)  Pd in H2 gas
C)  KI dissolved in H2O2
D)  H2SO4 with concentrated HCl
E)  H3PO4 with an alcohol

Question 3

Identify the rate-determining step.

Accepted Answer

A)  the slowest step
B)  the faster step
C)  the fast step
D)  always the last step
E)  always the second step

Question 4

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1) 
0.093 4.84 × 10-4
0.186 9.67 × 10-4
0.279 1.45 × 10-3

Accepted Answer

A)  Rate = 5.6 × 10-2 M-1 s-1[N2O5]2
B)  Rate = 6.0 × 10-1 M-2 s-1[N2O5]3
C)  Rate = 1.6 × 10-3 M1/2 s-1[N2O5]1/2
D)  Rate = 1.7 × 10-2 M-1/2 s-1[N2O5]3/2
E)  Rate = 5.2 × 10⁻3 s-1[N2O5]

Question 5

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Accepted Answer

A)  83.4 g
B)  16.6 g
C)  50.0 g
D)  36.6 g
E)  63.4 g

Question 6

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Accepted Answer

A)  3
B)  1
C)  1.75
D)  2.75
E)  2

Question 7

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

Accepted Answer

A)  3.56 × 10-3 mol L-1 s-1
B)  1.19 × 10-3 mol L-1 s-1
C)  1.78 × 10-3 mol L-1 s-1
D)  1.42 × 10-2 mol L-1 s-1
E)  7.12 × 10-3 mol L-1 s-1

Question 8

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 6.10 × 1014 s-1 and a rate constant of 13.0 s-1 at 320 K.

Accepted Answer

A)  62.8 kJ mol-1
B)  83.8 kJ mol-1
C)  41.3 kJ mol-1
D)  97.9 kJ mol-1
E)  106 kJ mol-1

Question 9

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2O3(g) → 3O2(g)

Accepted Answer

A)  Rate = - 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
B)  Rate = - 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
C)  Rate = + 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
D)  Rate = + 2]. 2O3(g) → 3O2(g)  
A)  Rate = -   
B)  Rate = -     
C)  Rate = +     
D)  Rate = +   
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
E)  It is not possible to determine the answer without more information.

Question 10

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2(g) → SO2(g) + Cl2(g) 
The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 is ________ atm.

Accepted Answer

A)  0.76
B)  2.2
C)  0.98
D)  0.29
E)  1.4 × 105

Question 11

For the first-order reaction, 2N2O(g) → 2N2(g) + O2(g) , what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00 L reaction vessel?

Accepted Answer

A)  1.6 × 10-2 mol L-1
B)  3.1 × 10-2 mol L-1
C)  6.2 × 10-2 mol L-1
D)  1.2 × 10-1 mol L-1

Question 12

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) → 2NO2(g) [NO]i (M) [O2]i (M) Initial Rate (M-1 s-1) 
0.030 0.0055 8.55 × 10-3
0.030 0.0110 1.71 × 10-2
0.060 0.0055 3.42 × 10-2

Accepted Answer

A)  Rate = 57 M-1 s-1[NO][O2]
B)  Rate = 3.8 M-1/2 s-1[NO][O2]1/2
C)  Rate = 3.1 × 105 M-3 s-1[NO]2[O2]2
D)  Rate = 1.7 × 103 M-2 s-1[NO]2[O2]
E)  Rate = 9.4 × 103 M-2 s-1[NO][O2]2

Question 13

Which of the following represents the integrated rate law for a zeroth-order reaction?

Accepted Answer

A)   t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = -kt
B)   t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > - t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = kt
C)  [A]t - [A]0 = -kt
D)  k = Ae(-Ea/RT) 
E)   t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > = t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > t - [A]0 = -kt 
D)  k = Ae(-Ea/RT)  
E)     =     + lnA" class="answers-bank-image d-inline" rel="preload" > + lnA

Question 14

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K. What is the rate constant at 314 K?

Accepted Answer

A)  6.15 s-1
B)  2.08 s-1
C)  7.68 s-1
D)  9.80 s-1
E)  4.00 s-1

Question 15

The second-order reaction 2Mn(CO) 5 → Mn2(CO) 10 has a rate constant equal to 3.0 × 109 L mol-1 s-1 at 25 °C. If the initial concentration of Mn(CO) 5 is 2.0 × 10-5 mol L-1, how long will it take for 90.% of the reactant to disappear?

Accepted Answer

A)  6.7 × 10-16 s
B)  7.4 × 10-15 s
C)  1.5 × 10-4 s
D)  6.0 × 103 s

Question 16

Given the following balanced equation, determine the rate of reaction with respect to [O3]. 2O3(g) → 3O2(g)

Accepted Answer

A)  Rate = - 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
B)  Rate = - 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
C)  Rate = + 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
D)  Rate = + 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" > 3]. 2O3(g) → 3O2(g)  
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information." class="answers-bank-image d-inline" rel="preload" >
E)  It is not possible to determine the answer without more information.

Question 17

If the activation energy for a given compound is found to be 42.0 kJ mol-1 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 × 10 5 s-1
E)  3.5 × 103 s-1

Question 18

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 mol L-1, what is the concentration of N2O after 9.6 s?

Accepted Answer

A)  7.4 × 10-3 mol L-1
B)  1.0 × 10-3 mol L-1
C)  1.4 × 10-3 mol L-1
D)  3.6 × 10-3 mol L-1
E)  8.7 × 10-3 mol L-1

Question 19

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 mol L-1, what is the concentration of N2O5 after 12.5 minutes?

Accepted Answer

A)  0.124 mol L-1
B)  0.805 mol L-1
C)  2.82 mol L-1
D)  0.355 mol L-1
E)  0.174 mol L-1

Question 20

What is a catalyst and what function does it serve?

Accepted Answer

A catalyst is a substance that is not us...

Exam 13: Chemical Kinetics

Which of the following represents the integrated rate law for a zeroth-order reaction?

Correct Answer
verified

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1. If the initial concentration of N₂O is 10.9 mol L^-1, what is the concentration of N₂O after 9.6 s?

Correct Answer
verified

A reaction with an activation energy of 34.0 kJ mol^-1 has a rate constant of 26.8 s^-1 at 354 K. What is the rate constant at 314 K?

Correct Answer
verified

The second-order reaction 2Mn(CO) ₅ → Mn₂(CO) ₁₀ has a rate constant equal to 3.0 × 10⁹ L mol^-1 s^-1 at 25 °C. If the initial concentration of Mn(CO) ₅ is 2.0 × 10^-5 mol L^-1, how long will it take for 90.% of the reactant to disappear?

Correct Answer
verified

For the first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00 L reaction vessel?

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1s^-1) 0.093 4.84 × 10^-4 0.186 9.67 × 10^-4 0.279 1.45 × 10^-3

Correct Answer
verified

Identify a heterogeneous catalyst.

Correct Answer
verified

Identify the rate-determining step.

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O₂(g) → 2NO₂(g) [NO]_i(M) [O₂]_i (M) Initial Rate (M^-1s^-1) 0.030 0.0055 8.55 × 10^-3 0.030 0.0110 1.71 × 10^-2 0.060 0.0055 3.42 × 10^-2

Correct Answer
verified

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2O₃(g) → 3O₂(g)

Correct Answer
verified

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1. If the initial concentration of N₂O₅ is 2.88 mol L^-1, what is the concentration of N₂O₅ after 12.5 minutes?

Correct Answer
verified

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Correct Answer
verified

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

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

Correct Answer
verified

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 6.10 × 10¹⁴ s^-1 and a rate constant of 13.0 s^-1 at 320 K.

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. 2O₃(g) → 3O₂(g)

Correct Answer
verified

What is a catalyst and what function does it serve?

Correct Answer
verified
A catalyst is a substance that is not us...
View Answer

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Correct Answer
verified

A reaction is found to have an activation energy of 108 kJ mol^-1. If the rate constant for this reaction is 4.60 × 10^-6 s^-1 at 275 K, what is the rate constant at 366 K?

Correct Answer
verified

Exam 13: Chemical Kinetics

Which of the following represents the integrated rate law for a zeroth-order reaction?

Correct AnswerverifiedShow Answer

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 mol L-1, what is the concentration of N2O after 9.6 s?

Correct AnswerverifiedShow Answer

A reaction with an activation energy of 34.0 kJ mol-1 has a rate constant of 26.8 s-1 at 354 K. What is the rate constant at 314 K?

Correct AnswerverifiedShow Answer

The second-order reaction 2Mn(CO) 5 → Mn2(CO) 10 has a rate constant equal to 3.0 × 109 L mol-1 s-1 at 25 °C. If the initial concentration of Mn(CO) 5 is 2.0 × 10-5 mol L-1, how long will it take for 90.% of the reactant to disappear?

Correct AnswerverifiedShow Answer

For the first-order reaction, 2N2O(g) → 2N2(g) + O2(g) , what is the concentration of N2O after 3 half-lives if 0.25 mol of N2O is initially placed into a 1.00 L reaction vessel?

Correct AnswerverifiedShow Answer

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1) 0.093 4.84 × 10-4 0.186 9.67 × 10-4 0.279 1.45 × 10-3

Correct AnswerverifiedShow Answer

Identify a heterogeneous catalyst.

Correct AnswerverifiedShow Answer

Identify the rate-determining step.

Correct AnswerverifiedShow Answer

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) → 2NO2(g) [NO]i (M) [O2]i (M) Initial Rate (M-1 s-1) 0.030 0.0055 8.55 × 10-3 0.030 0.0110 1.71 × 10-2 0.060 0.0055 3.42 × 10-2

Correct AnswerverifiedShow Answer

SO2Cl2 decomposes in the gas phase by the reaction SO2Cl2(g) → SO2(g) + Cl2(g) The reaction is first order in SO2Cl2 and the rate constant is 3.0 × 10-6 s-1at 600 K. A vessel is charged with 2.4 atm of SO2Cl2 at 600 K. The partial pressure of SO2Cl2 at 3.0 × 105 is ________ atm.

Correct AnswerverifiedShow Answer

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 2O3(g) → 3O2(g)

Correct AnswerverifiedShow Answer

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 mol L-1, what is the concentration of N2O5 after 12.5 minutes?

Correct AnswerverifiedShow Answer

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

Correct AnswerverifiedShow Answer

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 6.10 × 1014 s-1 and a rate constant of 13.0 s-1 at 320 K.

Correct AnswerverifiedShow Answer

Given the following balanced equation, determine the rate of reaction with respect to [O3]. 2O3(g) → 3O2(g)

Correct AnswerverifiedShow Answer

What is a catalyst and what function does it serve?

Correct AnswerverifiedA catalyst is a substance that is not us...View AnswerShow Answer

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Correct AnswerverifiedShow Answer

A reaction is found to have an activation energy of 108 kJ mol-1. If the rate constant for this reaction is 4.60 × 10-6 s-1 at 275 K, what is the rate constant at 366 K?

Correct AnswerverifiedShow Answer

Correct Answer
verified

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1. If the initial concentration of N₂O is 10.9 mol L^-1, what is the concentration of N₂O after 9.6 s?

Correct Answer
verified

A reaction with an activation energy of 34.0 kJ mol^-1 has a rate constant of 26.8 s^-1 at 354 K. What is the rate constant at 314 K?

Correct Answer
verified

The second-order reaction 2Mn(CO) ₅ → Mn₂(CO) ₁₀ has a rate constant equal to 3.0 × 10⁹ L mol^-1 s^-1 at 25 °C. If the initial concentration of Mn(CO) ₅ is 2.0 × 10^-5 mol L^-1, how long will it take for 90.% of the reactant to disappear?

Correct Answer
verified

For the first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , what is the concentration of N₂O after 3 half-lives if 0.25 mol of N₂O is initially placed into a 1.00 L reaction vessel?

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1s^-1) 0.093 4.84 × 10^-4 0.186 9.67 × 10^-4 0.279 1.45 × 10^-3

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O₂(g) → 2NO₂(g) [NO]_i(M) [O₂]_i (M) Initial Rate (M^-1s^-1) 0.030 0.0055 8.55 × 10^-3 0.030 0.0110 1.71 × 10^-2 0.060 0.0055 3.42 × 10^-2

Correct Answer
verified

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [O₂]. 2O₃(g) → 3O₂(g)

Correct Answer
verified

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1. If the initial concentration of N₂O₅ is 2.88 mol L^-1, what is the concentration of N₂O₅ after 12.5 minutes?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

Correct Answer
verified

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 6.10 × 10¹⁴ s^-1 and a rate constant of 13.0 s^-1 at 320 K.

Correct Answer
verified

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. 2O₃(g) → 3O₂(g)

Correct Answer
verified

Correct Answer
verified
A catalyst is a substance that is not us...
View Answer

Correct Answer
verified

A reaction is found to have an activation energy of 108 kJ mol^-1. If the rate constant for this reaction is 4.60 × 10^-6 s^-1 at 275 K, what is the rate constant at 366 K?

Correct Answer
verified