Question 1

The mechanism for the reaction 2H2O2(aq)   2H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be: Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the molecularity of the rate-determining step? A)  zeromolecular B)  unimolecular C)  bimolecular D)  termolecular E)  More information is needed to answer this question." class="answers-bank-image d-inline" rel="preload" > )  + O2(g)  in the presence of I-(aq)  is proposed to be: Step 1: H2O2(aq)  + I-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be: Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the molecularity of the rate-determining step? A)  zeromolecular B)  unimolecular C)  bimolecular D)  termolecular E)  More information is needed to answer this question." class="answers-bank-image d-inline" rel="preload" > )  + OI-(aq) 
(slow) 
Step 2: H2O2(aq)  + OI-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be: Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the molecularity of the rate-determining step? A)  zeromolecular B)  unimolecular C)  bimolecular D)  termolecular E)  More information is needed to answer this question." class="answers-bank-image d-inline" rel="preload" > )  + O2(g)  + I-(aq) 
(fast) 
What is the molecularity of the rate-determining step?

Accepted Answer

A)   zeromolecular
B)   unimolecular
C)   bimolecular
D)   termolecular
E)   More information is needed to answer this question.

Question 2

Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) 
T (K) 
2) 04  10-4
250
6) 78  10-3
400

Accepted Answer

A)   2.3
B)   5.3
C)   0.99
D)   0.63
E)   0.85

Question 3

The following energy profiles for four different reactions are shown. Which reaction is the most endothermic?

Accepted Answer

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

Question 4

The energy profiles for four different reactions are shown. Which of the reactions will have the smallest rate constant?

Accepted Answer

A)   
B)   
C)   
D)

Question 5

The difference between an average rate and an instantaneous rate is __________

Accepted Answer

A)   the average rate is taken over a larger time period.
B)   the instantaneous rate is taken from the slope of the curve at a specific time.
C)   they are not different if the time interval chosen is small enough.
D)   All the above are correct.

Question 6

The mechanism for the reaction 2H2O2(aq)   2H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the rate law for the overall reaction? A)  Rate = k[H2O2] B)  Rate = k[H2O2]2 C)  Rate = k[H2O2][I-] D)  Rate = k[H2O2][OI-] E)  Rate = k[H2O2]2[I-]/[H2O]" class="answers-bank-image d-inline" rel="preload" > )  + O2(g)  in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the rate law for the overall reaction? A)  Rate = k[H2O2] B)  Rate = k[H2O2]2 C)  Rate = k[H2O2][I-] D)  Rate = k[H2O2][OI-] E)  Rate = k[H2O2]2[I-]/[H2O]" class="answers-bank-image d-inline" rel="preload" > )  + OI-(aq) 
(slow) 
Step 2: H2O2(aq)  + OI-(aq)   H2O( 2O2(aq)   2H2O(   )  + O2(g)  in the presence of I-(aq)  is proposed to be Step 1: H2O2(aq)  + I-(aq)   H2O(   )  + OI-(aq)  (slow)  Step 2: H2O2(aq)  + OI-(aq)   H2O(   )  + O2(g)  + I-(aq)  (fast)  What is the rate law for the overall reaction? A)  Rate = k[H2O2] B)  Rate = k[H2O2]2 C)  Rate = k[H2O2][I-] D)  Rate = k[H2O2][OI-] E)  Rate = k[H2O2]2[I-]/[H2O]" class="answers-bank-image d-inline" rel="preload" > )  + O2(g)  + I-(aq) 
(fast) 
What is the rate law for the overall reaction?

Accepted Answer

A)   Rate = k[H2O2]
B)   Rate = k[H2O2]2
C)   Rate = k[H2O2][I-]
D)   Rate = k[H2O2][OI-]
E)   Rate = k[H2O2]2[I-]/[H2O]

Question 7

The following figure shows Arrhenius plots for four different reactions. Which reaction has the lowest activation energy?

Accepted Answer

A)   dashed
B)   dotted
C)   dash-dot
D)   solid

Question 8

For the reaction 2A + 3B F1F1F1S1F1F1F10 4C + 5D, the rate of the reaction in terms of F1F1F1S1F1F1F10A would be written as __________.

Accepted Answer

- <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> F1F1F1S...

Question 9

Large cities often issue ozone advisories. At what time of year would an advisory be likely to occur most often?

Accepted Answer

A)   winter
B)   spring
C)   summer
D)   fall
E)   No season should have more advisories than another.

Question 10

If the rate of the reaction: 2O3(g)   3O2(g) 
Is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?

Accepted Answer

A)   1.38 M
B)   4.13 M
C)   0.69 M
D)   0.25 M
E)   0.46 M

Question 11

In a rate law, the partial orders are determined by __________

Accepted Answer

A)   the reactant concentrations.
B)   the stoichiometric coefficients.
C)   the product concentrations.
D)   experiment.
E)   the difference between the forward and reverse rates.

Question 12

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H2(g)  + 2 NO(g)   N2O(g)  + H2O(g) 
Step 2: N2O(g)  + H2(g)   N2(g)  + H2O(g) 
What is the molecularity of Step 1?

Accepted Answer

A)   unimolecular
B)   bimolecular
C)   termolecular
D)   zero molecular (spontaneous) 
E)   More information is needed to answer this question.

Question 13

The energy profiles for four different reactions are shown. Which reaction requires the most energetic collisions to reach the transition state?

Accepted Answer

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

Question 14

A catalyst that is in the same phase as the reactants and products is a(n)  __________ catalyst.

Accepted Answer

A)   heterogeneous
B)   homogeneous
C)   inherent
D)   directed
E)   endogenous

Question 15

The greatest NO concentration is observed __________

Accepted Answer

A)   in the morning before rush hour.
B)   in the morning just after rush hour.
C)   in midmorning.
D)   at noon.
E)   in midafternoon.

Question 16

For the reaction 2A + 3B F1F1F1S1F1F1F10 4C + 5D, the rate of the reaction in terms of F1F1F1S1F1F1F10D would be written as __________.

Accepted Answer

+ <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> F1F1F1S...

Question 17

Ammonia gas (NH3)  is produced from hydrogen and nitrogen gas according to the following reaction: 3H2(g)  + N2(g)   2NH3(g) 
If the rate of production of ammonia is R(NH3) , what is the rate of loss of hydrogen and nitrogen gas, respectively?

Accepted Answer

A)   -R(H2)  = 2/3 R(NH3) ; -R(N2)  = 1/2 R(NH3) 
B)   -R(H2)  = 3/2 R(NH3) ; -R(N2)  = 2 R(NH3) 
C)   -R(H2)  = 3/2 R(NH3) ; -R(N2)  = 1/2 R(NH3) 
D)   -R(H2)  = 2/3 R(NH3) ; -R(N2)  = 2 R(NH3) 
E)   -R(H2)  = R(NH3) ; -R(N2)  = R(NH3)

Question 18

The linear form of __________ is very useful as it allows us to calculate the activation energy and the frequency factor.

Accepted Answer

A)   the Boltzmann equation
B)   the Arrhenius equation
C)   Planck's equation
D)   the rate law
E)   the integrated rate law

Question 19

The second-order reaction A + B  C will obey pseudo first-order kinetics when __________

Accepted Answer

A)   the concentrations of A and B are both small.
B)   the concentration of one of the reactants does not change.
C)   the concentration of C is large.
D)   the concentrations of A and B are both large.
E)   a catalyst changes the mechanism to a first-order reaction.

Question 20

The second-order reaction A  B is found to have a rate constant of 0.978 M-1s-1. What is the half-life of this reaction when [A]0 = 0.0300 M?

Accepted Answer

A)   0.0293 s
B)   0.710 s
C)   34.1 s
D)   60.1 s
E)   24.3 s

Exam 15: Chemical Kinetics

Correct Answer
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The following figure shows Arrhenius plots for four different reactions. Which reaction has the lowest activation energy?

Correct Answer
verified

The second-order reaction A + B  C will obey pseudo first-order kinetics when __________

Correct Answer
verified

In a rate law, the partial orders are determined by __________

Correct Answer
verified

The difference between an average rate and an instantaneous rate is __________

Correct Answer
verified

The energy profiles for four different reactions are shown. Which of the reactions will have the smallest rate constant?

Correct Answer
verified

For the reaction 2A + 3B  4C + 5D, the rate of the reaction in terms of D would be written as __________.

Correct Answer
verified
+ F1F1F1S...
View Answer

If the rate of the reaction: 2O₃(g)  3O₂(g) Is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?

Correct Answer
verified

Ammonia gas (NH₃) is produced from hydrogen and nitrogen gas according to the following reaction: 3H₂(g) + N₂(g)  2NH₃(g) If the rate of production of ammonia is R(NH₃) , what is the rate of loss of hydrogen and nitrogen gas, respectively?

Correct Answer
verified

For the reaction 2A + 3B  4C + 5D, the rate of the reaction in terms of A would be written as __________.

Correct Answer
verified
- F1F1F1S...
View Answer

The greatest NO concentration is observed __________

Correct Answer
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The energy profiles for four different reactions are shown. Which reaction requires the most energetic collisions to reach the transition state?

Correct Answer
verified

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g)  N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g)  N₂(g) + H₂O(g) What is the molecularity of Step 1?

Correct Answer
verified

Large cities often issue ozone advisories. At what time of year would an advisory be likely to occur most often?

Correct Answer
verified

Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) T (K) 2) 04  10^-⁴ 250 6) 78  10^-³ 400

Correct Answer
verified

The linear form of __________ is very useful as it allows us to calculate the activation energy and the frequency factor.

Correct Answer
verified

The following energy profiles for four different reactions are shown. Which reaction is the most endothermic?

Correct Answer
verified

The second-order reaction A  B is found to have a rate constant of 0.978 M^-¹s^-¹. What is the half-life of this reaction when [A]₀ = 0.0300 M?

Correct Answer
verified

The mechanism for the reaction 2H₂O₂(aq)  2H₂O( ) + O₂(g) in the presence of I^-(aq) is proposed to be Step 1: H₂O₂(aq) + I^-(aq)  H₂O( ) + OI^-(aq) (slow) Step 2: H₂O₂(aq) + OI^-(aq)  H₂O( ) + O₂(g) + I^-(aq) (fast) What is the rate law for the overall reaction?

Correct Answer
verified

A catalyst that is in the same phase as the reactants and products is a(n) __________ catalyst.

Correct Answer
verified

Exam 15: Chemical Kinetics

The mechanism for the reaction 2H2O2(aq)  2H2O( ) + O2(g) in the presence of I-(aq) is proposed to be: Step 1: H2O2(aq) + I-(aq)  H2O( ) + OI-(aq) (slow) Step 2: H2O2(aq) + OI-(aq)  H2O( ) + O2(g) + I-(aq) (fast) What is the molecularity of the rate-determining step?

Correct AnswerverifiedShow Answer

The following figure shows Arrhenius plots for four different reactions. Which reaction has the lowest activation energy?

Correct AnswerverifiedShow Answer

The second-order reaction A + B  C will obey pseudo first-order kinetics when __________

Correct AnswerverifiedShow Answer

In a rate law, the partial orders are determined by __________

Correct AnswerverifiedShow Answer

The difference between an average rate and an instantaneous rate is __________

Correct AnswerverifiedShow Answer

The energy profiles for four different reactions are shown. Which of the reactions will have the smallest rate constant?

Correct AnswerverifiedShow Answer

For the reaction 2A + 3B  4C + 5D, the rate of the reaction in terms of D would be written as __________.

Correct Answerverified+ F1F1F1S...View AnswerShow Answer

If the rate of the reaction: 2O3(g)  3O2(g) Is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?

Correct AnswerverifiedShow Answer

Ammonia gas (NH3) is produced from hydrogen and nitrogen gas according to the following reaction: 3H2(g) + N2(g)  2NH3(g) If the rate of production of ammonia is R(NH3) , what is the rate of loss of hydrogen and nitrogen gas, respectively?

Correct AnswerverifiedShow Answer

For the reaction 2A + 3B  4C + 5D, the rate of the reaction in terms of A would be written as __________.

Correct Answerverified- F1F1F1S...View AnswerShow Answer

The greatest NO concentration is observed __________

Correct AnswerverifiedShow Answer

The energy profiles for four different reactions are shown. Which reaction requires the most energetic collisions to reach the transition state?

Correct AnswerverifiedShow Answer

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H2(g) + 2 NO(g)  N2O(g) + H2O(g) Step 2: N2O(g) + H2(g)  N2(g) + H2O(g) What is the molecularity of Step 1?

Correct AnswerverifiedShow Answer

Large cities often issue ozone advisories. At what time of year would an advisory be likely to occur most often?

Correct AnswerverifiedShow Answer

Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) T (K) 2) 04  10-4 250 6) 78  10-3 400

Correct AnswerverifiedShow Answer

The linear form of __________ is very useful as it allows us to calculate the activation energy and the frequency factor.

Correct AnswerverifiedShow Answer

The following energy profiles for four different reactions are shown. Which reaction is the most endothermic?

Correct AnswerverifiedShow Answer

The second-order reaction A  B is found to have a rate constant of 0.978 M-1s-1. What is the half-life of this reaction when [A]0 = 0.0300 M?

Correct AnswerverifiedShow Answer

The mechanism for the reaction 2H2O2(aq)  2H2O( ) + O2(g) in the presence of I-(aq) is proposed to be Step 1: H2O2(aq) + I-(aq)  H2O( ) + OI-(aq) (slow) Step 2: H2O2(aq) + OI-(aq)  H2O( ) + O2(g) + I-(aq) (fast) What is the rate law for the overall reaction?

Correct AnswerverifiedShow Answer

A catalyst that is in the same phase as the reactants and products is a(n) __________ catalyst.

Correct AnswerverifiedShow Answer

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+ F1F1F1S...
View Answer

If the rate of the reaction: 2O₃(g)  3O₂(g) Is 0.250 M/s over the first 5.50 s, how much oxygen will form during this time?

Correct Answer
verified

Ammonia gas (NH₃) is produced from hydrogen and nitrogen gas according to the following reaction: 3H₂(g) + N₂(g)  2NH₃(g) If the rate of production of ammonia is R(NH₃) , what is the rate of loss of hydrogen and nitrogen gas, respectively?

Correct Answer
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Correct Answer
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- F1F1F1S...
View Answer

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A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: H₂(g) + 2 NO(g)  N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g)  N₂(g) + H₂O(g) What is the molecularity of Step 1?

Correct Answer
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Correct Answer
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Given the following data for the reaction A  B, determine the frequency factor, A, of the reaction. k (M/s) T (K) 2) 04  10^-⁴ 250 6) 78  10^-³ 400

Correct Answer
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Correct Answer
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Correct Answer
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The second-order reaction A  B is found to have a rate constant of 0.978 M^-¹s^-¹. What is the half-life of this reaction when [A]₀ = 0.0300 M?

Correct Answer
verified

The mechanism for the reaction 2H₂O₂(aq)  2H₂O( ) + O₂(g) in the presence of I^-(aq) is proposed to be Step 1: H₂O₂(aq) + I^-(aq)  H₂O( ) + OI^-(aq) (slow) Step 2: H₂O₂(aq) + OI^-(aq)  H₂O( ) + O₂(g) + I^-(aq) (fast) What is the rate law for the overall reaction?

Correct Answer
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Correct Answer
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