Question 1

From the following concentration versus time plot for four different reactions, which has the greatest instantaneous rate of disappearance at the time indicated by the arrow?

Accepted Answer

A)  I
B)  II
C)  III
D)  IV
E)  All have the same rate.

Question 2

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 3

If the rate of the reaction:  is 0.250 M/s over the first 5.50 s, how much ozone will be consumed during this time?

Accepted Answer

The answer of If the rate of the reaction: ...

Question 4

Which point in the reaction profile below represents an intermediate?

Accepted Answer

A)  II and IV
B)  II only
C)  III
D)  IV only
E)  V

Question 5

Which statement A-D regarding the reaction described by the energy profile below is not correct?

Accepted Answer

A)  The rate constant for the reverse reaction is smaller than the rate constant for the forward reaction.
B)  This reaction has two transition states.
C)  An intermediate is formed in this reaction.
D)  The rate-determining step is the first step.
E)  Statements A-D are all correct.

Question 6

Using the reaction shown below, which statement is correct?

Accepted Answer

A)  The concentration of all compounds are changing by the same amount at all times.
B)  The HCl concentration increases at the same rate as the concentration of iodine.
C)  The concentration of hydrogen decreases at the same rate as the concentration of ICl.
D)  The concentration of HCl increases twice as fast as the concentration of iodine.
E)  None of these statements is correct.

Question 7

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1:  Step 2:  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 8

Which of the following plots indicates that the reaction is second order?

Accepted Answer

A)   
B)   
C)   
D)

Question 9

For the rate law Rate F1F1F1S1F1F1F10 k[A]1/2[B], the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

Accepted Answer

Question 10

What is the predicted rate law for the following mechanism for the reduction of nitrogen in NO by hydrogen? Step 1:  k[H2][NO] B) Rate  k[H2]2[NO] C) Rate  k[H2][NO]2 D) Rate  k[H2]2[NO]2 E) More information is needed to answer this question." class="answers-bank-image d-inline" rel="preload" > (slow) 
Step 2:  k[H2][NO] B) Rate  k[H2]2[NO] C) Rate  k[H2][NO]2 D) Rate  k[H2]2[NO]2 E) More information is needed to answer this question." class="answers-bank-image d-inline" rel="preload" > (fast) 
What is the rate law?

Accepted Answer

A)  Rate  k[H2][NO]
B)  Rate  k[H2]2[NO]
C)  Rate  k[H2][NO]2
D)  Rate  k[H2]2[NO]2
E)  More information is needed to answer this question.

Question 11

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

Accepted Answer

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

Question 12

If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2? 2?   A) 0.173 M/s B) 0.345 M/s C) 0.690 M/s D) 245 M/s E) 0.518 M/s" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  0.173 M/s
B)  0.345 M/s
C)  0.690 M/s
D)  245 M/s
E)  0.518 M/s

Question 13

For the reaction 2A F1F1F1S1F1F1F10 3B  F1F1F1S1F1F1F104C F1F1F1S1F1F1F10 5D, the rate of the reaction in terms of F1F1F1S1F1F1F10A would be written as ________.

Accepted Answer

<font face="symbol">F1...

Question 14

The second-order reaction A  F1F1F1S1F1F1F10B is found to have a rate constant of 0.978 MF1F1F1S1F1F1F10F1F1F1S1F1F1F101sF1F1F1S1F1F1F101. What is the half-life of this reaction when [A]0 F1F1F1S1F1F1F10 0.0300 MF1F1F1S1F1F1F10?

Accepted Answer

Question 15

The order in which ozone, nitrogen monoxide, and nitrogen dioxide build up in the atmosphere over the course of the day is first ________ then ________ then ________.

Accepted Answer

nitrogen m...

Question 16

The high temperatures in an automobile engine cause nitrogen and oxygen to form noxious nitrogen monoxide. Use the following data on the temperature dependence of the rate constant to determine the activation energy for this reaction. T (K) 
K (M1 s1) 
2,200
1,800
2,400
7,400

Accepted Answer

A)  29 kJ/mol
B)  343 kJ/mol
C)  78 kJ/mol
D)  310 kJ/mol
E)  421 kJ/mol

Question 17

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

Accepted Answer

A)  the average rate is taken over a longer 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 of the above are correct.

Question 18

In a first order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15 seconds if the half-life of the reaction is 3 seconds?

Accepted Answer

A)  8.0  102 M
B)  2.0 M
C)  5.0  102 M
D)  2.5  102 M
E)  1.3  102 M

Question 19

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

Accepted Answer

A)   
B)   
C)   
D)

Question 20

For the rate law Rate  k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

Accepted Answer

A)    k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________. 
A)     
B)     
C)     
D)     
E)  The orders cannot be determined without a chemical reaction." class="answers-bank-image d-inline" rel="preload" >
B)    k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________. 
A)     
B)     
C)     
D)     
E)  The orders cannot be determined without a chemical reaction." class="answers-bank-image d-inline" rel="preload" >
C)    k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________. 
A)     
B)     
C)     
D)     
E)  The orders cannot be determined without a chemical reaction." class="answers-bank-image d-inline" rel="preload" >
D)    k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________. 
A)     
B)     
C)     
D)     
E)  The orders cannot be determined without a chemical reaction." class="answers-bank-image d-inline" rel="preload" >
E)  The orders cannot be determined without a chemical reaction.

Exam 13: Chemical Kinetics: Reactions in the Atmosphere

Which of the following plots indicates that the reaction is second order?

Correct AnswerverifiedShow Answer

Which statement A-D regarding the reaction described by the energy profile below is not correct?

Correct AnswerverifiedShow Answer

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: Step 2: What is the molecularity of step 1?

Correct AnswerverifiedShow Answer

For the rate law Rate  k[A]1/2[B], the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

Correct AnswerverifiedShow Answer

Using the reaction shown below, which statement is correct?

Correct AnswerverifiedShow Answer

Which point in the reaction profile below represents an intermediate?

Correct AnswerverifiedShow Answer

The high temperatures in an automobile engine cause nitrogen and oxygen to form noxious nitrogen monoxide. Use the following data on the temperature dependence of the rate constant to determine the activation energy for this reaction. T (K) K (M1 s1) 2,200 1,800 2,400 7,400

Correct AnswerverifiedShow Answer

What is the predicted rate law for the following mechanism for the reduction of nitrogen in NO by hydrogen? Step 1: (slow) Step 2: (fast) What is the rate law?

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

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

Correct AnswerverifiedShow Answer

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

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

If the rate of the reaction: is 0.250 M/s over the first 5.50 s, how much ozone will be consumed during this time?

Correct AnswerverifiedShow Answer

If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2?

Correct AnswerverifiedShow Answer

For the rate law Rate  k[A][B]1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedF1...View AnswerShow Answer

From the following concentration versus time plot for four different reactions, which has the greatest instantaneous rate of disappearance at the time indicated by the arrow?

Correct AnswerverifiedShow Answer

The order in which ozone, nitrogen monoxide, and nitrogen dioxide build up in the atmosphere over the course of the day is first ________ then ________ then ________.

Correct Answerverifiednitrogen m...View AnswerShow Answer

In a first order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15 seconds if the half-life of the reaction is 3 seconds?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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For the rate law Rate  k[A]^1/2[B], the partial order with respect to A is , the partial order with respect to B is , and the total order is .

Correct Answer
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Correct Answer
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Correct Answer
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The high temperatures in an automobile engine cause nitrogen and oxygen to form noxious nitrogen monoxide. Use the following data on the temperature dependence of the rate constant to determine the activation energy for this reaction. T (K) K (M^¹ s^¹) 2,200 1,800 2,400 7,400

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
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Correct Answer
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If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N₂?

Correct Answer
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For the rate law Rate  k[A][B]^1/2, the partial order with respect to A is , the partial order with respect to B is , and the total order is .

Correct Answer
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F1...
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The order in which ozone, nitrogen monoxide, and nitrogen dioxide build up in the atmosphere over the course of the day is first then then .

Correct Answer
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nitrogen m...
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Correct Answer
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