Question 1

The rate law of a particular reaction was determined to be Rate F1F1F1S1F1F1F10 k. What is the unit of the rate constant for the reaction?

Accepted Answer

A) M/s 
B) 1/(Ms) 
C) 1/(Ms2) 
D) 1/s 
E) Ms 
A) M/s 
B) 1/(Ms) 
C) 1/(Ms2) 
D) 1/s 
E) Ms A

Question 2

If the rate of formation of nitrogen monoxide is 0.413 M/s, what is the rate of disappearance of SO2?

Accepted Answer

A) 0.207 M/s 
B) 0.280 M/s 
C) 0.413 M/s 
D) 0.620 M/s 
E) 1.24 M/s 
A) 0.207 M/s 
B) 0.280 M/s 
C) 0.413 M/s 
D) 0.620 M/s 
E) 1.24 M/s D

Question 3

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

Accepted Answer

A) NO; NO2; O3 
B) NO; O3; NO2 
C) NO2; NO; O3 
D) NO2; O3; NO 
E) O3; NO; NO2 
A) NO; NO2; O3 
B) NO; O3; NO2 
C) NO2; NO; O3 
D) NO2; O3; NO 
E) O3; NO; NO2 A

Question 4

A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1:   Step 2:   Which of the following species is an intermediate?

Accepted Answer

A) Cl 
B) O3 
C) ClO 
D) O2 
E) This mechanism has no intermediates. 
A) Cl 
B) O3 
C) ClO 
D) O2 
E) This mechanism has no intermediates.

Question 5

Given the following data for the reaction A F1F1F1S1F1F1F10 B, determine the activation energy, Ea, of the reaction.
k (M/s)
T (K)
2.04 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104
250
6.78 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103
400

Accepted Answer

Question 6

A scientist conducts an experiment to determine the rate of NO formation in the reaction:   If the initial concentration of N2 was 0.500 M and the concentration of N2 was 0.450 M after 0.100 s, what is the average rate of NO formation?

Accepted Answer

A) 0.500 M/s 
B) 1.00 M/s 
C) 5.00 M/s 
D) 10.0 M/s 
E) 0.250 M/s 
A) 0.500 M/s 
B) 1.00 M/s 
C) 5.00 M/s 
D) 10.0 M/s 
E) 0.250 M/s

Question 7

Given the following data for the reaction A   F1F1F1S1F1F1F10B, determine the activation energy, Ea, of the reaction. k (M/s)
T (K)
0)730
250
0)739
450

Accepted Answer

A) 54.4 J/mol 
B) 6.89 J/mol 
C) 39.9 J/mol 
D) 57.3 J/mol 
E) 374 J/mol 
A) 54.4 J/mol 
B) 6.89 J/mol 
C) 39.9 J/mol 
D) 57.3 J/mol 
E) 374 J/mol

Question 8

A scientist conducts an experiment to determine the rate of the following reaction:   If the initial concentration of NO2 was 0.250 M and the concentration of NO2 was 0.200 M after
0.200 s, what is the average rate of the reaction?

Accepted Answer

Question 9

If the rate of the reaction:   is 0.870 M/s over the first 12.25 s, how much hydrogen sulfide will be consumed during this time?

Accepted Answer

A) 10.66 M 
B) 21.32 M 
C) 5.33 M 
D) 31.98 M 
E) 3.55 M 
A) 10.66 M 
B) 21.32 M 
C) 5.33 M 
D) 31.98 M 
E) 3.55 M

Question 10

The linear form of the Arrhenius equation is very useful, as a plot of ________ versus ________ allows us to calculate the activation energy from the slope and the frequency factor from the intercept.

Accepted Answer

The answer of The linear form of the Arrhenius equation...

Question 11

HI dissociates to form I2 and H2:   If the concentration of HI changes at a rate of F1F1F1S1F1F1F100.45 M/s, what is the rate of appearance of I2(g)?

Accepted Answer

A) 0.90 M/s 
B) 0.45 M/s 
C) 0.23 M/s 
D) 1.00 M/s 
E) 0.13 M/s 
A) 0.90 M/s 
B) 0.45 M/s 
C) 0.23 M/s 
D) 1.00 M/s 
E) 0.13 M/s

Question 12

One reaction that occurs in an automobile catalytic converter is the conversion of nitrogen monoxide to nitrogen and oxygen. How is the rate of this reaction related to the rate at which the concentration of a reactant or product changes? 2NO(g) →N2(g) F1F1F1S1F1F1F10 O2(g)
I. Rate F1F1F1S1F1F1F10   F1F1F1S1F1F1F10
II. Rate F1F1F1S1F1F1F10   F1F1F1S1F1F1F10
III. Rate F1F1F1S1F1F1F10  IV. Rate F1F1F1S1F1F1F10   F1F1F1S1F1F1F10

Accepted Answer

A) I only 
B) II only 
C) III and IV only 
D) I, III, and IV only 
E) II, III, and IV only 
A) I only 
B) II only 
C) III and IV only 
D) I, III, and IV only 
E) II, III, and IV only

Question 13

Which plot would provide the activation energy for a reaction?

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 14

In an elementary step of a reaction mechanism, the molecularities 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. 
A) the reactant concentrations. 
B) the stoichiometric coefficients. 
C) the product concentrations. 
D) experiment. 
E) the difference between the forward and reverse rates.

Question 15

The rate at which popcorn pops was measured at two different temperatures. How many times faster does the popcorn pop at 250°C compared with that at 210°C when the activation energy is 53.8 kJ/mol?

Accepted Answer

A) 2.8 
B) 3.9 
C) 140 
D) 125 
E) 12.7 
A) 2.8 
B) 3.9 
C) 140 
D) 125 
E) 12.7

Question 16

For the following energy profile:
a) identify any reaction intermediates, 
b) identify any transition states, 
c) state the number of steps, 
d) state whether the reaction is endo- or exothermic, 
e) indicate which step is rate determining.

Accepted Answer

a) III is a reaction intermedi

Question 17

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

1.3 F1F1F1

Question 18

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

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 
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 19

For the reaction 2A   F1F1F1S1F1F1F104B F1F1F1S1F1F1F10 3D, the rate of the reaction in terms of F1F1F1S1F1F1F10B would be written as ________

Accepted Answer

A) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
B) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
C) (F1F1F1S1F1F1F10F1F1F1S1F1F1F10   F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
D) (+   F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
E) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
A) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
B) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
C) (F1F1F1S1F1F1F10F1F1F1S1F1F1F10   F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
D) (+   F1F1F1S1F1F1F10   F1F1F1S1F1F1F10) 
E) (F1F1F1S1F1F1F10   F1F1F1S1F1F1F10)

Question 20

The following figure shows Arrhenius plots for four different reactions. Which reaction has the largest frequency factor?

Accepted Answer

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

Exam 13: Chemical Kinetics: Reactions in the Atmosphere

The rate law of a particular reaction was determined to be Rate  k. What is the unit of the rate constant for the reaction?

If the rate of formation of nitrogen monoxide is 0.413 M/s, what is the rate of disappearance of SO2?

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

A proposed mechanism for the decomposition of ozone in the atmosphere is: Step 1: Step 2: Which of the following species is an intermediate?

Given the following data for the reaction A  B, determine the activation energy, Ea, of the reaction. k (M/s) T (K) 2.04  104 250 6.78  103 400

A scientist conducts an experiment to determine the rate of NO formation in the reaction: If the initial concentration of N2 was 0.500 M and the concentration of N2 was 0.450 M after 0.100 s, what is the average rate of NO formation?

Given the following data for the reaction A B, determine the activation energy, Ea, of the reaction. k (M/s) T (K) 0)730 250 0)739 450

A scientist conducts an experiment to determine the rate of the following reaction: If the initial concentration of NO2 was 0.250 M and the concentration of NO2 was 0.200 M after 0.200 s, what is the average rate of the reaction?

If the rate of the reaction: is 0.870 M/s over the first 12.25 s, how much hydrogen sulfide will be consumed during this time?

The linear form of the Arrhenius equation is very useful, as a plot of ________ versus ________ allows us to calculate the activation energy from the slope and the frequency factor from the intercept.

HI dissociates to form I2 and H2: If the concentration of HI changes at a rate of 0.45 M/s, what is the rate of appearance of I2(g)?

Which plot would provide the activation energy for a reaction?

In an elementary step of a reaction mechanism, the molecularities are determined by ________

The rate at which popcorn pops was measured at two different temperatures. How many times faster does the popcorn pop at 250°C compared with that at 210°C when the activation energy is 53.8 kJ/mol?

For the following energy profile: a) identify any reaction intermediates, b) identify any transition states, c) state the number of steps, d) state whether the reaction is endo- or exothermic, e) indicate which step is rate determining.

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?

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

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

The following figure shows Arrhenius plots for four different reactions. Which reaction has the largest frequency factor?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

If the rate of formation of nitrogen monoxide is 0.413 M/s, what is the rate of disappearance of SO₂?

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

Given the following data for the reaction A  B, determine the activation energy, E_a, of the reaction. k (M/s) T (K) 2.04  10^⁴ 250 6.78  10^³ 400

A scientist conducts an experiment to determine the rate of NO formation in the reaction: If the initial concentration of N₂ was 0.500 M and the concentration of N₂ was 0.450 M after 0.100 s, what is the average rate of NO formation?

Given the following data for the reaction A B, determine the activation energy, E_a, of the reaction. k (M/s) T (K) 0)730 250 0)739 450

A scientist conducts an experiment to determine the rate of the following reaction: If the initial concentration of NO₂ was 0.250 M and the concentration of NO₂ was 0.200 M after 0.200 s, what is the average rate of the reaction?

The linear form of the Arrhenius equation is very useful, as a plot of versus allows us to calculate the activation energy from the slope and the frequency factor from the intercept.

HI dissociates to form I₂ and H₂: If the concentration of HI changes at a rate of 0.45 M/s, what is the rate of appearance of I₂(g)?

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