Question 1

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?
 Use a sketch of a reaction energy diagram.

Accepted Answer

The relationship between the activation

Question 2

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled?
Rate = k [X][Y]

Accepted Answer

A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 4. 
C)  The rate of reaction will decrease by a factor of 3. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged. 
A)  The rate of reaction will increase by a factor of 2. 
B)  The rate of reaction will increase by a factor of 4. 
C)  The rate of reaction will decrease by a factor of 3. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged.

Question 3

The rate constant for a reaction is 5.55 × 10-3 s-1.If after 4 minutes you have 44.1g of material left,what was the initial concentration?

Accepted Answer

A)  44.9 g 
B)  1.8 g 
C)  167 g 
D)  2.09 g 
E)  12.3 g 
A)  44.9 g 
B)  1.8 g 
C)  167 g 
D)  2.09 g 
E)  12.3 g

Question 4

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 are false. 
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 are false.

Question 5

Explain what the exponential factor in the Arrhenius equation represents.

Accepted Answer

The exponential factor depends on both t

Question 6

The rate constant,k,for a first-order reaction is equal to 4.2 × 10-4 s-1.What is the half-life for the reaction?

Accepted Answer

A)  2.9 × 10-4 s 
B)  1.2 × 103 s 
C)  1.7 × 103 s 
D)  2.4 × 103 s 
A)  2.9 × 10-4 s 
B)  1.2 × 103 s 
C)  1.7 × 103 s 
D)  2.4 × 103 s

Question 7

The rate constant for a zero-order reaction is 0.54 M s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Accepted Answer

A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s 
A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s

Question 8

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled?
Rate = k [X]2[Y]3

Accepted Answer

A)  The rate of reaction will increase by a factor of 5. 
B)  The rate of reaction will increase by a factor of 2. 
C)  the rate of reaction will increase by a factor of 8. 
D)  The rate of reaction will increase by a factor of 3. 
E)  The rate of reaction will remain unchanged. 
A)  The rate of reaction will increase by a factor of 5. 
B)  The rate of reaction will increase by a factor of 2. 
C)  the rate of reaction will increase by a factor of 8. 
D)  The rate of reaction will increase by a factor of 3. 
E)  The rate of reaction will remain unchanged.

Question 9

Which of the following is a rate law for a reaction that is first order with respect to oxygen?

Accepted Answer

A)  rate = k [NO2] 
B)  rate = k [NO2]2 [O2}1/2 
C)  rate = k [NO2] [O2}1/2 
D)  rate = k [NO2] [O2}1/2 [N2]1/2 
E)  rate = k [NO2]2 [O2} 
A)  rate = k [NO2] 
B)  rate = k [NO2]2 [O2}1/2 
C)  rate = k [NO2] [O2}1/2 
D)  rate = k [NO2] [O2}1/2 [N2]1/2 
E)  rate = k [NO2]2 [O2}

Question 10

For a reaction,what generally happens if the temperature is increased?

Accepted Answer

A)  A decrease in k occurs, which results in a faster rate. 
B)  A decrease in k occurs, which results in a slower rate. 
C)  An increase in k occurs, which results in a faster rate. 
D)  An increase in k occurs, which results in a slower rate. 
E)  There is no change with k or the rate. 
A)  A decrease in k occurs, which results in a faster rate. 
B)  A decrease in k occurs, which results in a slower rate. 
C)  An increase in k occurs, which results in a faster rate. 
D)  An increase in k occurs, which results in a slower rate. 
E)  There is no change with k or the rate.

Question 11

decomposes in the gas phase by the reaction     (g)→   (g)+   (g) The reaction is first order in     and the rate constant is 3.0 ×     at 600 K.A vessel is charged with 2.4 atm of   at 600 K.The partial pressure of     at   is ________ atm.

Accepted Answer

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

Question 12

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 × 10 5 s-1 
E)  3.5 × 103 s-1 
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 13

In aqueous solution,hypobromite ion,BrO-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation.   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 
A)  4.5 × 10-2 s 
B)  7.1 s 
C)  12 s 
D)  22 s

Question 14

A particular first-order reaction has a rate constant of 1.35 ×     at 25.0°C.What is the magnitude of k at 75.0°C if

Accepted Answer

A)  3.47 ×   s-1 
B)  1.92 × 104 s-1 
C)  670 s-1 
D)  3.85 ×   s-1 
E)  1.36 ×   s-1 
A)  3.47 ×   s-1 
B)  1.92 × 104 s-1 
C)  670 s-1 
D)  3.85 ×   s-1 
E)  1.36 ×   s-1

Question 15

The second-order decomposition of NO2 has a rate constant of 0.255 M-1s-1.How much NO2 decomposes in 4.00 s if the initial concentration of NO2 (1.00 L volume)is 1.33 M?

Accepted Answer

A)  1.8 mol 
B)  0.85 mol 
C)  0.48 mol 
D)  0.77 mol 
E)  0.56 mol 
A)  1.8 mol 
B)  0.85 mol 
C)  0.48 mol 
D)  0.77 mol 
E)  0.56 mol

Question 16

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

Accepted Answer

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

Question 17

The rate constant for the first-order decomposition of N2O is 3.40 s-1.What is the half-life of the decomposition?

Accepted Answer

A)  0.491 s 
B)  0.204 s 
C)  0.236 s 
D)  0.424 s 
E)  0.294 s 
A)  0.491 s 
B)  0.204 s 
C)  0.236 s 
D)  0.424 s 
E)  0.294 s

Question 18

Given the following balanced equation,determine the rate of reaction with respect to [O2].If the rate of formation of O2 is 7.78 × 10-1 M/s,what is the rate of the loss of O3?
2 O3(g)→ 3 O2(g)

Accepted Answer

A)  0.519 M/s 
B)  1.56 M/s 
C)  2.34 M/s 
D)  1.17 M/s 
E)  7.78 M/s 
A)  0.519 M/s 
B)  1.56 M/s 
C)  2.34 M/s 
D)  1.17 M/s 
E)  7.78 M/s

Question 19

What are the units of k in the following rate law?
Rate = k[X][Y]2

Accepted Answer

A)    
B)    
C)  M2 s 
D)    
E)    
A)    
B)    
C)  M2 s 
D)    
E)

Question 20

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

Exam 15: Chemical Kinetics

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction? Use a sketch of a reaction energy diagram.

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]

The rate constant for a reaction is 5.55 × 10-3 s-1.If after 4 minutes you have 44.1g of material left,what was the initial concentration?

Which of the following statements is FALSE?

Explain what the exponential factor in the Arrhenius equation represents.

The rate constant,k,for a first-order reaction is equal to 4.2 × 10-4 s-1.What is the half-life for the reaction?

The rate constant for a zero-order reaction is 0.54 M s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]2[Y]3

Which of the following is a rate law for a reaction that is first order with respect to oxygen?

For a reaction,what generally happens if the temperature is increased?

decomposes in the gas phase by the reaction (g)→ (g)+ (g) The reaction is first order in and the rate constant is 3.0 × at 600 K.A vessel is charged with 2.4 atm of at 600 K.The partial pressure of at is ________ atm.

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?

A particular first-order reaction has a rate constant of 1.35 × at 25.0°C.What is the magnitude of k at 75.0°C if

The second-order decomposition of NO2 has a rate constant of 0.255 M-1s-1.How much NO2 decomposes in 4.00 s if the initial concentration of NO2 (1.00 L volume)is 1.33 M?

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

The rate constant for the first-order decomposition of N2O is 3.40 s-1.What is the half-life of the decomposition?

Given the following balanced equation,determine the rate of reaction with respect to [O2].If the rate of formation of O2 is 7.78 × 10-1 M/s,what is the rate of the loss of O3? 2 O3(g)→ 3 O2(g)

What are the units of k in the following rate law? Rate = k[X][Y]2

Identify an heterogeneous catalyst.

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

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Chemical Equilibrium

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The rate constant for a reaction is 5.55 × 10^-3s^-1.If after 4 minutes you have 44.1g of material left,what was the initial concentration?

The rate constant,k,for a first-order reaction is equal to 4.2 × 10^-4 s^-1.What is the half-life for the reaction?

The rate constant for a zero-order reaction is 0.54 Ms^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Given the following rate law,how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X]²[Y]³

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?

The second-order decomposition of NO₂ has a rate constant of 0.255 M^-1s^-1.How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 M?

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

The rate constant for the first-order decomposition of N₂O is 3.40 s^-1.What is the half-life of the decomposition?

Given the following balanced equation,determine the rate of reaction with respect to [O₂].If the rate of formation of O₂ is 7.78 × 10^-1 M/s,what is the rate of the loss of O₃? 2 O₃(g)→ 3 O₂(g)

What are the units of k in the following rate law? Rate = k[X][Y]²