Question 1

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 to either 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 to either k or the rate

Question 2

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

Accepted Answer

A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information. 
A)  Rate = -     
B)  Rate = -     
C)  Rate = +     
D)  Rate = +     
E)  It is not possible to determine the answer without more information.

Question 3

What data should be plotted to show that experimental concentration data fit a second-order reaction?

Accepted Answer

A)  ln[reactant] vs. time 
B)  [reactant] vs. time 
C)  ln(k) vs.   
D)    vs. time 
E)  ln(k) vs. Ea 
A)  ln[reactant] vs. time 
B)  [reactant] vs. time 
C)  ln(k) vs.   
D)    vs. time 
E)  ln(k) vs. Ea

Question 4

Match the following.
-n, in Rate = k[A]n

Accepted Answer

A) reaction order 
B) frequency factor 
C) activation energy 
D) rate constant 
E) half-life 
A) reaction order 
B) frequency factor 
C) activation energy 
D) rate constant 
E) half-life

Question 5

What is the unit 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 6

The ________ is the fraction of approaches that are successful in surmounting the activation barrier and forming products.

Accepted Answer

A)  Activation factor 
B)  Frequency factor 
C)  Arrhenius factor 
D)  Exponential factor 
E)  Thermal factor 
A)  Activation factor 
B)  Frequency factor 
C)  Arrhenius factor 
D)  Exponential factor 
E)  Thermal factor

Question 7

The following reaction is first order, C2H6 → 2CH3. If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0. 20 mol in the same container?

Accepted Answer

A)  4.5 min 
B)  17 min 
C)  53 min 
D)  65 min 
A)  4.5 min 
B)  17 min 
C)  53 min 
D)  65 min

Question 8

Define the frequency factor.

Accepted Answer

The frequency factor

Question 9

For the first-order reaction, 2N2O(g) → 2N2(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 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 
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 10

Calculate the frequency factor, A, for a reaction with a rate constant of 6.3 × 103 s-1 and an activation energy, Ea, of 74 kJ mol-1 at 315 K.

Accepted Answer

A)  1.2 × 1016 s-1 
B)  3.8 × 1016 s-1 
C)  4.0 × 1016 s-1 
D)  6.1 × 1016 s-1 
E)  8.9 × 1016 s-1 
A)  1.2 × 1016 s-1 
B)  3.8 × 1016 s-1 
C)  4.0 × 1016 s-1 
D)  6.1 × 1016 s-1 
E)  8.9 × 1016 s-1

Question 11

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g) → 4NO2(g) + O2(g).
If the rate of appearance of O2 is equal to 3.00 mol min-1 at a particular moment, what is the rate of disappearance of N2O5 at that moment?

Accepted Answer

A)  0. 750 mol min-1 
B)  1. 50 mol min-1 
C)  6.00 mol min-1 
D)  12.0 mol min-1 
A)  0. 750 mol min-1 
B)  1. 50 mol min-1 
C)  6.00 mol min-1 
D)  12.0 mol min-1

Question 12

The ________ is the number of times that the reactants approach the activation barrier per unit time.

Accepted Answer

A)  Activation factor 
B)  Frequency factor 
C)  Arrhenius factor 
D)  Exponential factor 
E)  Thermal factor 
A)  Activation factor 
B)  Frequency factor 
C)  Arrhenius factor 
D)  Exponential factor 
E)  Thermal factor

Question 13

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

Accepted Answer

A)  zero order 
B)  first order 
C)  second order 
D)  third order 
E)  impossible to determine 
A)  zero order 
B)  first order 
C)  second order 
D)  third order 
E)  impossible to determine

Question 14

What is the unit of k in a second-order reaction?

Accepted Answer

A)  mol L-1 s-1 
B)  mol L-1 s 
C)  L mol-1 s-1 
D)  M2 s-1 
E)  s-1 
A)  mol L-1 s-1 
B)  mol L-1 s 
C)  L mol-1 s-1 
D)  M2 s-1 
E)  s-1

Question 15

Which of the following represents the equation for a first-order half-life?

Accepted Answer

A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 =   
A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 =

Question 16

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

Accepted Answer

A)  9.57   
B)  3.74 ×1087   
C)  1.36 ×     
D)  575   
E)  1.05 ×     
A)  9.57   
B)  3.74 ×1087   
C)  1.36 ×     
D)  575   
E)  1.05 ×

Question 17

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

Accepted Answer

A)    = -kt 
B)    -   = kt 
C)  [A]t - [A]0 = -kt 
D)  k = Ae(-Ea/RT) 
E)    =     + lnA 
A)    = -kt 
B)    -   = kt 
C)  [A]t - [A]0 = -kt 
D)  k = Ae(-Ea/RT) 
E)    =     + lnA

Question 18

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 8.12 × 109 s-1 and a rate constant of 3.05 × 104 s-1 at 375 K.

Accepted Answer

A)  72.5 kJ mol-1 
B)  38.9 kJ mol-1 
C)  104 kJ mol-1 
D)  68.0 kJ mol-1 
E)  71.6 kJ mol-1 
A)  72.5 kJ mol-1 
B)  38.9 kJ mol-1 
C)  104 kJ mol-1 
D)  68.0 kJ mol-1 
E)  71.6 kJ mol-1

Question 19

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Accepted Answer

A)  0. 143 hr 
B)  2.28 hr 
C)  6.99 hr 
D)  22.8 hr 
A)  0. 143 hr 
B)  2.28 hr 
C)  6.99 hr 
D)  22.8 hr

Question 20

Given the following balanced equation, determine the rate of reaction with respect to [SO2]. 2SO2(g) + O2(g) → 2SO3(g)

Accepted Answer

A)  Rate = -     
B)  Rate = +     
C)  Rate = -   
D)  Rate = +   
E)  It is not possible to determine the answer without more information. 
A)  Rate = -     
B)  Rate = +     
C)  Rate = -   
D)  Rate = +   
E)  It is not possible to determine the answer without more information.

Exam 13: Chemical Kinetics

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

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

What data should be plotted to show that experimental concentration data fit a second-order reaction?

Match the following. -n, in Rate = k[A]n

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

The ________ is the fraction of approaches that are successful in surmounting the activation barrier and forming products.

The following reaction is first order, C2H6 → 2CH3. If the rate constant is equal to 5.5 × 10-4 s-1 at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0. 20 mol in the same container?

Define the frequency factor.

For the first-order reaction, 2N2O(g) → 2N2(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?

Calculate the frequency factor, A, for a reaction with a rate constant of 6.3 × 103 s-1 and an activation energy, Ea, of 74 kJ mol-1 at 315 K.

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g) → 4NO2(g) + O2(g). If the rate of appearance of O2 is equal to 3.00 mol min-1 at a particular moment, what is the rate of disappearance of N2O5 at that moment?

The ________ is the number of times that the reactants approach the activation barrier per unit time.

Without performing complex calculations, determine the order of a reaction that has the following initial rates for the specified starting concentration:

What is the unit of k in a second-order reaction?

Which of the following represents the equation for a first-order half-life?

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

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

Calculate the activation energy, Ea, for a reaction with a frequency factor, A, of 8.12 × 109 s-1 and a rate constant of 3.05 × 104 s-1 at 375 K.

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 16.5% of its initial value?

Given the following balanced equation, determine the rate of reaction with respect to [SO2]. 2SO2(g) + O2(g) → 2SO3(g)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Equilibrium

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Gibbs Energy and Thermodynamics

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Organic Chemistry I: Structures

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Metals and Metallurgy

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Filters

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

Match the following. -n, in Rate = k[A]ⁿ

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

The following reaction is first order, C₂H₆ → 2CH₃. If the rate constant is equal to 5.5 × 10^-4 s^-1 at 1000 K, how long will it take for 0.35 mol of C₂H₆ in a 1.00 L container to decrease to 0. 20 mol in the same container?

For the first-order reaction, 2N₂O(g) → 2N₂(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?

Calculate the frequency factor, A, for a reaction with a rate constant of 6.3 × 10³ s^-1 and an activation energy, E_a, of 74 kJ mol^-1 at 315 K.

The decomposition of dinitrogen pentoxide is described by the chemical equation 2N₂O₅(g) → 4NO₂(g) + O₂(g). If the rate of appearance of O₂ is equal to 3.00 mol min^-1 at a particular moment, what is the rate of disappearance of N₂O₅ at that moment?

Calculate the activation energy, E_a, for a reaction with a frequency factor, A, of 8.12 × 10⁹ s^-1 and a rate constant of 3.05 × 10⁴ s^-1 at 375 K.

The first-order reaction, SO₂Cl₂ → SO₂ + Cl₂, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO₂Cl₂ to fall to 16.5% of its initial value?

Given the following balanced equation, determine the rate of reaction with respect to [SO₂]. 2SO₂(g) + O₂(g) → 2SO₃(g)