Question 1

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. 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. B

Question 2

What are the two key components of the frequency factor?

Accepted Answer

A)  Orientation factor and collision frequency 
B)  Activation energy and collision frequency 
C)  Orientation factor and ideal gas constant 
D)  Activation energy and temperature 
A)  Orientation factor and collision frequency 
B)  Activation energy and collision frequency 
C)  Orientation factor and ideal gas constant 
D)  Activation energy and temperature A

Question 3

Derive an expression for a "1/4-life" for a first-order reaction.

Accepted Answer

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

Question 4

Derive an expression for a "1/3-life" for a first-order reaction.

Accepted Answer

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

Question 5

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

Accepted Answer

A)  6 
B)  5 
C)  7 
D)  6.5 
E)  7.5 
A)  6 
B)  5 
C)  7 
D)  6.5 
E)  7.5

Question 6

Determine the rate law and the value of k for the following reaction using the data provided: NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate (M-1 s-1)
0)10 0.33 1.42
0)10 0.66 2.84
0)25 0.66 7.10

Accepted Answer

A)  Rate = 1360 M-2.5 s-1[NO2]2.5[O3] 
B)  Rate = 227 M-2.5 s-1[NO2][O3]2.5 
C)  Rate = 43 M-1 s-1[NO2][O3] 
D)  Rate = 430 M-2 s-1[NO2]2[O3] 
E)  Rate = 130 M-2 s-1[NO2][O3]2 
A)  Rate = 1360 M-2.5 s-1[NO2]2.5[O3] 
B)  Rate = 227 M-2.5 s-1[NO2][O3]2.5 
C)  Rate = 43 M-1 s-1[NO2][O3] 
D)  Rate = 430 M-2 s-1[NO2]2[O3] 
E)  Rate = 130 M-2 s-1[NO2][O3]2

Question 7

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

Accepted Answer

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

Question 8

Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction)
Mechanism
A2 ⇌ 2A fast
A + B → AB slow

Accepted Answer

A)  Rate = k[A][B] 
B)  Rate = k[A2][B] 
C)  Rate = k[A2][B]1/2 
D)  Rate = k[A2] 
E)  Rate = k[A2]1/2[B] 
A)  Rate = k[A][B] 
B)  Rate = k[A2][B] 
C)  Rate = k[A2][B]1/2 
D)  Rate = k[A2] 
E)  Rate = k[A2]1/2[B]

Question 9

The combustion of ethylene proceeds by the reaction     (g) + 3   (g) → 2C   (g) +   O(g) When the rate of disappearance of   is 0.74 mol L-1   , the rate of disappearance of     is ________

Accepted Answer

A)  1.5 
B)  0.49 
C)  1.1 
D)  2.2 
E)  0.25 
A)  1.5 
B)  0.49 
C)  1.1 
D)  2.2 
E)  0.25

Question 10

Match the following.
-Ea

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 11

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1)
0)093 4.84 × 10-4
0)186 9.67 × 10-4
0)279 1.45 × 10-3

Accepted Answer

A)  Rate = 5.6 × 10-2 M-1 s-1[N2O5]2 
B)  Rate = 6.0 × 10-1 M-2 s-1[N2O5]3 
C)  Rate = 1.6 × 10-3 M1/2 s-1[N2O5]1/2 
D)  Rate = 1.7 × 10-2 M-1/2 s-1[N2O5]3/2 
E)  Rate = 5.2 × 10⁻3 s-1[N2O5] 
A)  Rate = 5.6 × 10-2 M-1 s-1[N2O5]2 
B)  Rate = 6.0 × 10-1 M-2 s-1[N2O5]3 
C)  Rate = 1.6 × 10-3 M1/2 s-1[N2O5]1/2 
D)  Rate = 1.7 × 10-2 M-1/2 s-1[N2O5]3/2 
E)  Rate = 5.2 × 10⁻3 s-1[N2O5]

Question 12

Which of the following represents the integrated rate law for a first-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 13

Define half-life.

Accepted Answer

A half-life of a reaction is t

Question 14

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

Accepted Answer

A)  1.00% 
B)  37.8% 
C)  40.2% 
D)  62.2% 
A)  1.00% 
B)  37.8% 
C)  40.2% 
D)  62.2%

Question 15

The aquation of tris (1,10-phenanthroline)iron(II) in acid solution takes place according to the equation: Fe(phen)32+ + 3H3O+ + 3H2O → Fe(H2O)62+ + 3phenH+.
If the activation energy, Ea, is 126 kJ mol-1 and the rate constant at 30 °C is 9.8 × 10-3 min-1, what is the rate constant at 35°C?

Accepted Answer

A)  4.4 × 10-3 min-1 
B)  2.2 × 10-2 min-1 
C)  4.5 × 101 min-1 
D)  2.3 × 102 min-1 
A)  4.4 × 10-3 min-1 
B)  2.2 × 10-2 min-1 
C)  4.5 × 101 min-1 
D)  2.3 × 102 min-1

Question 16

Explain what the exponential factor in the Arrhenius equation represents.

Accepted Answer

The exponential factor depends on both t

Question 17

Which of the following statements is FALSE?

Accepted Answer

A)  The rate of a chemical reaction is a measure of how fast a reaction occurs. 
B)  The half-life of a first-order reaction is independent of the initial concentration of reactant. 
C)  The rate of a zero-order reaction is dependent on the concentration of the reactant. 
D)  The rate law shows the relationship between the rate and the concentrations of each reactant. 
E)  The rate order with respect to each reactant must be determined experimentally. 
A)  The rate of a chemical reaction is a measure of how fast a reaction occurs. 
B)  The half-life of a first-order reaction is independent of the initial concentration of reactant. 
C)  The rate of a zero-order reaction is dependent on the concentration of the reactant. 
D)  The rate law shows the relationship between the rate and the concentrations of each reactant. 
E)  The rate order with respect to each reactant must be determined experimentally.

Question 18

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

Accepted Answer

A)  The rate of reaction will increase by a factor of 9. 
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 4. 
E)  The rate of reaction will remain unchanged. 
A)  The rate of reaction will increase by a factor of 9. 
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 4. 
E)  The rate of reaction will remain unchanged.

Question 19

For a reaction that follows the general rate law Rate = k[A]1/2[B]2, what will happen to the rate of reaction if the concentration of A and B are is increased by a factor of 4?

Accepted Answer

A)  The rate will decrease by a factor of 1/32.0. 
B)  The rate will decrease by a factor of 1/32.00. 
C)  The rate will increase by a factor of 32. 
D)  The rate will increase by a factor of 16.0. 
A)  The rate will decrease by a factor of 1/32.0. 
B)  The rate will decrease by a factor of 1/32.00. 
C)  The rate will increase by a factor of 32. 
D)  The rate will increase by a factor of 16.0.

Question 20

Nitrogen dioxide decomposes at 300 °C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation: 2NO2(g) → 2NO(g) + O2(g).
A sample of NO2(g) is initially placed in a 2.50 L reaction vessel at 300 °C. If the half-life and the rate constant at 300 °C are 11 seconds and 0.54 L mol-1 s-1, respectively, how many moles of NO2 were in the original sample?

Accepted Answer

A)  0. 17 mol 
B)  0. 42 mol 
C)  5.9 mol 
D)  15 mol 
A)  0. 17 mol 
B)  0. 42 mol 
C)  5.9 mol 
D)  15 mol

Exam 13: Chemical Kinetics

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

What are the two key components of the frequency factor?

Derive an expression for a "1/4-life" for a first-order reaction.

Derive an expression for a "1/3-life" for a first-order reaction.

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value?

Determine the rate law and the value of k for the following reaction using the data provided: NO2(g) + O3(g) → NO3(g) + O2(g) [NO2]i (M) [O3]i (M) Initial Rate (M-1 s-1) 0)10 0.33 1.42 0)10 0.66 2.84 0)25 0.66 7.10

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

Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism A2 ⇌ 2A fast A + B → AB slow

The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L-1 , the rate of disappearance of is ________

Match the following. -Ea

Determine the rate law and the value of k for the following reaction using the data provided: 2N2O5(g) → 4NO2(g) + O2(g) [N2O5]i (M) Initial Rate (M-1 s-1) 0)093 4.84 × 10-4 0)186 9.67 × 10-4 0)279 1.45 × 10-3

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

Define half-life.

The first-order reaction, SO2Cl2 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2Cl2 will remain after 6.00 hours?

The aquation of tris (1,10-phenanthroline)iron(II) in acid solution takes place according to the equation: Fe(phen)32+ + 3H3O+ + 3H2O → Fe(H2O)62+ + 3phenH+. If the activation energy, Ea, is 126 kJ mol-1 and the rate constant at 30 °C is 9.8 × 10-3 min-1, what is the rate constant at 35°C?

Explain what the exponential factor in the Arrhenius equation represents.

Which of the following statements is FALSE?

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

For a reaction that follows the general rate law Rate = k[A]1/2[B]2, what will happen to the rate of reaction if the concentration of A and B are is increased by a factor of 4?

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

Determine the rate law and the value of k for the following reaction using the data provided: NO₂(g) + O₃(g) → NO₃(g) + O₂(g) [NO₂]_i(M) [O₃]_i (M) Initial Rate (M^-1s^-1) 0)10 0.33 1.42 0)10 0.66 2.84 0)25 0.66 7.10

Given the following proposed mechanism, predict the rate law for the overall reaction. A₂ + 2B → 2AB (overall reaction) Mechanism A₂ ⇌ 2A fast A + B → AB slow

The combustion of ethylene proceeds by the reaction (g) + 3 (g) → 2C (g) + O(g) When the rate of disappearance of is 0.74 mol L^-1 , the rate of disappearance of is ________

Match the following. -E_a

Determine the rate law and the value of k for the following reaction using the data provided: 2N₂O₅(g) → 4NO₂(g) + O₂(g) [N₂O₅]_i (M) Initial Rate (M^-1s^-1) 0)093 4.84 × 10^-4 0)186 9.67 × 10^-4 0)279 1.45 × 10^-3

The first-order reaction, SO₂Cl₂ → SO₂ + Cl₂, has a rate constant equal to 2.20 × 10^-5 s^-1 at 593 K. What percentage of the initial amount of SO₂Cl₂ will remain after 6.00 hours?

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

For a reaction that follows the general rate law Rate = k[A]^1/2[B]², what will happen to the rate of reaction if the concentration of A and B are is increased by a factor of 4?