Question 1

Which of the following represents the equation for a second-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 2

What is the unit of k in a first-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 3

The rate constant for a first-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

Accepted Answer

A)  2.0 s 
B)  5.0 s 
C)  0.25 s 
D)  6.9 s 
E)  1.3 s 
A)  2.0 s 
B)  5.0 s 
C)  0.25 s 
D)  6.9 s 
E)  1.3 s

Question 4

Write a balanced reaction for which the following rate relationships are true. Rate = -     =     =

Accepted Answer

A)  2N2O5 → 4NO2 + O2 
B)  4NO2 + O2 → 2N2O5 
C)  2N2O5 → NO2 + 4O2 
D)    NO2 + O2 →      N2O5 
E)    N2O5 →      NO2 + O2 
A)  2N2O5 → 4NO2 + O2 
B)  4NO2 + O2 → 2N2O5 
C)  2N2O5 → NO2 + 4O2 
D)    NO2 + O2 →      N2O5 
E)    N2O5 →      NO2 + O2

Question 5

Which of the following represents the integrated rate law for a zeroth-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 6

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

Accepted Answer

A)  3.56 × 10-3 mol L-1 s-1 
B)  1.19 × 10-3 mol L-1 s-1 
C)  1.78 × 10-3 mol L-1 s-1 
D)  1.42 × 10-2 mol L-1 s-1 
E)  7.12 × 10-3 mol L-1 s-1 
A)  3.56 × 10-3 mol L-1 s-1 
B)  1.19 × 10-3 mol L-1 s-1 
C)  1.78 × 10-3 mol L-1 s-1 
D)  1.42 × 10-2 mol L-1 s-1 
E)  7.12 × 10-3 mol L-1 s-1

Question 7

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2NO(g) + Cl2(g) → 2NOCl(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 8

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

Accepted Answer

A)  4.21 g 
B)  183 g 
C)  54.8 g 
D)  76.3 g 
E)  67.5 g 
A)  4.21 g 
B)  183 g 
C)  54.8 g 
D)  76.3 g 
E)  67.5 g

Question 9

Given the following balanced equation, determine the rate of reaction with respect to [O3]. If the rate of loss of O3 is 3.91 × 10-1 mol L-1 s-1, what is the rate of the formation of O2? 2O3(g) → 3O2(g)

Accepted Answer

A)  2.61 mol L-1 s-1 
B)  0.937 mol L-1 s-1 
C)  0.261 mol L-1 s-1 
D)  0.587 mol L-1 s-1 
E)  0.817 mol L-1 s-1 
A)  2.61 mol L-1 s-1 
B)  0.937 mol L-1 s-1 
C)  0.261 mol L-1 s-1 
D)  0.587 mol L-1 s-1 
E)  0.817 mol L-1 s-1

Question 10

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Accepted Answer

A)  83.4 g 
B)  16.6 g 
C)  50.0 g 
D)  36.6 g 
E)  63.4 g 
A)  83.4 g 
B)  16.6 g 
C)  50.0 g 
D)  36.6 g 
E)  63.4 g

Question 11

Which rate law is bimolecular?

Accepted Answer

A)  rate = k[A][B]2 
B)  rate = k[A][B] 
C)  rate = k[A] 
D)  rate = k[A][B][C][D] 
E)  rate = k[A][A][B] 
A)  rate = k[A][B]2 
B)  rate = k[A][B] 
C)  rate = k[A] 
D)  rate = k[A][B][C][D] 
E)  rate = k[A][A][B]

Question 12

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Accepted Answer

A)  1 
B)  3 
C)  1.5 
D)  2.5 
E)  2 
A)  1 
B)  3 
C)  1.5 
D)  2.5 
E)  2

Question 13

Determine the missing initial rate for the following   order reaction given the following information:

Accepted Answer

A)  0.0352 mol L-1 s-1 
B)  0.0301 mol L-1 s-1 
C)  0.0215 mol L-1 s-1 
D)  0.0233 mol L-1 s-1 
E)  0.0280 mol L-1 s-1 
A)  0.0352 mol L-1 s-1 
B)  0.0301 mol L-1 s-1 
C)  0.0215 mol L-1 s-1 
D)  0.0233 mol L-1 s-1 
E)  0.0280 mol L-1 s-1

Question 14

Given the following balanced equation, determine the rate of reaction with respect to [NH3]. N2(g) + 3H2(g) → 2NH3(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 15

Given the following balanced equation, determine the rate of reaction with respect to [O2]. 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.

Question 16

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?

Accepted Answer

The relationship between the activation

Question 17

Explain how the order of a reaction can be determined.

Accepted Answer

The order of a react

Question 18

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation: 2HI(g) → H2(g) + I2(g)
At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 mol L-1 to 3.50 × 10-2 mol L-1. What is the rate constant for the reaction at this temperature?

Accepted Answer

A)  5.12 × 10-4 L mol-1 s-1 
B)  9.69 × 10-2 L mol-1 s-1 
C)  10.3 L mol-1 s-1 
D)  1.95 × 103 L mol-1 s-1 
A)  5.12 × 10-4 L mol-1 s-1 
B)  9.69 × 10-2 L mol-1 s-1 
C)  10.3 L mol-1 s-1 
D)  1.95 × 103 L mol-1 s-1

Question 19

Which of the following reactions would you predict to have the smallest orientation factor?

Accepted Answer

A)  X2 + Y2 → 2XY 
B)  NOCl2 + NO → 2 NOCl 
C)  N2 + O2 → 2NO 
D)  N + O2 → NO2 
E)  All of these reactions should have nearly identical orientation factors. 
A)  X2 + Y2 → 2XY 
B)  NOCl2 + NO → 2 NOCl 
C)  N2 + O2 → 2NO 
D)  N + O2 → NO2 
E)  All of these reactions should have nearly identical orientation factors.

Question 20

A reaction is found to have a rate constant of 3.36 × 104 L mol-1 s-1 at 344 K and a rate constant of 7.69 L mol-1 s-1 at 219 K. Determine the activation energy for this reaction.

Accepted Answer

A)  23.8 kJ mol-1 
B)  42.0 kJ mol-1 
C)  11.5 kJ mol-1 
D)  12.5 kJ mol-1 
E)  58.2 kJ mol-1 
A)  23.8 kJ mol-1 
B)  42.0 kJ mol-1 
C)  11.5 kJ mol-1 
D)  12.5 kJ mol-1 
E)  58.2 kJ mol-1

Exam 13: Chemical Kinetics

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

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

The rate constant for a first-order reaction is 0.54 L mol-1 s-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L-1?

Write a balanced reaction for which the following rate relationships are true. Rate = - = =

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

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2NO(g) + Cl2(g) → 2NOCl(g)

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon remain after 7.22 days if the sample initially weighs 250.0 grams?

Given the following balanced equation, determine the rate of reaction with respect to [O3]. If the rate of loss of O3 is 3.91 × 10-1 mol L-1 s-1, what is the rate of the formation of O2? 2O3(g) → 3O2(g)

The first-order decay of radon has a half-life of 3.823 days. How many grams of radon decomposes after 5.55 days if the sample initially weighs 100.0 grams?

Which rate law is bimolecular?

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Determine the missing initial rate for the following order reaction given the following information:

Given the following balanced equation, determine the rate of reaction with respect to [NH3]. N2(g) + 3H2(g) → 2NH3(g)

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

Is the activation energy for a forward reaction the same as the activation energy for the reverse of the same reaction?

Explain how the order of a reaction can be determined.

Which of the following reactions would you predict to have the smallest orientation factor?

A reaction is found to have a rate constant of 3.36 × 104 L mol-1 s-1 at 344 K and a rate constant of 7.69 L mol-1 s-1 at 219 K. Determine the activation energy for this reaction.

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The rate constant for a first-order reaction is 0.54 L mol^-1s^-1. What is the half-life of this reaction if the initial concentration is 0.27 mol L^-1?

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of O₂ loss is 3.56 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. 2NO(g) + Cl₂(g) → 2NOCl(g)

Given the following balanced equation, determine the rate of reaction with respect to [O₃]. If the rate of loss of O₃ is 3.91 × 10^-1 mol L^-1 s^-¹, what is the rate of the formation of O₂? 2O₃(g) → 3O₂(g)

Given the following balanced equation, determine the rate of reaction with respect to [NH₃]. N₂(g) + 3H₂(g) → 2NH₃(g)

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

A reaction is found to have a rate constant of 3.36 × 10⁴ L mol^-1s^-1 at 344 K and a rate constant of 7.69 L mol^-1s^-1 at 219 K. Determine the activation energy for this reaction.