Question 1

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

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 increase by a factor of 5. 
D) The rate of reaction will decrease by a factor of 2. 
E) The rate of reaction will remain unchanged.

Question 2

Which of the following represents the equation for a zero-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 =

Question 3

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

Question 4

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

Question 5

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

Question 6

The first-order reaction, 2N2O(g)→ 2N2(g)+ O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Accepted Answer

A) 0.62 s 
B) 2.8 s 
C) 6.3 s 
D) 8.4 s

Question 7

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 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 8

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of SO2 loss is 1.19 × 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

Question 9

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K. What is the rate constant at 401 K?

Accepted Answer

A) 1.92 L mol-1 s-1 
B) 7.90 × 10-5 L mol-1 s-1 
C) 0.0445 L mol-1 s-1 
D) 0.345 L mol-1 s-1 
E) 15.1 L mol-1 s-1

Question 10

Determine the rate law and the value of k for the following reaction using the data provided: CO(g)+ Cl2(g)→ COCl2(g)[CO]i (M)[Cl2]i (M)Initial Rate (M1 s-1)
0.25 0.40 0.696
0.25 0.80 1.97
0.50 0.80 3.94

Accepted Answer

A) Rate = 11 M-3/2 s-1 [CO][Cl2]3/2 
B) Rate = 36 M-1.8 s-1 [CO][Cl2]2.8 
C) Rate = 17 M-2 s-1 [CO][Cl2]2 
D) Rate = 4.4 M-1/2 s-1 [CO][Cl2]1/2 
E) Rate = 18 M-3/2 s-1 [CO]2[Cl2]1/2

Question 11

Match the following.

-n, in Rate = k[A]n

Accepted Answer

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

Question 12

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

Accepted Answer

A)   
B)   
C)   
D)   
E)

Question 13

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

Question 14

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

Question 15

The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction 2N2O5(soln)→ 4NO2(soln)+ O2(soln)
The reaction is first order and has a rate constant of 4.82 × 10-3 s-1 at 64 °C. If the reaction is initiated with 0.058 mol in a 1.00 L vessel, how many moles remain after 151 s?

Accepted Answer

A) 0.055 mol L-1 
B) 0.060 mol L-1 
C) 0.028 mol L-1 
D) 12 mol L-1 
E) 2.0 × 103 mol L-1

Question 16

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

Question 17

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.

Question 18

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 =

Question 19

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

Question 20

What are the units 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

Exam 13: Chemical Kinetics

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

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

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

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 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 first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , has a rate constant equal to 0.76 s^-1 at 1000 K. How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

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

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of SO₂ loss is 1.19 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

A reaction with an activation energy of 61.0 kJ mol^-1 has a rate constant of 0.0345 L mol^-1 s^-1 at 301 K. What is the rate constant at 401 K?

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl₂(g) → COCl₂(g) [CO]_i(M) [Cl₂]_i (M) Initial Rate (M¹s^-1) 0.25 0.40 0.696 0.25 0.80 1.97 0.50 0.80 3.94

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

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

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.

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

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

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

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

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

What are the units of k in a second-order reaction?

Exam 13: Chemical Kinetics

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

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

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

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 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 first-order reaction, 2N2O(g) → 2N2(g) + O2(g) , has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

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

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of SO2 loss is 1.19 × 10-3 mol L-1 s-1, what is the rate of formation of SO3? 2SO2(g) + O2(g) → 2SO3(g)

A reaction with an activation energy of 61.0 kJ mol-1 has a rate constant of 0.0345 L mol-1 s-1 at 301 K. What is the rate constant at 401 K?

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl2(g) → COCl2(g) [CO]i (M) [Cl2]i (M) Initial Rate (M1 s-1) 0.25 0.40 0.696 0.25 0.80 1.97 0.50 0.80 3.94

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

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

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.

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

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

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

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

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 are the units of k in a second-order reaction?

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

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 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 first-order reaction, 2N₂O(g) → 2N₂(g) + O₂(g) , has a rate constant equal to 0.76 s^-1 at 1000 K. How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

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

Given the following balanced equation, determine the rate of reaction with respect to [SO₃]. If the rate of SO₂ loss is 1.19 × 10^-3 mol L^-1 s^-1, what is the rate of formation of SO₃? 2SO₂(g) + O₂(g) → 2SO₃(g)

A reaction with an activation energy of 61.0 kJ mol^-1 has a rate constant of 0.0345 L mol^-1 s^-1 at 301 K. What is the rate constant at 401 K?

Determine the rate law and the value of k for the following reaction using the data provided: CO(g) + Cl₂(g) → COCl₂(g) [CO]_i(M) [Cl₂]_i (M) Initial Rate (M¹s^-1) 0.25 0.40 0.696 0.25 0.80 1.97 0.50 0.80 3.94

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

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.

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 [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