Question 1

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 is 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 is FALSE.

Question 2

Give the characteristic of a first-order reaction having only one reactant.

Accepted Answer

A)  The rate of the reaction is not proportional to the concentration of the reactant. 
B)  The rate of the reaction is proportional to the square of the concentration of the reactant. 
C)  The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D)  The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E)  The rate of the reaction is directly proportional to the concentration of the reactant. 
A)  The rate of the reaction is not proportional to the concentration of the reactant. 
B)  The rate of the reaction is proportional to the square of the concentration of the reactant. 
C)  The rate of the reaction is proportional to the square root of the concentration of the reactant. 
D)  The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. 
E)  The rate of the reaction is directly proportional to the concentration of the reactant.

Question 3

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0,what is the new rate if the concentration of [A] is increased to 0.200 M?

Accepted Answer

A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s 
A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s

Question 4

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

Accepted Answer

A)  4.55 M 
B)  0.258 M 
C)  3.87 M 
D)  2.20 M 
E)  2.39 M 
A)  4.55 M 
B)  0.258 M 
C)  3.87 M 
D)  2.20 M 
E)  2.39 M

Question 5

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0[B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

Accepted Answer

A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s 
A)  0.0200 M/s 
B)  0.0400 M/s 
C)  0.0600 M/s 
D)  0.0800 M/s 
E)  0.100 M/s

Question 6

Define activation energy.

Accepted Answer

Activation energy is the energ

Question 7

Define the frequency factor.

Accepted Answer

The frequency factor

Question 8

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 × 105 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 × 105 s-1 
E)  3.5 × 103 s-1

Question 9

In aqueous solution,hypobromite ion,BrO-,reacts to produce bromate ion,BrO3-,and bromide ion,Br-,according to the following chemical equation. 3 BrO-(aq)→ BrO3-(aq)+ 2 Br-(aq)
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 10

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of disappearance of Cl2 is 4.24 × 10-2 M/s,what is the rate of formation of NO? 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

Accepted Answer

A)  4.24 × 10-2 M/s 
B)  2.12 × 10-2 M/s 
C)  1.06 × 10-1 M/s 
D)  8.48 × 10-2 M/s 
E)  1.61 × 10-2 M/s 
A)  4.24 × 10-2 M/s 
B)  2.12 × 10-2 M/s 
C)  1.06 × 10-1 M/s 
D)  8.48 × 10-2 M/s 
E)  1.61 × 10-2 M/s

Question 11

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

Accepted Answer

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

Question 12

What is the difference between average reaction rate and instantaneous reaction rate?

Accepted Answer

An average reaction rate is determined u

Question 13

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

Accepted Answer

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

Question 14

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0°C.What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?

Accepted Answer

A)  9.56 × 103 s-1 
B)  2.85 × 104 s-1 
C)  576 s-1 
D)  4.33 × 1087 s-1 
E)  1.36 ×   s-1 
A)  9.56 × 103 s-1 
B)  2.85 × 104 s-1 
C)  576 s-1 
D)  4.33 × 1087 s-1 
E)  1.36 ×   s-1

Question 15

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 5.00? The rate will

Accepted Answer

A)  decrease by a factor of 1/25.0. 
B)  decrease by a factor of 1/5.00. 
C)  increase by a factor of 5.00. 
D)  increase by a factor of 25.00. 
A)  decrease by a factor of 1/25.0. 
B)  decrease by a factor of 1/5.00. 
C)  increase by a factor of 5.00. 
D)  increase by a factor of 25.00.

Question 16

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)  22.7 hr 
A)  0.143 hr 
B)  2.28 hr 
C)  6.99 hr 
D)  22.7 hr

Question 17

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]o 
A)  t 1/2 =   
B)  t 1/2 =   
C)  t 1/2 =   
D)  t 1/2 =   
E)  t 1/2 = [A]o

Question 18

The following reaction is first order,C2H6 → 2 CH3.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 19

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

Accepted Answer

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

Question 20

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

Accepted Answer

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

Exam 14: Chemical Kinetics

Which of the following statements is FALSE?

Give the characteristic of a first-order reaction having only one reactant.

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0,what is the new rate if the concentration of [A] is increased to 0.200 M?

The second-order decomposition of HI has a rate constant of 1.80 × 10-3 M-1s-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]0[B]2,what is the new rate if the concentration of [A] is increased to 0.200 M?

Define activation energy.

Define the frequency factor.

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?

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of disappearance of Cl2 is 4.24 × 10-2 M/s,what is the rate of formation of NO? 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

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

What is the difference between average reaction rate and instantaneous reaction rate?

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

A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0°C.What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol?

For a reaction that follows the general rate law,Rate = k[A][B]2,what will happen to the rate of reaction if the concentration of B is increased by a factor of 5.00? The rate will

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?

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

The following reaction is first order,C2H6 → 2 CH3.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?

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

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A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰,what is the new rate if the concentration of [A] is increased to 0.200 M?

The second-order decomposition of HI has a rate constant of 1.80 × 10^-3 M^-1s^-1.How much HI remains after 27.3 s if the initial concentration of HI is 4.78 M?

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]⁰[B]²,what is the new rate if the concentration of [A] is increased to 0.200 M?

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?

Given the following balanced equation,determine the rate of reaction with respect to [Cl₂].If the rate of disappearance of Cl₂ is 4.24 × 10^-2 M/s,what is the rate of formation of NO? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

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

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

A particular first-order reaction has a rate constant of 1.35 × 10² s^-1 at 25.0°C.What is the magnitude of k at 95.0°C if E_a = 55.5 kJ/mol?

For a reaction that follows the general rate law,Rate = k[A][B]²,what will happen to the rate of reaction if the concentration of B is increased by a factor of 5.00? The rate will

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?

The following reaction is first order,C₂H₆ → 2 CH₃.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?

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