Question 1

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

Accepted Answer

A)  adsorption. 
B)  diffusion. 
C)  reaction. 
D)  desorption. 
E)  none of the above 
A)  adsorption. 
B)  diffusion. 
C)  reaction. 
D)  desorption. 
E)  none of the above

Question 2

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)

Question 3

The rate constant for a first-order reaction is 0.54 s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

Accepted Answer

A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s 
A)  0.089 s 
B)  1.8 s 
C)  0.31 s 
D)  5.6 s 
E)  1.3 s

Question 4

Match between columns
                        Premises: n,in Rate = k[A]S1U1P1nS1S1P0
k
A
ES1U1B1aS1U1B0
tS1U1B11/2S1U1B0

Accepted Answer

The Answer of frequency factor and rate constant and reaction is...

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)  4 
C)  24 
D)  6.5 
E)  7.5 
A)  6 
B)  4 
C)  24 
D)  6.5 
E)  7.5

Question 6

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]2[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 7

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]1,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 8

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

Accepted Answer

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

Question 9

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1.If the initial concentration of N2O is 10.9 M,what is the concentration of N2O after 9.6 s?

Accepted Answer

A)  7.4 × 10-3 M 
B)  1.0 × 10-3 M 
C)  1.4 × 10-3 M 
D)  3.6 × 10-3 M 
E)  8.7 × 10-3 M 
A)  7.4 × 10-3 M 
B)  1.0 × 10-3 M 
C)  1.4 × 10-3 M 
D)  3.6 × 10-3 M 
E)  8.7 × 10-3 M

Question 10

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

Accepted Answer

A)  adsorption. 
B)  diffusion. 
C)  reaction. 
D)  desorption. 
E)  none of the above 
A)  adsorption. 
B)  diffusion. 
C)  reaction. 
D)  desorption. 
E)  none of the above

Question 11

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

Accepted Answer

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

Question 12

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1.If the initial concentration of N2O5 is 2.88 M,what is the concentration of N2O5 after 12.5 minutes?

Accepted Answer

A)  0.124 M 
B)  0.805 M 
C)  2.82 M 
D)  0.355 M 
E)  0.174 M 
A)  0.124 M 
B)  0.805 M 
C)  2.82 M 
D)  0.355 M 
E)  0.174 M

Question 13

Determine the rate law and the value of k for the following reaction using the data provided. S2O82⁻(aq)+ 3 I⁻(aq)→ 2 SO42⁻(g)+ I3⁻(aq)[S2O82⁻]i (M)[I⁻]i (M)Initial Rate (M-1s-1)
0)30 0.42 4.54
0)44 0.42 6.65
0)44 0.21 3.33

Accepted Answer

A)  Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] 
B)  Rate = 36 M-1s-1 [S2O82⁻][I⁻] 
C)  Rate = 86 M-2s-1 [S2O82⁻][I⁻]2 
D)  Rate = 195 M-3s-1 [S2O82⁻]2[I⁻]2 
E)  Rate = 23 M-1/2s-1 [S2O82⁻][I⁻]1/2 
A)  Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] 
B)  Rate = 36 M-1s-1 [S2O82⁻][I⁻] 
C)  Rate = 86 M-2s-1 [S2O82⁻][I⁻]2 
D)  Rate = 195 M-3s-1 [S2O82⁻]2[I⁻]2 
E)  Rate = 23 M-1/2s-1 [S2O82⁻][I⁻]1/2

Question 14

What are the units of k in the following rate law? Rate = k[X] [Y]3

Accepted Answer

A)    
B)    
C)  M s2 
D)    
E)    
A)    
B)    
C)  M s2 
D)    
E)

Question 15

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

Accepted Answer

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

Question 16

Explain what the exponential factor in the Arrhenius equation represents.

Accepted Answer

The exponential factor depends on both t

Question 17

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s-1)for the reaction?

Accepted Answer

A)  2.0 × 10-4 s-1 
B)  9.6 × 10-4 s-1 
C)  1.2 × 10-2 s-1 
D)  5.8 × 10-2 s-1 
A)  2.0 × 10-4 s-1 
B)  9.6 × 10-4 s-1 
C)  1.2 × 10-2 s-1 
D)  5.8 × 10-2 s-1

Question 18

Given the following balanced equation,determine the rate of reaction with respect to [NOCl]. 2 NO(g)+ Cl2(g)→ 2 NOCl(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 19

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 20

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 with 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 with k or the rate.

Exam 14: Chemical Kinetics

In the hydrogenation of double bonds,a catalyst is needed.In the first step,the reactants must come into contact with a metal surface.This step is known as

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

The rate constant for a first-order reaction is 0.54 s-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

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

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

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]1,what is the new rate if the concentration of [A] is increased to 0.200 M?

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

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1.If the initial concentration of N2O is 10.9 M,what is the concentration of N2O after 9.6 s?

In the hydrogenation of double bonds,a catalyst is needed.In the second step,the reactants diffuse on the surface until they approach each other.This step is known as

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

The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1.If the initial concentration of N2O5 is 2.88 M,what is the concentration of N2O5 after 12.5 minutes?

Determine the rate law and the value of k for the following reaction using the data provided. S2O82⁻(aq)+ 3 I⁻(aq)→ 2 SO42⁻(g)+ I3⁻(aq)[S2O82⁻]i (M)[I⁻]i (M)Initial Rate (M-1s-1) 0)30 0.42 4.54 0)44 0.42 6.65 0)44 0.21 3.33

What are the units of k in the following rate law? Rate = k[X] [Y]3

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

Explain what the exponential factor in the Arrhenius equation represents.

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s-1)for the reaction?

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

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?

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

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The rate constant for a first-order reaction is 0.54 s^-1.What is the half-life of this reaction if the initial concentration is 0.33 M?

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

A rate is equal to 0.0200 M/s.If [A] = 0.100 M and rate = k[A]¹,what is the new rate if the concentration of [A] is increased to 0.200 M?

The first-order decomposition of N₂O at 1000 K has a rate constant of 0.76 s^-1.If the initial concentration of N₂O is 10.9 M,what is the concentration of N₂O after 9.6 s?

The first-order decomposition of N₂O₅ at 328 K has a rate constant of 1.70 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 2.88 M,what is the concentration of N₂O₅ after 12.5 minutes?

Determine the rate law and the value of k for the following reaction using the data provided. S₂O₈²⁻(aq)+ 3 I⁻(aq)→ 2 SO₄²⁻(g)+ I₃⁻(aq)[S₂O₈²⁻]_i(M)[I⁻]_i (M)Initial Rate (M^-1s^-1) 0)30 0.42 4.54 0)44 0.42 6.65 0)44 0.21 3.33

What are the units of k in the following rate law? Rate = k[X][Y]³

For a particular first-order reaction,it takes 24 minutes for the concentration of the reactant to decrease to 25% of its initial value.What is the value for rate constant (in s^-1)for the reaction?

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

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?