Question 1

Identify an heterogeneous catalyst.

Accepted Answer

A) CFCs with ozone 
B) Pd in H2 gas 
C) KI dissolved in H2O2 
D) H2SO4 with concentrated HCl 
E) H3PO4 with an alcohol 
A) CFCs with ozone 
B) Pd in H2 gas 
C) KI dissolved in H2O2 
D) H2SO4 with concentrated HCl 
E) H3PO4 with an alcohol

Question 2

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

Accepted Answer

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

Question 3

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 4

What data should be plotted to show that experimental concentration data fits a second-order reaction?

Accepted Answer

A) ln[reactant] vs.time 
B) [reactant] vs.time 
C) ln(k)vs.1/T 
D) 1/[reactant] vs.time 
E) ln(k)vs.Ea 
A) ln[reactant] vs.time 
B) [reactant] vs.time 
C) ln(k)vs.1/T 
D) 1/[reactant] vs.time 
E) ln(k)vs.Ea

Question 5

Match the following.
-t1/2

Accepted Answer

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

Question 6

Match the following.
-k

Accepted Answer

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

Question 7

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

Accepted Answer

A)    
B)    
C) [A]t - [A]o = - kt 
D) k = Ae(-Ea/RT) 
E)    
A)    
B)    
C) [A]t - [A]o = - kt 
D) k = Ae(-Ea/RT) 
E)

Question 8

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

Accepted Answer

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

Question 9

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 × 102 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 × 102 s-1

Question 10

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

Accepted Answer

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

Question 11

Given the following balanced equation,determine the rate of reaction with respect to [Cl2].If the rate of Cl2 loss is 4.24 × 10-2 M/s,what is the rate of formation of NOCl?
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 12

Which of the following statements is true?

Accepted Answer

A) The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. 
B) A catalyst raises the activation energy of a reaction. 
C) Rate constants are temperature dependent. 
D) The addition of a homogeneous catalyst does not change the activation energy of a given reaction. 
E) None of the above are true. 
A) The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. 
B) A catalyst raises the activation energy of a reaction. 
C) Rate constants are temperature dependent. 
D) The addition of a homogeneous catalyst does not change the activation energy of a given reaction. 
E) None of the above are true.

Question 13

The graph represents the first-order decomposition of N2O5(g)to form NO2(g)and O2(g).
N2O5(g)→ 2NO2(g)+1/2O2(g)
What is the estimated rate constant?

Accepted Answer

A) 0.28 hr-1 
B) 0.70 hr-1 
C) 0.58 hr-1 
D) The data is insufficient to calculate rate constant. 
A) 0.28 hr-1 
B) 0.70 hr-1 
C) 0.58 hr-1 
D) The data is insufficient to calculate rate constant.

Question 14

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Accepted Answer

A) 3 
B) 1 
C) 1.75 
D) 2.75 
E) 2 
A) 3 
B) 1 
C) 1.75 
D) 2.75 
E) 2

Question 15

Given the following rate law,how does the rate of reaction change if the concentration of Y 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. 
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 16

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 17

What is the overall reaction order for the reaction that has the rate law: Rate = k[O2] [NO ]2?

Accepted Answer

A) zero order 
B) first order 
C) second order 
D) third order 
A) zero order 
B) first order 
C) second order 
D) third order

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

A first order reaction has a half-life of 30 min.If the initial concentration of the reactant is 0.50 M,what will the concentration of the reactant be after 2.00 hr?

Accepted Answer

A) 0.50 M 
B) 0.031 M 
C) 0.25 M 
D) The concentration cannot be determined without the rate constant. 
A) 0.50 M 
B) 0.031 M 
C) 0.25 M 
D) The concentration cannot be determined without the rate constant.

Question 20

Determine the rate law and the value of k for the following reaction using the data provided.
CO(g)+ Cl2(g)→ COCl2(g)

Accepted Answer

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

Identify an heterogeneous catalyst.

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

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

What data should be plotted to show that experimental concentration data fits a second-order reaction?

Match the following. -t_1/2

Match the following. -k

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

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

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?

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

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

Which of the following statements is true?

The graph represents the first-order decomposition of N₂O₅(g)to form NO₂(g)and O₂(g). N₂O₅(g)→ 2NO₂(g)+1/2O₂(g) What is the estimated rate constant?

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

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

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?

What is the overall reaction order for the reaction that has the rate law: Rate = k[O₂][NO]²?

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?

A first order reaction has a half-life of 30 min.If the initial concentration of the reactant is 0.50 M,what will the concentration of the reactant be after 2.00 hr?

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl₂(g)→ COCl₂(g)

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

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Chemical Equilibrium

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Exam 13: Chemical Kinetics

Identify an heterogeneous catalyst.

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

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

What data should be plotted to show that experimental concentration data fits a second-order reaction?

Match the following. -t1/2

Match the following. -k

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

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

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?

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

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

Which of the following statements is true?

The graph represents the first-order decomposition of N2O5(g)to form NO2(g)and O2(g). N2O5(g)→ 2NO2(g)+1/2O2(g) What is the estimated rate constant?

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

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

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?

What is the overall reaction order for the reaction that has the rate law: Rate = k[O2] [NO ]2?

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?

A first order reaction has a half-life of 30 min.If the initial concentration of the reactant is 0.50 M,what will the concentration of the reactant be after 2.00 hr?

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl2(g)→ COCl2(g)

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

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

Match the following. -t_1/2

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?

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

The graph represents the first-order decomposition of N₂O₅(g)to form NO₂(g)and O₂(g). N₂O₅(g)→ 2NO₂(g)+1/2O₂(g) What is the estimated rate constant?

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

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?

What is the overall reaction order for the reaction that has the rate law: Rate = k[O₂][NO]²?

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?

Determine the rate law and the value of k for the following reaction using the data provided. CO(g)+ Cl₂(g)→ COCl₂(g)