Question 1

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 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?

Accepted Answer

A) 2.9 × 10-4 s 
B) 1.2 × 103 s 
C) 1.7 × 103 s 
D) 2.4 × 103 s 
A) 2.9 × 10-4 s 
B) 1.2 × 103 s 
C) 1.7 × 103 s 
D) 2.4 × 103 s

Question 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 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 4

The second-order reaction 2 Mn(CO)5 → Mn2(CO)10,has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C.If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

Accepted Answer

A) 6.7 × 10-16 s 
B) 7.4 × 10-15 s 
C) 1.5 × 10-4 s 
D) 6.0 × 103 s 
A) 6.7 × 10-16 s 
B) 7.4 × 10-15 s 
C) 1.5 × 10-4 s 
D) 6.0 × 103 s

Question 5

The reaction that occurs in a Breathalyzer,a device used to determine the alcohol level in a person's bloodstream,is given below.If the rate of appearance of Cr2(SO4)3 is 1.64 mol/min at a particular moment,what is the rate of disappearance of C2H6O at that moment?
2 K2Cr2O7 + 8 H2SO4 + 3 C2H6O → 2 Cr2(SO4)3 + 2 K2SO4 + 11 H2O

Accepted Answer

A) 0.547 mol/min 
B) 1.09 mol/min 
C) 2.46 mol/min 
D) 4.92 mol/min 
A) 0.547 mol/min 
B) 1.09 mol/min 
C) 2.46 mol/min 
D) 4.92 mol/min

Question 6

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl2 loss is 4.84 × 10-2 M/s,what is the rate of formation of NOCl?
2 NO(g)+ Cl2(g)→ 2 NOCl(g)

Accepted Answer

A) 4.84 × 10-2 M/s 
B) 2.42 × 10-2 M/s 
C) 1.45 × 10-1 M/s 
D) 9.68 × 10-2 M/s 
E) 1.61 × 10-2 M/s 
A) 4.84 × 10-2 M/s 
B) 2.42 × 10-2 M/s 
C) 1.45 × 10-1 M/s 
D) 9.68 × 10-2 M/s 
E) 1.61 × 10-2 M/s

Question 7

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 8

Given the following proposed mechanism,predict the rate law for the overall reaction.
2NO2 + Cl2 → 2NO2Cl (overall reaction)
Mechanism
NO2 + Cl2 → NO2Cl + Cl slow
NO2 + Cl → NO2Cl fast

Accepted Answer

A) Rate = k[NO2][Cl2] 
B) Rate = k[NO2]2[Cl2] 
C) Rate = k[NO2][Cl] 
D) Rate = k[NO2Cl][Cl] 
E) Rate = k[NO2Cl]2 
A) Rate = k[NO2][Cl2] 
B) Rate = k[NO2]2[Cl2] 
C) Rate = k[NO2][Cl] 
D) Rate = k[NO2Cl][Cl] 
E) Rate = k[NO2Cl]2

Question 9

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M.What is the rate constant for this reaction?

Accepted Answer

A) 1.0 × 10-2 M-1s-1 
B) 4.5 × 10-2 M-1s-1 
C) 9.7 × 10-2 M-1s-1 
D) 2.2 × 10-2 M-1s-1 
E) 3.8 × 10-2 M-1s-1 
A) 1.0 × 10-2 M-1s-1 
B) 4.5 × 10-2 M-1s-1 
C) 9.7 × 10-2 M-1s-1 
D) 2.2 × 10-2 M-1s-1 
E) 3.8 × 10-2 M-1s-1

Question 10

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)

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

Question 11

Determine the rate law and the value of k for the following reaction using the data provided.
2 NO(g)+ O2(g)→ 2 NO2(g)

Accepted Answer

A) Rate = 57 M-1s-1[NO][O2] 
B) Rate = 3.8 M-1/2s-1[NO][O2]1/2 
C) Rate = 3.1 × 105 M-3s-1[NO]2[O2]2 
D) Rate = 1.7 × 103 M-2s-1[NO]2[O2] 
E) Rate = 9.4 × 103 M-2s-1[NO][O2]2 
A) Rate = 57 M-1s-1[NO][O2] 
B) Rate = 3.8 M-1/2s-1[NO][O2]1/2 
C) Rate = 3.1 × 105 M-3s-1[NO]2[O2]2 
D) Rate = 1.7 × 103 M-2s-1[NO]2[O2] 
E) Rate = 9.4 × 103 M-2s-1[NO][O2]2

Question 12

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 13

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. 
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 14

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

Accepted Answer

A)    
B)    
C)   
D) k = Ae(-Ea/RT) 
E)   
A)    
B)    
C)   
D) k = Ae(-Ea/RT) 
E)

Question 15

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

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 16

What is the overall order of the following reaction,given the rate law?
2NO(g)+ H2(g)→ N2(g)+ 2H2O(g)Rate = k[NO]2[H2]

Accepted Answer

A) 1st order 
B) 7th order 
C) 3rd order 
D) 4th order 
E) 0th order 
A) 1st order 
B) 7th order 
C) 3rd order 
D) 4th order 
E) 0th order

Question 17

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 75.0°C if Ea = 85.6 kJ/mol?

Accepted Answer

A) 3.47 × 104 s-1 
B) 1.92 × 104 s-1 
C) 670 s-1 
D) 3.85 × 106 s-1 
E) 1.36 × 102 s-1 
A) 3.47 × 104 s-1 
B) 1.92 × 104 s-1 
C) 670 s-1 
D) 3.85 × 106 s-1 
E) 1.36 × 102 s-1

Question 18

What is the overall order for the reaction?
2NO(g)+ 2H2(g)→ N2(g)+ 2H2O(g)

Accepted Answer

A) 3 
B) 4 
C) 2 
D) 1 
A) 3 
B) 4 
C) 2 
D) 1

Question 19

Give the characteristic of a second 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 20

Which statement is true for a catalyst?

Accepted Answer

A) A catalyst increases rate by providing a reaction path which has lower activation energy. 
B) A catalyst increases rate by decreasing the activation energy. 
C) A catalyst increases rate by increasing the activation energy. 
D) A catalyst increases rate by increasing the frequency factor A. 
A) A catalyst increases rate by providing a reaction path which has lower activation energy. 
B) A catalyst increases rate by decreasing the activation energy. 
C) A catalyst increases rate by increasing the activation energy. 
D) A catalyst increases rate by increasing the frequency factor A.

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

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?

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 rate constant (in s^-1)for the reaction?

The second-order reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 2.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl₂ loss is 4.84 × 10^-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

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?

Given the following proposed mechanism,predict the rate law for the overall reaction. 2NO₂ + Cl₂ → 2NO₂Cl (overall reaction) Mechanism NO₂ + Cl₂ → NO₂Cl + Cl slow NO₂ + Cl → NO₂Cl fast

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M.What is the rate constant for this reaction?

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)

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g)+ O₂(g)→ 2 NO₂(g)

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?

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

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

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

What is the overall order of the following reaction,given the rate law? 2NO(g)+ H₂(g)→ N₂(g)+ 2H₂O(g)Rate = k[NO]²[H₂]

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 75.0°C if E_a = 85.6 kJ/mol?

What is the overall order for the reaction? 2NO(g)+ 2H₂(g)→ N₂(g)+ 2H₂O(g)

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

Which statement is true for a catalyst?

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Exam 13: Chemical Kinetics

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

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?

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 rate constant (in s-1)for the reaction?

The second-order reaction 2 Mn(CO)5 → Mn2(CO)10,has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C.If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M,how long will it take for 90.% of the reactant to disappear?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl2 loss is 4.84 × 10-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl2(g)→ 2 NOCl(g)

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?

Given the following proposed mechanism,predict the rate law for the overall reaction. 2NO2 + Cl2 → 2NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.67 M.What is the rate constant for this reaction?

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)

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g)+ O2(g)→ 2 NO2(g)

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?

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

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

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

What is the overall order of the following reaction,given the rate law? 2NO(g)+ H2(g)→ N2(g)+ 2H2O(g)Rate = k[NO]2[H2]

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 75.0°C if Ea = 85.6 kJ/mol?

What is the overall order for the reaction? 2NO(g)+ 2H2(g)→ N2(g)+ 2H2O(g)

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

Which statement is true for a catalyst?

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

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Aqueous Ionic Equilibrium

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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?

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 rate constant (in s^-1)for the reaction?

The second-order reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 2.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

Given the following balanced equation,determine the rate of reaction with respect to [NOCl].If the rate of Cl₂ loss is 4.84 × 10^-2 M/s,what is the rate of formation of NOCl? 2 NO(g)+ Cl₂(g)→ 2 NOCl(g)

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?

Given the following proposed mechanism,predict the rate law for the overall reaction. 2NO₂ + Cl₂ → 2NO₂Cl (overall reaction) Mechanism NO₂ + Cl₂ → NO₂Cl + Cl slow NO₂ + Cl → NO₂Cl fast

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)

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g)+ O₂(g)→ 2 NO₂(g)

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?

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

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

What is the overall order of the following reaction,given the rate law? 2NO(g)+ H₂(g)→ N₂(g)+ 2H₂O(g)Rate = k[NO]²[H₂]

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 75.0°C if E_a = 85.6 kJ/mol?

What is the overall order for the reaction? 2NO(g)+ 2H₂(g)→ N₂(g)+ 2H₂O(g)