Question 1

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

Accepted Answer

A)  1st order 
B)  2nd order 
C)  3rd order 
D)  4th order 
E)  0th order 
A)  1st order 
B)  2nd order 
C)  3rd order 
D)  4th order 
E)  0th order C

Question 2

Identify the CFC with the shortest atmospheric lifetime.

Accepted Answer

A)  CFC-113 
B)  CFC-12 
C)  CFC-114 
D)  CFC-11 
E)  CFC-115 
A)  CFC-113 
B)  CFC-12 
C)  CFC-114 
D)  CFC-11 
E)  CFC-115 D

Question 3

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 
A)  0.491 s 
B)  0.204 s 
C)  0.236 s 
D)  0.424 s 
E)  0.294 s B

Question 4

Which rate law has a molecularity of two?

Accepted Answer

A)  Rate = k[A]0 
B)  Rate = k[A][B] 
C)  Rate = k[A][B][C] 
D)  Rate = k[A] 
E)  Rate = k[A]3 
A)  Rate = k[A]0 
B)  Rate = k[A][B] 
C)  Rate = k[A][B][C] 
D)  Rate = k[A] 
E)  Rate = k[A]3

Question 5

The rate constant for a zero-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 6

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 7

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

Accepted Answer

A)  4.28 × 10-4 yr-1 
B)  1.12 × 10-4 yr-1 
C)  2.33 × 10-4 yr-1 
D)  8.91 × 10-4 yr-1 
E)  6.17 × 10-4 yr-1 
A)  4.28 × 10-4 yr-1 
B)  1.12 × 10-4 yr-1 
C)  2.33 × 10-4 yr-1 
D)  8.91 × 10-4 yr-1 
E)  6.17 × 10-4 yr-1

Question 8

What are the units of k in the following rate law? Rate = k[X]2[Y]

Accepted Answer

A)    
B)    
C)  M2s2 
D)    
E)    
A)    
B)    
C)  M2s2 
D)    
E)

Question 9

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)  2 
C)  2.5 
D)  2.75 
E)  8 
A)  3 
B)  2 
C)  2.5 
D)  2.75 
E)  8

Question 10

Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen monoxide and oxygen according to the following chemical equation. 2 NO2(g)→ 2 NO(g)+ O2(g).
A sample of NO2(g)is initially placed in a 2.50-L reaction vessel at 300°C.If the half-life and the rate constant at 300°C are 11 seconds and 0.54 M-1 s-1,respectively,how many moles of NO2 were in the original sample?

Accepted Answer

A)  0.17 mol 
B)  0.42 mol 
C)  5.9 mol 
D)  15 mol 
A)  0.17 mol 
B)  0.42 mol 
C)  5.9 mol 
D)  15 mol

Question 11

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 1.33 M,what is the concentration of cyclopropane after 644 s?

Accepted Answer

A)  0.43 M 
B)  0.15 M 
C)  0.94 M 
D)  0.86 M 
E)  0.67 M 
A)  0.43 M 
B)  0.15 M 
C)  0.94 M 
D)  0.86 M 
E)  0.67 M

Question 12

Biological catalysts that increase the rates of biochemical reactions are known as

Accepted Answer

A)  substrates. 
B)  inhibitors. 
C)  enzymes. 
D)  binders. 
E)  trumanettes. 
A)  substrates. 
B)  inhibitors. 
C)  enzymes. 
D)  binders. 
E)  trumanettes.

Question 13

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

Accepted Answer

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

Question 14

Given the following proposed mechanism,predict the rate law for the overall reaction. A2 + 2 B → 2 AB (overall reaction)
Mechanism
A2 ⇌ 2 A fast
A + B → AB slow

Accepted Answer

A)  Rate = k[A]1/2[B]2 
B)  Rate = k[A2][B] 
C)  Rate = k[A2]2[B]1/2 
D)  Rate = k[A2]1/2 
E)  Rate = k[A2]1/2[B] 
A)  Rate = k[A]1/2[B]2 
B)  Rate = k[A2][B] 
C)  Rate = k[A2]2[B]1/2 
D)  Rate = k[A2]1/2 
E)  Rate = k[A2]1/2[B]

Question 15

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 16

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

Accepted Answer

A)  7 
B)  10 
C)  3 
D)  4 
E)  5 
A)  7 
B)  10 
C)  3 
D)  4 
E)  5

Question 17

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

Accepted Answer

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

Question 18

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

Accepted Answer

A)    N2 + O2 → 
 
  N2O 
B)  2 N2O → 2 N2 + O2 
C)  N2O → N2 + 2 O2 
D)    N2O →
  N2 + O2 
E)  2 N2 + O2 → 2 N2O 
A)    N2 + O2 → 
 
  N2O 
B)  2 N2O → 2 N2 + O2 
C)  N2O → N2 + 2 O2 
D)    N2O →
  N2 + O2 
E)  2 N2 + O2 → 2 N2O

Question 19

Given the following balanced equation,determine the rate of reaction with respect to [SO3]. 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

Carbon-14,which is present in all living tissue,radioactively decays via a first-order process.A one-gram sample of wood taken from a living tree gives a rate for carbon-14 decay of 13.6 counts per minute.If the half-life for carbon-14 is 5720 years,how old is a wood sample that gives a rate for carbon-14 decay of 11.9 counts per minute?

Accepted Answer

A)  5.3 × 102 yr 
B)  7.6 × 102 yr 
C)  1.1 × 103 yr 
D)  9.4 × 103 yr 
A)  5.3 × 102 yr 
B)  7.6 × 102 yr 
C)  1.1 × 103 yr 
D)  9.4 × 103 yr

Exam 14: Chemical Kinetics

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

Identify the CFC with the shortest atmospheric lifetime.

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

Which rate law has a molecularity of two?

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

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

The half-life for the decay of radium is 1620 years.What is the rate constant for this first-order process?

What are the units of k in the following rate law? Rate = k[X]2[Y]

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

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10-4 s-1.If the initial concentration of cyclopropane is 1.33 M,what is the concentration of cyclopropane after 644 s?

Biological catalysts that increase the rates of biochemical reactions are known as

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

Given the following proposed mechanism,predict the rate law for the overall reaction. A2 + 2 B → 2 AB (overall reaction) Mechanism A2 ⇌ 2 A fast A + B → AB slow

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?

If the concentration of a reactant is 6.25%,how many half-lives has it gone through?

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

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]. 2 SO2(g)+ O2(g)→ 2 SO3(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,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

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

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

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

What are the units of k in the following rate law? Rate = k[X]²[Y]

The first-order decomposition of cyclopropane has a rate constant of 6.7 × 10^-4 s^-1.If the initial concentration of cyclopropane is 1.33 M,what is the concentration of cyclopropane after 644 s?

Given the following proposed mechanism,predict the rate law for the overall reaction. A₂ + 2 B → 2 AB (overall reaction) Mechanism A₂ ⇌ 2 A fast A + B → AB slow

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