Question 1

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 1/2. 
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 1/2. 
D)  The rate of reaction will decrease by a factor of 2. 
E)  The rate of reaction will remain unchanged.

Question 2

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 102 M-1s-1 at 249 K,what is the rate constant at 436 K?

Accepted Answer

A)  2.38 × 105 M-1s-1 
B)  1.26 × 103 M-1s-1 
C)  7.94 × 104 M-1s-1 
D)  4.20 × 105 M-1s-1 
E)  3.80 × 104 M-1s-1 
A)  2.38 × 105 M-1s-1 
B)  1.26 × 103 M-1s-1 
C)  7.94 × 104 M-1s-1 
D)  4.20 × 105 M-1s-1 
E)  3.80 × 104 M-1s-1

Question 3

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

Accepted Answer

A)  1 
B)  4 
C)  1.5 
D)  3.5 
E)  2 
A)  1 
B)  4 
C)  1.5 
D)  3.5 
E)  2

Question 4

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 5

Which rate law has a molecularity of three?

Accepted Answer

A)  Rate = k[A]0 
B)  Rate = k[A][B]2 
C)  Rate = k[A][B] 
D)  Rate = k[A] 
E)  Rate = k[A]2 
A)  Rate = k[A]0 
B)  Rate = k[A][B]2 
C)  Rate = k[A][B] 
D)  Rate = k[A] 
E)  Rate = k[A]2

Question 6

Identify the methods used to monitor a reaction as it occurs in the reaction flask.

Accepted Answer

A)  polarimeter 
B)  spectrometer 
C)  pressure measurement 
D)  none of the above 
E)  all of the above 
A)  polarimeter 
B)  spectrometer 
C)  pressure measurement 
D)  none of the above 
E)  all of the above

Question 7

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

Accepted Answer

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

Question 8

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

Accepted Answer

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

Question 9

Which of the following statements is FALSE?

Accepted Answer

A)  The average rate of a reaction decreases during a reaction. 
B)  It is not possible to determine the rate of a reaction from its balanced equation. 
C)  The rate of zero-order reactions is not dependent on concentration. 
D)  The half-life of a first-order reaction is dependent on the initial concentration of reactant. 
E)  None of the statements is FALSE. 
A)  The average rate of a reaction decreases during a reaction. 
B)  It is not possible to determine the rate of a reaction from its balanced equation. 
C)  The rate of zero-order reactions is not dependent on concentration. 
D)  The half-life of a first-order reaction is dependent on the initial concentration of reactant. 
E)  None of the statements is FALSE.

Question 10

Hydrogen iodide decomposes at 800 K via a second-order process to produce hydrogen and iodine according to the following chemical equation. 2 HI(g)→ H2(g)+ I2(g)
At 800 K it takes 142 seconds for the initial concentration of HI to decrease from 6.75 × 10-2 M to 3.50 × 10-2 M.What is the rate constant for the reaction at this temperature?

Accepted Answer

A)  5.12 × 10-4 M-1s-1 
B)  9.69 × 10-2 M-1s-1 
C)  10.3 M-1s-1 
D)  1.95 × 103 M-1s-1 
A)  5.12 × 10-4 M-1s-1 
B)  9.69 × 10-2 M-1s-1 
C)  10.3 M-1s-1 
D)  1.95 × 103 M-1s-1

Question 11

The first-order reaction,2 N2O(g)→ 2 N2(g)+ O2(g),has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Accepted Answer

A)  0.62 s 
B)  2.8 s 
C)  6.3 s 
D)  8.4 s 
A)  0.62 s 
B)  2.8 s 
C)  6.3 s 
D)  8.4 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 is 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 is true.

Question 13

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 14

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g)
Is first order in CH3NC.The rate constant for the reaction is 9.45 × 10-5 s-1 at 478 K.The half-life of the reaction when the initial [CH3NC] is 0.030 M is ________ s.

Accepted Answer

A)  1.06 × 104 
B)  5.29 × 103 
C)  3.53 × 105 
D)  7.33 × 103 
E)  1.36 × 10-4 
A)  1.06 × 104 
B)  5.29 × 103 
C)  3.53 × 105 
D)  7.33 × 103 
E)  1.36 × 10-4

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

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

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.

Which rate law has a molecularity of three?

Identify the methods used to monitor a reaction as it occurs in the reaction flask.

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

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

Which of the following statements is FALSE?

The first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

Which of the following statements is TRUE?

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

The isomerization of methylisonitrile to acetonitrile CH₃NC(g)→ CH₃CN(g) Is first order in CH₃NC.The rate constant for the reaction is 9.45 × 10^-5 s^-1 at 478 K.The half-life of the reaction when the initial [CH₃NC] is 0.030 M is ________ s.

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

Exam 14: Chemical Kinetics

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

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 102 M-1s-1 at 249 K,what is the rate constant at 436 K?

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value?

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.

Which rate law has a molecularity of three?

Identify the methods used to monitor a reaction as it occurs in the reaction flask.

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

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

Which of the following statements is FALSE?

The first-order reaction,2 N2O(g)→ 2 N2(g)+ O2(g),has a rate constant equal to 0.76 s-1 at 1000 K.How long will it take for the concentration of N2O to decrease to 12% of its initial concentration?

Which of the following statements is TRUE?

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

The isomerization of methylisonitrile to acetonitrile CH3NC(g)→ CH3CN(g) Is first order in CH3NC.The rate constant for the reaction is 9.45 × 10-5 s-1 at 478 K.The half-life of the reaction when the initial [CH3NC] is 0.030 M is ________ s.

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

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

A reaction is found to have an activation energy of 38.0 kJ/mol.If the rate constant for this reaction is 1.60 × 10² M^-1s^-1 at 249 K,what is the rate constant at 436 K?

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.

The first-order reaction,2 N₂O(g)→ 2 N₂(g)+ O₂(g),has a rate constant equal to 0.76 s^-1 at 1000 K.How long will it take for the concentration of N₂O to decrease to 12% of its initial concentration?

The isomerization of methylisonitrile to acetonitrile CH₃NC(g)→ CH₃CN(g) Is first order in CH₃NC.The rate constant for the reaction is 9.45 × 10^-5 s^-1 at 478 K.The half-life of the reaction when the initial [CH₃NC] is 0.030 M is ________ s.