Question 1

With respect to the figure below, which choice correctly identifies all the numbered positions?

Accepted Answer

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

Question 2

Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 
2ClO2(aq)+ 2OH-(aq) $\rarr$ClO2-(aq)+ ClO3-(aq)+ H2O(l)
A kinetic study of this reaction under a certain set of conditions yielded the data below.    
 Which one of the following is the rate law for this reaction?

Accepted Answer

A) rate = k[ClO2][OH-] 
B) rate = k[ClO2]2[OH-] 
C) rate = k[ClO2][OH-]2 
D) rate = k[ClO2]2[OH-]2 
E) rate = k[ClO2]4[OH-] 
A) rate = k[ClO2][OH-] 
B) rate = k[ClO2]2[OH-] 
C) rate = k[ClO2][OH-]2 
D) rate = k[ClO2]2[OH-]2 
E) rate = k[ClO2]4[OH-]

Question 3

Concerning the rate law, Rate = k[A][B], what are appropriate units for the rate constant k?

Accepted Answer

A) s-1 
B) M-1s-1 
C) M-2s-1 
D) M/s 
E) M2/s 
A) s-1 
B) M-1s-1 
C) M-2s-1 
D) M/s 
E) M2/s

Question 4

The isomerization of cyclopropane follows first order kinetics.The rate constant at 700 K is 6.20 × 10-4 min-1, and the half-life at 760 K is 29.0 min.Calculate the activation energy for this reaction.

Accepted Answer

A) 5.07 kJ/mol 
B) 27.0 kJ/mol 
C) 50.7 kJ/mol 
D) 60.kJ/mol 
E) 270.kJ/mol 
A) 5.07 kJ/mol 
B) 27.0 kJ/mol 
C) 50.7 kJ/mol 
D) 60.kJ/mol 
E) 270.kJ/mol

Question 5

Aspirin, C9H8O4, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, HC2H3O2, and 2-hydroxybenzoic acid, C7H6O3 (this is why old bottles of aspirin often smell like vinegar):
C9H8O4 + H2O $\rarr$HC2H3O2 + C7H6O3
  
Concentration and rate data for this reaction are given below.    
Write the rate law for this reaction and calculate k (be sure to include the correct units).

Accepted Answer

The rate law is rate

Question 6

For the reaction X + Y $\rarr$Z, the reaction rate is found to depend only upon the concentration of X.A plot of 1/X verses time gives a straight line.

What is the rate law for this reaction?

Accepted Answer

A) rate = k [X] 
B) rate = k [X]2 
C) rate = k [X][Y] 
D) rate = k [X]2[Y] 
A) rate = k [X] 
B) rate = k [X]2 
C) rate = k [X][Y] 
D) rate = k [X]2[Y]

Question 7

When the concentrations of reactant molecules are increased, the rate of reaction increases.The best explanation for this phenomenon is that as the reactant concentration increases,

Accepted Answer

A) the average kinetic energy of molecules increases. 
B) the frequency of molecular collisions increases. 
C) the rate constant increases. 
D) the activation energy increases. 
E) the order of reaction increases. 
A) the average kinetic energy of molecules increases. 
B) the frequency of molecular collisions increases. 
C) the rate constant increases. 
D) the activation energy increases. 
E) the order of reaction increases.

Question 8

A certain first-order reaction A $\rarr$ B is 25% complete in 42 min at 25°C.What is the half-life of the reaction?

Accepted Answer

A) 21 min 
B) 42 min 
C) 84 min 
D) 20 min 
E) 101 min 
A) 21 min 
B) 42 min 
C) 84 min 
D) 20 min 
E) 101 min

Question 9

The graphs below all refer to the same reaction.What is the order of this reaction?

Accepted Answer

A) zero order 
B) first order 
C) second order 
D) unable to predict 
A) zero order 
B) first order 
C) second order 
D) unable to predict

Question 10

Nitric acid is formed by the gas-phase hydrolysis of N2O5.Draw an energy profile curve for the reaction N2O5 + H2O $\rarr$2HNO3 given that Ea(forward)= 15 kJ and Ea(reverse)= 51 kJ/mol.Label the activation energies of the forward and reverse reactions and label $\Delta$H for the reaction.

Accepted Answer

With respect to the figure below, which choice correctly identifies all the numbered positions?

Concerning the rate law, Rate = k[A][B], what are appropriate units for the rate constant k?

The isomerization of cyclopropane follows first order kinetics.The rate constant at 700 K is 6.20 × 10^-4min^-1, and the half-life at 760 K is 29.0 min.Calculate the activation energy for this reaction.

When the concentrations of reactant molecules are increased, the rate of reaction increases.The best explanation for this phenomenon is that as the reactant concentration increases,

A certain first-order reaction A $\rarr$ B is 25% complete in 42 min at 25°C.What is the half-life of the reaction?

The graphs below all refer to the same reaction.What is the order of this reaction?

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

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Exam 13: Chemical Kinetics

With respect to the figure below, which choice correctly identifies all the numbered positions?

Concerning the rate law, Rate = k[A][B], what are appropriate units for the rate constant k?

The isomerization of cyclopropane follows first order kinetics.The rate constant at 700 K is 6.20 × 10-4 min-1, and the half-life at 760 K is 29.0 min.Calculate the activation energy for this reaction.

For the reaction X + Y →\rarr→ Z, the reaction rate is found to depend only upon the concentration of X.A plot of 1/X verses time gives a straight line. What is the rate law for this reaction?

When the concentrations of reactant molecules are increased, the rate of reaction increases.The best explanation for this phenomenon is that as the reactant concentration increases,

A certain first-order reaction A →\rarr→ B is 25% complete in 42 min at 25°C.What is the half-life of the reaction?

The graphs below all refer to the same reaction.What is the order of this reaction?

Nitric acid is formed by the gas-phase hydrolysis of N2O5.Draw an energy profile curve for the reaction N2O5 + H2O →\rarr→ 2HNO3 given that Ea(forward)= 15 kJ and Ea(reverse)= 51 kJ/mol.Label the activation energies of the forward and reverse reactions and label Δ\DeltaΔ H for the reaction.

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

The isomerization of cyclopropane follows first order kinetics.The rate constant at 700 K is 6.20 × 10^-4min^-1, and the half-life at 760 K is 29.0 min.Calculate the activation energy for this reaction.

A certain first-order reaction A $\rarr$ B is 25% complete in 42 min at 25°C.What is the half-life of the reaction?