Question 1

The first-order reaction SO2Cl2 $\rarr$ SO2 + Cl2 is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

Accepted Answer

A) 1.8 min 
B) 104 min 
C) 530 min 
D) 2300 min 
E) 990 min 
A) 1.8 min 
B) 104 min 
C) 530 min 
D) 2300 min 
E) 990 min D

Question 2

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Accepted Answer

A) 3 
B) 6 
C) 9 
D) 27 
E) 30 
A) 3 
B) 6 
C) 9 
D) 27 
E) 30 C

Question 3

The following initial rate data apply to the reaction below. F2(g)+ 2Cl2O(g) $\rarr$ 2FClO2(g)+ Cl2(g)   Which of the following is the rate law (rate equation)for this reaction?

Accepted Answer

A) rate = k[F2]2[Cl2O]4 
B) rate = k[F2]2[Cl2O] 
C) rate = k[F2][Cl2O] 
D) rate = k[F2][Cl2O]2 
E) rate = k[F2]2[Cl2O]2 
A) rate = k[F2]2[Cl2O]4 
B) rate = k[F2]2[Cl2O] 
C) rate = k[F2][Cl2O] 
D) rate = k[F2][Cl2O]2 
E) rate = k[F2]2[Cl2O]2 C

Question 4

The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H3AsO4 + 3I - + 2 H3O + $\rarr$H3AsO3 + I3- + H2O. The experimental rate law for this reaction is
Rate = k [H3AsO4] [I-] [H3O+].
According to the rate law for the reaction, an increase in the concentration of hydronium ion has what effect on this reaction?

Accepted Answer

The rate of reaction

Question 5

Ammonium ion (NH4+)reacts with nitrite ion (NO2-)to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations.   Which of the following is the rate law (rate equation)for this reaction?

Accepted Answer

A) rate = k [NH4+] [NO2-]4 
B) rate = k [NH4+] [NO2-] 
C) rate = k [NH4+] [NO2-]2 
D) rate = k [NH4+]2 [NO2-] 
E) rate = k [NH4+]1/2 [NO2-]1/4 
A) rate = k [NH4+] [NO2-]4 
B) rate = k [NH4+] [NO2-] 
C) rate = k [NH4+] [NO2-]2 
D) rate = k [NH4+]2 [NO2-] 
E) rate = k [NH4+]1/2 [NO2-]1/4

Question 6

Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + 1/2Cl2 $\rarr$ NOCl

Accepted Answer

A) rate = k[NO] 
B) rate = k[NO][Cl2]1/2 
C) rate = k[NO][Cl2] 
D) rate = k[NO]2[Cl2] 
E) rate = k[NO]2[Cl2]2 
A) rate = k[NO] 
B) rate = k[NO][Cl2]1/2 
C) rate = k[NO][Cl2] 
D) rate = k[NO]2[Cl2] 
E) rate = k[NO]2[Cl2]2

Question 7

The isomerization of cyclopropane to form propene is a first-order reaction.   At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

Accepted Answer

A) 3.66 * 10-2 min-1 
B) 1.04 * 10-2 min-1 
C) 2.42 min-1 
D) 2.06 * 10-3 min-1 
E) 2.40 * 10-2 min-1 
A) 3.66 * 10-2 min-1 
B) 1.04 * 10-2 min-1 
C) 2.42 min-1 
D) 2.06 * 10-3 min-1 
E) 2.40 * 10-2 min-1

Question 8

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g)$\rarr$ 2NO2(g)+ 1/2O2(g)
The value of the rate constant (k)is 1.35 * 10-4 s-1  at 35°C. What is the value of k at 0°C?

Accepted Answer

A) 8.2 * 10-7 s-1 
B) 1.9 * 10-5 s-1 
C) 4.2 * 10-5 s-1 
D) 2.2 * 10-2 s-1 
E) none of these 
A) 8.2 * 10-7 s-1 
B) 1.9 * 10-5 s-1 
C) 4.2 * 10-5 s-1 
D) 2.2 * 10-2 s-1 
E) none of these

Question 9

At 25°C, the second-order reaction NOCl(g)$\rarr$ NO(g)+ 1/2Cl2(g) is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Accepted Answer

A) 8.22 hr 
B) 11.6 hr 
C) 15.5 hr 
D) 17.5 hr 
E) 23.0 hr 
A) 8.22 hr 
B) 11.6 hr 
C) 15.5 hr 
D) 17.5 hr 
E) 23.0 hr

Question 10

Which one of the following units would not be an acceptable way to express reaction rate?

Accepted Answer

A) M/s 
B) M. min-1 
C) L .mol-1 . s-1 
D) mol. L-1 .s-1 
E) mmHg/min 
A) M/s 
B) M. min-1 
C) L .mol-1 . s-1 
D) mol. L-1 .s-1 
E) mmHg/min

Question 11

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO $\rarr$ NO + CO2
 Which one of the following mechanisms is consistent with the observed reaction order?

Accepted Answer

A) NO2 + 2CO $\rarr$ N + 2CO2 fast N + NO2 $\rarr$ 2NO slow 
B) NO2 + 2CO $\rarr$ N + 2CO2 slow N + NO2 $\rarr$ 2NO fast 
C) NO2 + NO2 $\rarr$ NO3 + NO fast NO3 + CO $\rarr$ NO2 + CO2 slow 
D) NO2 + NO2 $\rarr$ NO3 + NO slow NO3 + CO $\rarr$ NO2 + CO2 fast 
A) NO2 + 2CO $\rarr$ N + 2CO2 fast N + NO2 $\rarr$ 2NO slow 
B) NO2 + 2CO $\rarr$ N + 2CO2 slow N + NO2 $\rarr$ 2NO fast 
C) NO2 + NO2 $\rarr$ NO3 + NO fast NO3 + CO $\rarr$ NO2 + CO2 slow 
D) NO2 + NO2 $\rarr$ NO3 + NO slow NO3 + CO $\rarr$ NO2 + CO2 fast

Question 12

A reaction mechanism usually is

Accepted Answer

A) the same as the balanced chemical equation. 
B) restricted to only one possible explanation. 
C) obvious if the reaction order is known. 
D) difficult, if not impossible, to prove. 
E) obvious if the activation energy is known. 
A) the same as the balanced chemical equation. 
B) restricted to only one possible explanation. 
C) obvious if the reaction order is known. 
D) difficult, if not impossible, to prove. 
E) obvious if the activation energy is known.

Question 13

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

Accepted Answer

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

Question 14

For the chemical reaction A $\rarr$ B + C, a plot of [A]t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

Accepted Answer

A) zeroth 
B) first 
C) second 
D) third 
E) Such a plot cannot reveal the order of the reaction. 
A) zeroth 
B) first 
C) second 
D) third 
E) Such a plot cannot reveal the order of the reaction.

Question 15

The rate law predicted by the following two-step mechanism is rate = k[A][B].
A $\rarr$  C + B slow
A + B $\rarr$ C + E fast

Accepted Answer

A) True 
 B)False

Question 16

For the reaction C6H14(g)$\rarr$ C6H6(g)+ 4H2(g), $\Delta$P(H2)/$\Delta$t was found to be 2.5 * 10-2 atm/s, where $\Delta$P(H2)is the change in pressure of hydrogen. Determine $\Delta$P(C6H14)/$\Delta$t for this reaction at the same time.

Accepted Answer

A) 2.5 * 10-2 atm/s 
B) -6.2 * 10-3 atm/s 
C) -2.5 * 10-2 atm/s 
D) 0.10 atm/s 
E) 6.2 * 10-3 atm/s 
A) 2.5 * 10-2 atm/s 
B) -6.2 * 10-3 atm/s 
C) -2.5 * 10-2 atm/s 
D) 0.10 atm/s 
E) 6.2 * 10-3 atm/s

Question 17

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 18

For what order reaction does the half-life get longer as the initial concentration increases?

Accepted Answer

A) zeroth order 
B) first order 
C) second order 
D) none of them because half-life is always independent of the initial concentration 
A) zeroth order 
B) first order 
C) second order 
D) none of them because half-life is always independent of the initial concentration

Question 19

The reaction A + 2B $\rarr$ products was found to follow the rate law: rate = k[A]2[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

Accepted Answer

A) 5 
B) 6 
C) 12 
D) 18 
E) None of these. 
A) 5 
B) 6 
C) 12 
D) 18 
E) None of these.

Question 20

A first-order reaction has a rate constant of 3.00 * 10-3 s-1. The time required for the reaction to be 75.0% complete is

Accepted Answer

A) 95.8 s. 
B) 462 s. 
C) 231 s. 
D) 201 s. 
E) 41.7 s. 
A) 95.8 s. 
B) 462 s. 
C) 231 s. 
D) 201 s. 
E) 41.7 s.

The first-order reaction SO₂Cl₂ $\rarr$ SO₂ + Cl₂ is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Ammonium ion (NH₄⁺)reacts with nitrite ion (NO₂^-)to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation)for this reaction?

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g)+ ¹/₂O₂(g) The value of the rate constant (k)is 1.35 * 10^-4 s^-1 at 35°C. What is the value of k at 0°C?

At 25°C, the second-order reaction NOCl(g) $\rarr$ NO(g)+ ¹/₂Cl₂(g)is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Which one of the following units would not be an acceptable way to express reaction rate?

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO $\rarr$ NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?

A reaction mechanism usually is

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

For the chemical reaction A $\rarr$ B + C, a plot of [A]_t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

The rate law predicted by the following two-step mechanism is rate = k[A][B]. A $\rarr$ C + B slow A + B $\rarr$ C + E fast

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g)+ 4H₂(g), $\Delta$ P(H₂)/ $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂)is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄)/ $\Delta$ t for this reaction at the same time.

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?

For what order reaction does the half-life get longer as the initial concentration increases?

The reaction A + 2B $\rarr$ products was found to follow the rate law: rate = k[A]²[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

A first-order reaction has a rate constant of 3.00 * 10^-3s^-1. The time required for the reaction to be 75.0% complete is

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 14: Chemical Kinetics

The first-order reaction SO2Cl2 →\rarr→ SO2 + Cl2 is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

The reaction A + 2B →\rarr→ products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

The following initial rate data apply to the reaction below. F2(g)+ 2Cl2O(g) →\rarr→ 2FClO2(g)+ Cl2(g) Which of the following is the rate law (rate equation)for this reaction?

Ammonium ion (NH4+)reacts with nitrite ion (NO2-)to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation)for this reaction?

Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + 1/2Cl2 →\rarr→ NOCl

The isomerization of cyclopropane to form propene is a first-order reaction. At 760 K, 85% of a sample of cyclopropane changes to propene in 79.0 min. Determine the rate constant for this reaction at 760 K.

The activation energy for the following first-order reaction is 102 kJ/mol. N2O5(g) →\rarr→ 2NO2(g)+ 1/2O2(g) The value of the rate constant (k)is 1.35 * 10-4 s-1 at 35°C. What is the value of k at 0°C?

At 25°C, the second-order reaction NOCl(g) →\rarr→ NO(g)+ 1/2Cl2(g) is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

Which one of the following units would not be an acceptable way to express reaction rate?

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO2, and zeroth-order with respect to CO below 25°C. NO2 + CO →\rarr→ NO + CO2 Which one of the following mechanisms is consistent with the observed reaction order?

A reaction mechanism usually is

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

For the chemical reaction A →\rarr→ B + C, a plot of [A]t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

The rate law predicted by the following two-step mechanism is rate = k[A][B]. A →\rarr→ C + B slow A + B →\rarr→ C + E fast

For the reaction C6H14(g) →\rarr→ C6H6(g)+ 4H2(g), Δ\DeltaΔ P(H2)/ Δ\DeltaΔ t was found to be 2.5 * 10-2 atm/s, where Δ\DeltaΔ P(H2)is the change in pressure of hydrogen. Determine Δ\DeltaΔ P(C6H14)/ Δ\DeltaΔ t for this reaction at the same time.

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?

For what order reaction does the half-life get longer as the initial concentration increases?

The reaction A + 2B →\rarr→ products was found to follow the rate law: rate = k[A]2[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

A first-order reaction has a rate constant of 3.00 * 10-3 s-1. The time required for the reaction to be 75.0% complete is

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

The first-order reaction SO₂Cl₂ $\rarr$ SO₂ + Cl₂ is 10% complete in 80. min. How long would it take for the reaction to be 95% complete?

The reaction A + 2B $\rarr$ products has been found to have the rate law, rate = k[A] [B]². While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases.

Ammonium ion (NH₄⁺)reacts with nitrite ion (NO₂^-)to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Which of the following is the rate law (rate equation)for this reaction?

The activation energy for the following first-order reaction is 102 kJ/mol. N₂O₅(g) $\rarr$ 2NO₂(g)+ ¹/₂O₂(g) The value of the rate constant (k)is 1.35 * 10^-4 s^-1 at 35°C. What is the value of k at 0°C?

At 25°C, the second-order reaction NOCl(g) $\rarr$ NO(g)+ ¹/₂Cl₂(g)is 50% complete after 5.82 hours when the initial concentration of NOCl is 4.46 mol/L. How long will it take for the reaction to be 75% complete?

The gas phase reaction of nitrogen dioxide and carbon monoxide was found by experiment to be second-order with respect to NO₂, and zeroth-order with respect to CO below 25°C. NO₂ + CO $\rarr$ NO + CO₂ Which one of the following mechanisms is consistent with the observed reaction order?

For the chemical reaction A $\rarr$ B + C, a plot of [A]_t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A?

The rate law predicted by the following two-step mechanism is rate = k[A][B]. A $\rarr$ C + B slow A + B $\rarr$ C + E fast

For the reaction C₆H₁₄(g) $\rarr$ C₆H₆(g)+ 4H₂(g), $\Delta$ P(H₂)/ $\Delta$ t was found to be 2.5 * 10^-2 atm/s, where $\Delta$ P(H₂)is the change in pressure of hydrogen. Determine $\Delta$ P(C₆H₁₄)/ $\Delta$ t for this reaction at the same time.

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 reaction A + 2B $\rarr$ products was found to follow the rate law: rate = k[A]²[B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled, the concentration of B is tripled, and the temperature remains constant.

A first-order reaction has a rate constant of 3.00 * 10^-3s^-1. The time required for the reaction to be 75.0% complete is