Butadiene, C4H6 (used to make synthetic rubber and latex paints) reacts to C8H12 with a rate law of rate = 0.014 L/(mol·s) [C4H6]2. What will be the concentration of C4H6 after 3.0 hours if the initial concentration is 0.025 M?

A) 0.0052 M B) 0.024 M C) 43 M D) 190 M E) 0.0000 M A) 0.0052 M B) 0.024 M C) 43 M D) 190 M E) 0.0000 M

The rate law for the rearrangement of CH3NC to CH3CN at 800 K is Rate = (1300 s-1)[CH3NC]. What is the half-life for this reaction?

A) 7.69 × 10-4 s B) 5.3 × 10-4 s C) 1.9 × 10-3 s D) 520 s E) 1920 s A) 7.69 × 10-4 s B) 5.3 × 10-4 s C) 1.9 × 10-3 s D) 520 s E) 1920 s

The rate constant for the reaction 3A F1F1F1S1F1F1F10 4B is 6.00 × 10-3 L mol-1min-1. How long will it take the concentration of A to drop from 0.75 M to 0.25 M?

A) 2.2 × 10-3 min B) 5.5 × 10-3 min C) 180 min D) 440 min E) 5.0 × 102 min A) 2.2 × 10-3 min B) 5.5 × 10-3 min C) 180 min D) 440 min E) 5.0 × 102 min

Consider the general reaction 5Br-(aq) + BrO3-(aq) + 6H+(aq) F1F1F1S1F1F1F10 3Br2(aq) + 3H2O(aq) For this reaction, the rate when expressed as F1F1F1S1F1F1F10[Br2]/F1F1F1S1F1F1F10t is the same as

A) -F1F1F1S1F1F1F10[H2O]/F1F1F1S1F1F1F10t B) 3F1F1F1S1F1F1F10[BrO3-]/F1F1F1S1F1F1F10t C) -5F1F1F1S1F1F1F10[Br-]/F1F1F1S1F1F1F10t D) -0.6F1F1F1S1F1F1F10[Br-]/F1F1F1S1F1F1F10t E) none of the above A) -F1F1F1S1F1F1F10[H2O]/F1F1F1S1F1F1F10t B) 3F1F1F1S1F1F1F10[BrO3-]/F1F1F1S1F1F1F10t C) -5F1F1F1S1F1F1F10[Br-]/F1F1F1S1F1F1F10t D) -0.6F1F1F1S1F1F1F10[Br-]/F1F1F1S1F1F1F10t E) none of the above

Sulfuryl chloride, SO2Cl2(g), decomposes at high temperature to form SO2(g) and Cl2(g). The rate constant at a certain temperature is 4.68 × 10-5s-1. What is the order of the reaction?

A) zero B) first C) second D) third E) More information is needed to determine the order. A) zero B) first C) second D) third E) More information is needed to determine the order.

The gas-phase reaction CH3NC F1F1F1S1F1F1F10 CH3CN has been studied in a closed vessel, and the rate equation was found to be: Rate = -F1F1F1S1F1F1F10[CH3NC]/F1F1F1S1F1F1F10t = k[CH3NC]. Which one of the following actions is least likely to cause a change in the rate of the reaction?

A) lowering the temperature B) adding a catalyst C) using a larger initial amount of CH3NC in the same vessel D) using a bigger vessel, but the same initial amount of CH3NC E) continuously removing CH3CN as it is formed A) lowering the temperature B) adding a catalyst C) using a larger initial amount of CH3NC in the same vessel D) using a bigger vessel, but the same initial amount of CH3NC E) continuously removing CH3CN as it is formed

A first-order reaction has a half-life of 20.0 minutes. Starting with 1.00 × 1020 molecules of reactant at time t = 0, how many molecules remain unreacted after 100.0 minutes?

A) 1.00 × 104 molecules B) 2.00 × 1019 molecules C) 3.20 × 1016 molecules D) 5.00 × 1020 molecules E) none of the above A) 1.00 × 104 molecules B) 2.00 × 1019 molecules C) 3.20 × 1016 molecules D) 5.00 × 1020 molecules E) none of the above

Tetrafluoroethylene, C2F4, can be converted to octafluorocyclobutane which can be used as a refrigerant or an aerosol propellant. A plot of 1/[C2F4] vs. time gives a straight line with a slope of 0.0448 L mol-1s-1. What is the rate law for this reaction?

A) Rate = 0.0448 (L mol-1s-1)[C2F4] B) Rate = 22.3 (mol L-1s)[C2F4] C) Rate = 0.0448 (L mol-1s-1)[C2F4]2 D) Rate = 22.3 (mol L-1s)[C2F4]2 E) Rate = 0.0448 s-1 [C2F4] A) Rate = 0.0448 (L mol-1s-1)[C2F4] B) Rate = 22.3 (mol L-1s)[C2F4] C) Rate = 0.0448 (L mol-1s-1)[C2F4]2 D) Rate = 22.3 (mol L-1s)[C2F4]2 E) Rate = 0.0448 s-1 [C2F4]

Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 2.5 × 103 s-1 at -5°C and k = 3.5 × 104 s-1 at 25°C, what is the activation energy for the decomposition?

A) 0.73 kJ/mol B) 58 kJ/mol C) 140 kJ/mol D) 580 kJ/mol E) > 1000 kJ/mol A) 0.73 kJ/mol B) 58 kJ/mol C) 140 kJ/mol D) 580 kJ/mol E) > 1000 kJ/mol

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 164.5°C to 179.0°C, the rate constantincreases by a factor of 4.27. What is the activation energy of this oxidation reaction?

(Multiple Choice)

4.8/5

(34)

Question 21

Butadiene, C₄H₆ (used to make synthetic rubber and latex paints) reacts to C₈H₁₂ with a rate law of rate = 0.014 L/(mol·s) [C₄H₆]². What will be the concentration of C₄H₆after 3.0 hours if the initial concentration is 0.025 M?

(Multiple Choice)

4.9/5

(46)

Question 22

The rate law for the rearrangement of CH₃NC to CH₃CN at 800 K is Rate = (1300 s^-1)[CH₃NC]. What is the half-life for this reaction?

(Multiple Choice)

4.8/5

(38)

Question 23

All bimolecular reactions are second-order reactions.

(True/False)

4.9/5

(41)

Question 24

The rate constant for the reaction 3A  4B is 6.00 × 10^-3 L mol^-1min^-1. How long will it take the concentration of A to drop from 0.75 M to 0.25 M?

(Multiple Choice)

4.8/5

(37)

Question 25

At 25.0°C, a rate constant has the value 5.21 × 10^-8 L mol^-1 s^-1. If the activation energy is 75.2 kJ/mol, calculate the rate constant when the temperature is 50.0°C.

(Short Answer)

4.9/5

(37)

Question 26

Consider the general reaction 5Br^-(aq) + BrO₃^-(aq) + 6H⁺(aq)  3Br₂(aq) + 3H₂O(aq) For this reaction, the rate when expressed as [Br₂]/t is the same as

(Multiple Choice)

4.8/5

(45)

Question 27

Reaction intermediates differ from activated complexes in that

(Multiple Choice)

4.8/5

(42)

Question 28

The half-life of a second-order reaction does not depend on the initial concentration of reactant.

(True/False)

4.9/5

(37)

Question 29

Sulfuryl chloride, SO₂Cl₂(g), decomposes at high temperature to form SO₂(g) and Cl₂(g). The rate constant at a certain temperature is 4.68 × 10^-5s^-1. What is the order of the reaction?

(Multiple Choice)

4.8/5

(39)

Question 30

The gas-phase reaction CH₃NC  CH₃CN has been studied in a closed vessel, and the rate equation was found to be: Rate = -[CH₃NC]/t = k[CH₃NC]. Which one of the following actions is least likely to cause a change in the rate of the reaction?

(Multiple Choice)

4.8/5

(35)

Question 31

For each of the following terms/concepts, give a brief explanation or definition. Where possible, use examples. a. order of a reaction b. elementary reaction c. reaction intermediate

(Essay)

4.8/5

(33)

Question 32

The elementary reaction HBr(g) + Br(g)  H(g) + Br₂(g) is endothermic. a. Would you expect the rate constant for the back reaction to be smaller or larger than that for the forward reaction? Explain, briefly. b. Draw a fully-labeled reaction energy diagram for this reaction, showing the locations of the reactants, products, and transition state.

(Essay)

4.8/5

(35)

Question 33

A first-order reaction has a half-life of 20.0 minutes. Starting with 1.00 × 10²⁰ molecules of reactant at time t = 0, how many molecules remain unreacted after 100.0 minutes?

(Multiple Choice)

4.8/5

(40)

Question 34

Tetrafluoroethylene, C₂F₄, can be converted to octafluorocyclobutane which can be used as a refrigerant or an aerosol propellant. A plot of 1/[C₂F₄] vs. time gives a straight line with a slope of 0.0448 L mol^-1s^-1. What is the rate law for this reaction?

(Multiple Choice)

4.8/5

(29)

Question 35

A reaction has the following rate law: Rate = k[A][B]² In experiment 1, the concentrations of A and B are both 0.10 mol L^-1; in experiment 2, the concentrations are both 0.30 mol L^-1. If the temperature stays constant, what is the value of the ratio, Rate(2)/Rate(1)?

(Multiple Choice)

4.8/5

(36)

Question 36

In the gas phase at 500.°C, cyclopropane reacts to form propene in a first-order reaction. The figure below shows the concentration of cyclopropane plotted versus time. Use the graph to calculate approximate values of a. the rate of the reaction, 600. seconds after the start. b. the half-life of the reaction, t_1/2.

(Essay)

4.9/5

(41)

Question 37

An increase in temperature increases the reaction rate because

(Multiple Choice)

5.0/5

(37)

Question 38

Chlorine atoms act as heterogeneous catalysts in the destruction of ozone in the stratosphere.

(True/False)

4.9/5

(35)

Question 39

Dinitrogen tetraoxide, N₂O₄, decomposes to nitrogen dioxide, NO₂, in a first-order process. If k = 2.5 × 10³s^-1 at -5°C and k = 3.5 × 10⁴ s^-1 at 25°C, what is the activation energy for the decomposition?

(Multiple Choice)

4.8/5

(38)

Question 40

Showing 21 - 40 of 88

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 164.5°C to 179.0°C, the rate constant increases by a factor of 4.27. What is the activation energy of this oxidation reaction?

Butadiene, C4H6 (used to make synthetic rubber and latex paints) reacts to C8H12 with a rate law of rate = 0.014 L/(mol·s) [C4H6]2. What will be the concentration of C4H6 after 3.0 hours if the initial concentration is 0.025 M?

The rate law for the rearrangement of CH3NC to CH3CN at 800 K is Rate = (1300 s-1)[CH3NC]. What is the half-life for this reaction?

All bimolecular reactions are second-order reactions.

The rate constant for the reaction 3A  4B is 6.00 × 10-3 L mol-1min-1. How long will it take the concentration of A to drop from 0.75 M to 0.25 M?

At 25.0°C, a rate constant has the value 5.21 × 10-8 L mol-1 s-1. If the activation energy is 75.2 kJ/mol, calculate the rate constant when the temperature is 50.0°C.

Consider the general reaction 5Br-(aq) + BrO3-(aq) + 6H+(aq)  3Br2(aq) + 3H2O(aq) For this reaction, the rate when expressed as [Br2]/t is the same as

Reaction intermediates differ from activated complexes in that

The half-life of a second-order reaction does not depend on the initial concentration of reactant.

Sulfuryl chloride, SO2Cl2(g), decomposes at high temperature to form SO2(g) and Cl2(g). The rate constant at a certain temperature is 4.68 × 10-5s-1. What is the order of the reaction?

The gas-phase reaction CH3NC  CH3CN has been studied in a closed vessel, and the rate equation was found to be: Rate = -[CH3NC]/t = k[CH3NC]. Which one of the following actions is least likely to cause a change in the rate of the reaction?

For each of the following terms/concepts, give a brief explanation or definition. Where possible, use examples. a. order of a reaction b. elementary reaction c. reaction intermediate

A first-order reaction has a half-life of 20.0 minutes. Starting with 1.00 × 1020 molecules of reactant at time t = 0, how many molecules remain unreacted after 100.0 minutes?

Tetrafluoroethylene, C2F4, can be converted to octafluorocyclobutane which can be used as a refrigerant or an aerosol propellant. A plot of 1/[C2F4] vs. time gives a straight line with a slope of 0.0448 L mol-1s-1. What is the rate law for this reaction?

A reaction has the following rate law: Rate = k[A][B]2 In experiment 1, the concentrations of A and B are both 0.10 mol L-1; in experiment 2, the concentrations are both 0.30 mol L-1. If the temperature stays constant, what is the value of the ratio, Rate(2)/Rate(1)?

An increase in temperature increases the reaction rate because

Chlorine atoms act as heterogeneous catalysts in the destruction of ozone in the stratosphere.

Dinitrogen tetraoxide, N2O4, decomposes to nitrogen dioxide, NO2, in a first-order process. If k = 2.5 × 103 s-1 at -5°C and k = 3.5 × 104 s-1 at 25°C, what is the activation energy for the decomposition?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 164.5°C to 179.0°C, the rate constantincreases by a factor of 4.27. What is the activation energy of this oxidation reaction?

Butadiene, C₄H₆ (used to make synthetic rubber and latex paints) reacts to C₈H₁₂ with a rate law of rate = 0.014 L/(mol·s) [C₄H₆]². What will be the concentration of C₄H₆after 3.0 hours if the initial concentration is 0.025 M?

The rate law for the rearrangement of CH₃NC to CH₃CN at 800 K is Rate = (1300 s^-1)[CH₃NC]. What is the half-life for this reaction?

The rate constant for the reaction 3A  4B is 6.00 × 10^-3 L mol^-1min^-1. How long will it take the concentration of A to drop from 0.75 M to 0.25 M?

At 25.0°C, a rate constant has the value 5.21 × 10^-8 L mol^-1 s^-1. If the activation energy is 75.2 kJ/mol, calculate the rate constant when the temperature is 50.0°C.

Consider the general reaction 5Br^-(aq) + BrO₃^-(aq) + 6H⁺(aq)  3Br₂(aq) + 3H₂O(aq) For this reaction, the rate when expressed as [Br₂]/t is the same as

Sulfuryl chloride, SO₂Cl₂(g), decomposes at high temperature to form SO₂(g) and Cl₂(g). The rate constant at a certain temperature is 4.68 × 10^-5s^-1. What is the order of the reaction?

The gas-phase reaction CH₃NC  CH₃CN has been studied in a closed vessel, and the rate equation was found to be: Rate = -[CH₃NC]/t = k[CH₃NC]. Which one of the following actions is least likely to cause a change in the rate of the reaction?

A first-order reaction has a half-life of 20.0 minutes. Starting with 1.00 × 10²⁰ molecules of reactant at time t = 0, how many molecules remain unreacted after 100.0 minutes?

Tetrafluoroethylene, C₂F₄, can be converted to octafluorocyclobutane which can be used as a refrigerant or an aerosol propellant. A plot of 1/[C₂F₄] vs. time gives a straight line with a slope of 0.0448 L mol^-1s^-1. What is the rate law for this reaction?

A reaction has the following rate law: Rate = k[A][B]² In experiment 1, the concentrations of A and B are both 0.10 mol L^-1; in experiment 2, the concentrations are both 0.30 mol L^-1. If the temperature stays constant, what is the value of the ratio, Rate(2)/Rate(1)?

Dinitrogen tetraoxide, N₂O₄, decomposes to nitrogen dioxide, NO₂, in a first-order process. If k = 2.5 × 10³s^-1 at -5°C and k = 3.5 × 10⁴ s^-1 at 25°C, what is the activation energy for the decomposition?