The decomposition of hydrogen peroxide is a first-order process with a rate constant of 1.06 *10¯3 min¯1. How long will it take for the concentration of H2O2 to drop from 0.0200 M to 0.0120 M?

A) < 1 min B) 7.55 min C) 481 min D) 4550 min E) 31,400 min A) < 1 min B) 7.55 min C) 481 min D) 4550 min E) 31,400 min

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

A rate constant obeys the Arrhenius equation, the factor A being 2.2 *1013 s¯1 and the activation energy being 150. kJ mol¯1. What is the value of the rate constant at 227$\degree$C, in s¯1?

A) 2.1 *1013 s¯1 B) 6.7 * 10¯22 s¯1 C) 1.5 * 1011 s¯1 D) 4.7 *10¯3 s¯1 E) None of these choices is correct. A) 2.1 *1013 s¯1 B) 6.7 * 10¯22 s¯1 C) 1.5 * 1011 s¯1 D) 4.7 *10¯3 s¯1 E) None of these choices is correct.

Cyclopropane is converted to propene in a first-order process. The rate constant is 5.4 * 10¯2 hr¯1. If the initial concentration of cyclopropane is 0.150 M, what will its concentration be after 22.0 hours?

A) 0.0457 M B) 0.105 M C) 0.127 M D) 0.492 M E) None of these choices is correct. A) 0.0457 M B) 0.105 M C) 0.127 M D) 0.492 M E) None of these choices is correct.

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 *¯4 mol L¯1 and the rate constant k = 1.08 *10¯6 s¯1, what concentration of R remains after 25 days?

A) 1.0 * 10¯3 mol L¯1 B) 1.0 *10¯4 mol L¯1 C) 9.6 * 10¯5 mol L¯1 D) 4.3 * 10¯5 mol L¯1 E) 9.7 *10¯6 mol L¯1 A) 1.0 * 10¯3 mol L¯1 B) 1.0 *10¯4 mol L¯1 C) 9.6 * 10¯5 mol L¯1 D) 4.3 * 10¯5 mol L¯1 E) 9.7 *10¯6 mol L¯1

The active ingredient in an over-the-counter pain killer analgesic decomposes with a rate constant, k = 9.05 x 10¯4 day¯1. How many days does it take for 15% of the original ingredient to decompose?

A) 730 days B) 414 days C) 365 days D) 180 days E) 78 days A) 730 days B) 414 days C) 365 days D) 180 days E) 78 days

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

The decomposition of hydrogen peroxide is a first-order process with a rate constant of 1.06 *10¯³ min¯¹. How long will it take for the concentration of H₂O₂ to drop from 0.0200 M to 0.0120 M?

(Multiple Choice)

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Question 41

A catalyst lowers the activation energy but does not affect the mechanism of a reaction.

(True/False)

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Question 42

The rate law cannot be predicted from the stoichiometry of a reaction.

(True/False)

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Question 43

Which one of the following sets of units is appropriate for a third-order rate constant?

(Multiple Choice)

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Question 44

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?

(Multiple Choice)

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Question 45

In the lock and key model of enzyme action, the active site on the enzyme provides an exact fit for the substrate.

(True/False)

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Question 46

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

(Multiple Choice)

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Question 47

A rate constant obeys the Arrhenius equation, the factor A being 2.2 *10¹³ s¯¹ and the activation energy being 150. kJ mol¯¹. What is the value of the rate constant at 227 $\degree$ C, in s¯¹?

(Multiple Choice)

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Question 48

All bimolecular reactions are second-order reactions.

(True/False)

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Question 49

Cyclopropane is converted to propene in a first-order process. The rate constant is 5.4 * 10¯² hr¯¹. If the initial concentration of cyclopropane is 0.150 M, what will its concentration be after 22.0 hours?

(Multiple Choice)

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Question 50

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

(True/False)

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Question 51

A chemical reaction of the general type A $\rightarrow$ 2B is first-order, with a rate constant of 1.52 *10¯⁴ s¯¹. A) Calculate the half-life of A. B) Assuming the initial concentration of A is 0.067 mol L¯¹, calculate the time needed for the concentration to fall to 0.010 mol L¯¹.

(Essay)

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Question 52

Which of the following sets of units could be appropriate for a zero-order rate constant?

(Multiple Choice)

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Question 53

The reaction CH₃NC(g) $\rightarrow$ CH₃CN(g) is first-order with respect to methyl isocyanide, CH₃NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min¯¹?

(Multiple Choice)

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Question 54

A reaction intermediate is a species corresponding to a local energy maximum on a reaction energy diagram.

(True/False)

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Question 55

What is the molecularity of the following elementary reaction?

(Multiple Choice)

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Question 56

When the reaction A $\rightarrow$ B + C is studied, a plot 1/[A]_t vs. time gives a straight line with a positive slope. What is the order of the reaction?

(Multiple Choice)

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Question 57

You are required to determine the energy of activation (E_a) of a reaction. Briefly describe the experimental measurements you would make and how you would obtain the activation energy from a suitable linear plot of the experimental data.

(Essay)

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Question 58

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 ¯⁴ mol L¯¹ and the rate constant k = 1.08 10¯⁶ s¯¹, what concentration of R remains after 25 days?

(Multiple Choice)

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Question 59

The active ingredient in an over-the-counter pain killer analgesic decomposes with a rate constant, k = 9.05 x 10¯⁴ day¯¹. How many days does it take for 15% of the original ingredient to decompose?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 89

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

The decomposition of hydrogen peroxide is a first-order process with a rate constant of 1.06 *10¯3 min¯1. How long will it take for the concentration of H2O2 to drop from 0.0200 M to 0.0120 M?

A catalyst lowers the activation energy but does not affect the mechanism of a reaction.

The rate law cannot be predicted from the stoichiometry of a reaction.

Which one of the following sets of units is appropriate for a third-order rate constant?

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?

In the lock and key model of enzyme action, the active site on the enzyme provides an exact fit for the substrate.

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

A rate constant obeys the Arrhenius equation, the factor A being 2.2 *1013 s¯1 and the activation energy being 150. kJ mol¯1. What is the value of the rate constant at 227 °\degree° C, in s¯1?

All bimolecular reactions are second-order reactions.

Cyclopropane is converted to propene in a first-order process. The rate constant is 5.4 * 10¯2 hr¯1. If the initial concentration of cyclopropane is 0.150 M, what will its concentration be after 22.0 hours?

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

A chemical reaction of the general type A →\rightarrow→ 2B is first-order, with a rate constant of 1.52 *10¯4 s¯1. A) Calculate the half-life of A. B) Assuming the initial concentration of A is 0.067 mol L¯1, calculate the time needed for the concentration to fall to 0.010 mol L¯1.

Which of the following sets of units could be appropriate for a zero-order rate constant?

The reaction CH3NC(g) →\rightarrow→ CH3CN(g) is first-order with respect to methyl isocyanide, CH3NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min¯1?

A reaction intermediate is a species corresponding to a local energy maximum on a reaction energy diagram.

What is the molecularity of the following elementary reaction?

When the reaction A →\rightarrow→ B + C is studied, a plot 1/[A]t vs. time gives a straight line with a positive slope. What is the order of the reaction?

You are required to determine the energy of activation (Ea) of a reaction. Briefly describe the experimental measurements you would make and how you would obtain the activation energy from a suitable linear plot of the experimental data.

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 *¯4 mol L¯1 and the rate constant k = 1.08 *10¯6 s¯1, what concentration of R remains after 25 days?

The active ingredient in an over-the-counter pain killer analgesic decomposes with a rate constant, k = 9.05 x 10¯4 day¯1. How many days does it take for 15% of the original ingredient to decompose?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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

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The decomposition of hydrogen peroxide is a first-order process with a rate constant of 1.06 *10¯³ min¯¹. How long will it take for the concentration of H₂O₂ to drop from 0.0200 M to 0.0120 M?

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?

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

A rate constant obeys the Arrhenius equation, the factor A being 2.2 *10¹³ s¯¹ and the activation energy being 150. kJ mol¯¹. What is the value of the rate constant at 227 $\degree$ C, in s¯¹?

Cyclopropane is converted to propene in a first-order process. The rate constant is 5.4 * 10¯² hr¯¹. If the initial concentration of cyclopropane is 0.150 M, what will its concentration be after 22.0 hours?

A chemical reaction of the general type A $\rightarrow$ 2B is first-order, with a rate constant of 1.52 *10¯⁴ s¯¹. A) Calculate the half-life of A. B) Assuming the initial concentration of A is 0.067 mol L¯¹, calculate the time needed for the concentration to fall to 0.010 mol L¯¹.

The reaction CH₃NC(g) $\rightarrow$ CH₃CN(g) is first-order with respect to methyl isocyanide, CH₃NC. If it takes 10.3 minutes for exactly one quarter of the initial amount of methyl isocyanide to react, what is the rate constant in units of min¯¹?

When the reaction A $\rightarrow$ B + C is studied, a plot 1/[A]_t vs. time gives a straight line with a positive slope. What is the order of the reaction?

You are required to determine the energy of activation (E_a) of a reaction. Briefly describe the experimental measurements you would make and how you would obtain the activation energy from a suitable linear plot of the experimental data.

A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 ¯⁴ mol L¯¹ and the rate constant k = 1.08 10¯⁶ s¯¹, what concentration of R remains after 25 days?

The active ingredient in an over-the-counter pain killer analgesic decomposes with a rate constant, k = 9.05 x 10¯⁴ day¯¹. How many days does it take for 15% of the original ingredient to decompose?