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°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 the above 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 the above

The rate law for the reaction 3A F1F1F1S1F1F1F10 2B is rate = k[A] with a rate constant of 0.0447 hr-1. What is the half-life of the reaction?

A) 0.0224 hr B) 0.0645 hr C) 15.5 hr D) 22.4 hr E) 44.7 hr A) 0.0224 hr B) 0.0645 hr C) 15.5 hr D) 22.4 hr E) 44.7 hr

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Sucrose decomposes to fructose and glucose in acid solution. When ln [sucrose] is plotted vs. time, a straight line with slope of -0.208 hr^-1 results. What is the rate law for the reaction?

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Question 1

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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.

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Question 2

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Rate constants k over a suitable range of absolute temperatures T. A plot of ln k versus 1/T should be linear, and its slope is - E_a/R.

Which of the following affects the activation energy of a reaction?

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Question 3

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

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Question 4

An elementary reaction is a simple, one-step process.

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Question 5

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?

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Question 6

In the gas phase at 500.°C, cyclopropane reacts to form propene in a first-order reaction. The figure shows the natural logarithm of the concentration of cyclopropane (in mol/L) plotted versus time. a. Explain how this plot confirms that the reaction is first order. b. Calculate the first-order rate constant, k. c. Determine the initial concentration of cyclopropane in this experiment.

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Question 7

For the reaction A(g) + 2B(g)  2C(g) + 2D(g) The following data were collected at constant temperature. Determine the correct rate law for this reaction.

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Question 8

A reaction has an activation energy of 195.0 kJ/mol. When the temperature is increased from 200.°C to 220.°C, the rate constant will increase by a factor of

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Question 9

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

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Question 10

The greater the energy of activation, E_a, the faster will be the reaction.

(True/False)

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Question 11

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°C, in s^-1?

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Question 12

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

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Question 13

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 H₂O₂to drop from 0.0200 M to 0.0120 M?

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Question 14

Carbon-14 is a radioactive isotope which decays with a half-life of 5730 years. What is the first-order rate constant for its decay, in units of years^-1?

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Question 15

The rate law for the reaction 3A  2B is rate = k[A] with a rate constant of 0.0447 hr^-1. What is the half-life of the reaction?

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Question 16

You are studying the rate of the reaction 2A  B and have obtained measurements of the concentration of A at times t = 100, 200, 300, ......, 1000 seconds from the start of the reaction. Carefully describe how you would plot a graph and use it to a. prove that the reaction is second-order with respect to A. b. determine the second-order rate constant k.

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Question 17

Is a bimolecular reaction necessarily second-order? Is a second-order reaction necessarily bimolecular? Answer, with explanations and clarifications.

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Question 18

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

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Question 19

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

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Question 20

Showing 1 - 20 of 88

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Sucrose decomposes to fructose and glucose in acid solution. When ln [sucrose] is plotted vs. time, a straight line with slope of -0.208 hr-1 results. What is the rate law for 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.

Which of the following affects the activation energy of a reaction?

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

An elementary reaction is a simple, one-step process.

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?

For the reaction A(g) + 2B(g)  2C(g) + 2D(g) The following data were collected at constant temperature. Determine the correct rate law for this reaction.

A reaction has an activation energy of 195.0 kJ/mol. When the temperature is increased from 200.°C to 220.°C, the rate constant will increase by a factor of

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

The greater the energy of activation, Ea, the faster will be the 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°C, in s-1?

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

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?

Carbon-14 is a radioactive isotope which decays with a half-life of 5730 years. What is the first-order rate constant for its decay, in units of years-1?

The rate law for the reaction 3A  2B is rate = k[A] with a rate constant of 0.0447 hr-1. What is the half-life of the reaction?

Is a bimolecular reaction necessarily second-order? Is a second-order reaction necessarily bimolecular? Answer, with explanations and clarifications.

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

The active ingredient in an over the counter pain killer analgesic decomposes with a rate constant, k = 9.05 × 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

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

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Sucrose decomposes to fructose and glucose in acid solution. When ln [sucrose] is plotted vs. time, a straight line with slope of -0.208 hr^-1 results. What is the rate law for 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.

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 greater the energy of activation, E_a, the faster will be the 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°C, in s^-1?

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 H₂O₂to drop from 0.0200 M to 0.0120 M?

Carbon-14 is a radioactive isotope which decays with a half-life of 5730 years. What is the first-order rate constant for its decay, in units of years^-1?

The rate law for the reaction 3A  2B is rate = k[A] with a rate constant of 0.0447 hr^-1. What is the half-life of the reaction?

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