A rate constant obeys the Arrhenius equation,the factor A being 2.2 $\times$ 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 $\times$ 1013 s-1 B) 6.7 $\times$ 10-22 s-1 C) 1.5 $\times$ 1011 s-1 D) 4.7 $\times$ 10-3 s-1 E) None of these choices is correct. A) 2.1 $\times$ 1013 s-1 B) 6.7 $\times$ 10-22 s-1 C) 1.5 $\times$ 1011 s-1 D) 4.7 $\times$ 10-3 s-1 E) None of these choices is correct. D

The gas-phase reaction CH3NC $\to$ CH3CN has been studied in a closed vessel,and the rate equation was found to be: rate = -$\Delta$[CH3NC]/$\Delta$t = 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 E

What is the molecularity of the following elementary reaction? NH2Cl(aq)+ OH-(aq) $\to$NHCl-(aq)+ H2O(l)

A) unimolecular B) bimolecular C) termolecular D) tetramolecular E) The reaction order must be known before molecularity can be determined. A) unimolecular B) bimolecular C) termolecular D) tetramolecular E) The reaction order must be known before molecularity can be determined. B

Butadiene,C4H6 (used to make synthetic rubber and latex paints)dimerizes 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

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

A rate constant obeys the Arrhenius equation,the factor A being 2.2 $\times$ 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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(Multiple Choice)

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Question 1

Correct Answer:

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

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Question 2

Correct Answer:

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What is the molecularity of the following elementary reaction? NH₂Cl(aq)+ OH^-(aq) $\to$ NHCl^-(aq)+ H₂O(l)

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Question 3

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

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Question 4

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)?

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Question 5

Cyclobutane decomposes to ethene in a first-order reaction.From measurements of the rate constant (k)at various absolute temperatures (T),the accompanying Arrhenius plot was obtained (ln k versus 1/T). a.Calculate the energy of activation,E_a. b.Determine the value of the rate constant at 740.K.(In the plot,the units of k are s^-1. )

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Question 6

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

(True/False)

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Question 7

Reaction intermediates differ from activated complexes in that

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Question 8

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 9

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 10

Butadiene,C₄H₆ (used to make synthetic rubber and latex paints)dimerizes 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?

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Question 11

If the activation energy of a reaction decreases by 10.0 kJ/mol,from 100.0 to 90.0 kJ/mol,what effect will this have on the rate of reaction at 298K?

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Question 12

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

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Question 13

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

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Question 14

According to the collision theory of reaction rates,what are the three requirements which must be met before an elementary reaction between two molecules can occur?

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Question 15

At 25.0°C,a rate constant has the value 5.21 $\times$ 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.

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Question 16

All bimolecular reactions are second-order reactions.

(True/False)

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Question 17

In the collision theory of reaction rates,the rate constant for a bimolecular reaction can be written as k = z·p·exp(-E_a/RT) In one sentence each,clearly explain the physical meaning (interpretation)of the following three factors which appear in the above expression: a.z b.p c.exp(-E_a/RT)

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Question 18

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 19

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

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Question 20

Showing 1 - 20 of 76

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

A rate constant obeys the Arrhenius equation,the factor A being 2.2 ×\times× 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 gas-phase reaction CH3NC →\to→ CH3CN has been studied in a closed vessel,and the rate equation was found to be: rate = - Δ\DeltaΔ [CH3NC]/ Δ\DeltaΔ t = k[CH3NC].Which one of the following actions is least likely to cause a change in the rate of the reaction?

What is the molecularity of the following elementary reaction? NH2Cl(aq)+ OH-(aq) →\to→ NHCl-(aq)+ H2O(l)

For the reaction A(g)+ 2B(g) →\to→ 2C(g)+ 2D(g) The following data was collected at constant temperature.Determine the correct 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)?

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

Reaction intermediates differ from activated complexes in that

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?

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.

Butadiene,C4H6 (used to make synthetic rubber and latex paints)dimerizes 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?

If the activation energy of a reaction decreases by 10.0 kJ/mol,from 100.0 to 90.0 kJ/mol,what effect will this have on the rate of reaction at 298K?

Which of the following affects the activation energy of a 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

According to the collision theory of reaction rates,what are the three requirements which must be met before an elementary reaction between two molecules can occur?

At 25.0°C,a rate constant has the value 5.21 ×\times× 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.

All bimolecular reactions are second-order reactions.

In the collision theory of reaction rates,the rate constant for a bimolecular reaction can be written as k = z·p·exp(-Ea/RT) In one sentence each,clearly explain the physical meaning (interpretation)of the following three factors which appear in the above expression: a.z b.p c.exp(-Ea/RT)

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?

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

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 Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

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 Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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A rate constant obeys the Arrhenius equation,the factor A being 2.2 $\times$ 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 gas-phase reaction CH₃NC $\to$ CH₃CN has been studied in a closed vessel,and the rate equation was found to be: rate = - $\Delta$ [CH₃NC]/ $\Delta$ t = k[CH₃NC].Which one of the following actions is least likely to cause a change in the rate of the reaction?

What is the molecularity of the following elementary reaction? NH₂Cl(aq)+ OH^-(aq) $\to$ NHCl^-(aq)+ H₂O(l)

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)?

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?

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.

Butadiene,C₄H₆ (used to make synthetic rubber and latex paints)dimerizes 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?

At 25.0°C,a rate constant has the value 5.21 $\times$ 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.

In the collision theory of reaction rates,the rate constant for a bimolecular reaction can be written as k = z·p·exp(-E_a/RT) In one sentence each,clearly explain the physical meaning (interpretation)of the following three factors which appear in the above expression: a.z b.p c.exp(-E_a/RT)

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?

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