Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br- $\to$ HOBr + H2O (slow) HOBr + H+ + Br- $\to$ Br2 + H2O (fast) What is the overall reaction equation for this process?

A) 2H2O+-OH + 2Br- $\to$ H2O2 + Br2 + 2H2O B) 2H+ + 2Br- + H2O2 $\to$ Br2 + 2H2O C) 2H+ + H2O2 + Br- + HOBr $\to$ H2O+-OH + Br2 + H2O D) H2O+-OH + Br- + H+ $\to$ Br2 + H2O E) None of these choices is correct. A) 2H2O+-OH + 2Br- $\to$ H2O2 + Br2 + 2H2O B) 2H+ + 2Br- + H2O2 $\to$ Br2 + 2H2O C) 2H+ + H2O2 + Br- + HOBr $\to$ H2O+-OH + Br2 + H2O D) H2O+-OH + Br- + H+ $\to$ Br2 + H2O E) None of these choices is correct.

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

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br- $\to$ HOBr + H2O (slow) HOBr + H+ + Br- $\to$ Br2 + H2O (fast) Which of the following rate laws is consistent with the mechanism?

A) Rate = k[H2O2][H+]2[Br-] B) Rate = k [H2O+-OH][Br-] C) Rate = k[H2O2][H+][Br-] D) Rate = k[HOBr][H+][Br-][H2O2] E) Rate = k[Br-] A) Rate = k[H2O2][H+]2[Br-] B) Rate = k [H2O+-OH][Br-] C) Rate = k[H2O2][H+][Br-] D) Rate = k[HOBr][H+][Br-][H2O2] E) Rate = k[Br-]

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

A) -$\Delta$[H2O]/$\Delta$t B) 3$\Delta$[BrO3-]/$\Delta$t C) -5$\Delta$[Br-]/$\Delta$t D) -0.6$\Delta$[Br-]/$\Delta$t E) None of these choices is correct. A) -$\Delta$[H2O]/$\Delta$t B) 3$\Delta$[BrO3-]/$\Delta$t C) -5$\Delta$[Br-]/$\Delta$t D) -0.6$\Delta$[Br-]/$\Delta$t E) None of these choices is correct.

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H⁺ + H₂O₂ $Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br- \to HOBr + H2O (slow) HOBr + H+ + Br- \to Br2 + H2O (fast) What is the overall reaction equation for this process?$ H₂O⁺-OH (rapid equilibrium) H₂O⁺-OH + Br^- $\to$ HOBr + H₂O (slow) HOBr + H⁺ + Br^- $\to$ Br₂ + H₂O (fast) What is the overall reaction equation for this process?

(Multiple Choice)

4.8/5

(33)

Question 21

The units of the rate of reaction depend on the order of the reaction.

(True/False)

4.9/5

(34)

Question 22

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

(Multiple Choice)

4.8/5

(34)

Question 23

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

(Essay)

5.0/5

(33)

Question 24

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

(34)

Question 25

The compound RX₃ decomposes according to the equation 3RX₃ \(\to\0 R + R₂X₃ + 3X₂ In an experiment the following data were collected for the decomposition at 100°C.What is the average rate of reaction over the entire experiment? $The compound RX3 decomposes according to the equation 3RX3 \(\to\0 R + R2X3 + 3X2 In an experiment the following data were collected for the decomposition at 100°C.What is the average rate of reaction over the entire experiment?$

(Multiple Choice)

4.8/5

(26)

Question 26

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H⁺ + H₂O₂ $Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br- \to HOBr + H2O (slow) HOBr + H+ + Br- \to Br2 + H2O (fast) Which of the following rate laws is consistent with the mechanism?$ H₂O⁺-OH (rapid equilibrium) H₂O⁺-OH + Br^- $\to$ HOBr + H₂O (slow) HOBr + H⁺ + Br^- $\to$ Br₂ + H₂O (fast) Which of the following rate laws is consistent with the mechanism?

(Multiple Choice)

4.8/5

(37)

Question 27

When the reaction A $\to$ 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)

5.0/5

(39)

Question 28

The decomposition of dinitrogen pentaoxide to nitrogen dioxide and oxygen follows first-order kinetics and has an activation energy of 102 kJ/mol.By what factor will the fraction of collisions with energy greater than or equal to the activation energy increase if the reaction temperature goes from 30°C to 60°C?

(Multiple Choice)

4.8/5

(32)

Question 29

The rate constant for the reaction 3A $\to$ 4B is 6.00 $\times$ 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)

4.9/5

(46)

Question 30

The reaction A $\to$ B is first-order overall and first-order with respect to the reactant A.The result of doubling the initial concentration of A will be to

(Multiple Choice)

4.8/5

(38)

Question 31

A $\to$ B At very low pressures many such reactions occur by the following mechanism: $A \to B At very low pressures many such reactions occur by the following mechanism: (A* represents a molecule with sufficient energy to overcome the activation energy barrier. ) a.Which of the three reactions above is/are elementary? b.Where appropriate,identify the molecularity of the reactions. c.Show that the proposed mechanism is consistent with reaction 1,the observed reaction. d.Given the mechanism above,suggest a likely rate law for reaction (1).$ (A* represents a molecule with sufficient energy to overcome the activation energy barrier. ) a.Which of the three reactions above is/are elementary? b.Where appropriate,identify the molecularity of the reactions. c.Show that the proposed mechanism is consistent with reaction 1,the observed reaction. d.Given the mechanism above,suggest a likely rate law for reaction (1).

(Essay)

4.8/5

(31)

Question 32

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

(True/False)

4.8/5

(43)

Question 33

A chemical reaction of the general type A $\to$ 2B is first-order,with a rate constant of 1.52 $\times$ 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)

4.9/5

(33)

Question 34

A reactant R is being consumed in a first-order reaction.What fraction of the initial R is consumed in 4.0 half-lives?

(Multiple Choice)

4.7/5

(35)

Question 35

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

(Multiple Choice)

4.8/5

(40)

Question 36

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

(Multiple Choice)

4.8/5

(41)

Question 37

You are studying the rate of the reaction 2A $\to$ 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.

(Essay)

4.8/5

(37)

Question 38

Briefly list the features/properties common to all catalysts and how they work.Draw a labeled reaction energy diagram as part of your answer.

(Essay)

4.9/5

(28)

Question 39

The kinetics of the decomposition of dinitrogen pentaoxide is studied at 50°C and at 75°C.Which of the following statements concerning the studies is correct?

(Multiple Choice)

4.8/5

(43)

Question 40

Showing 21 - 40 of 76

The units of the rate of reaction depend on the order of the reaction.

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

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

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?

When the reaction A $\to$ 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?

The rate constant for the reaction 3A $\to$ 4B is 6.00 $\times$ 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?

The reaction A $\to$ B is first-order overall and first-order with respect to the reactant A.The result of doubling the initial concentration of A will be to

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

A chemical reaction of the general type A $\to$ 2B is first-order,with a rate constant of 1.52 $\times$ 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.

A reactant R is being consumed in a first-order reaction.What fraction of the initial R is consumed in 4.0 half-lives?

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

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

Briefly list the features/properties common to all catalysts and how they work.Draw a labeled reaction energy diagram as part of your answer.

The kinetics of the decomposition of dinitrogen pentaoxide is studied at 50°C and at 75°C.Which of the following statements concerning the studies is correct?

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

Filters

Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 H2O+-OH (rapid equilibrium) H2O+-OH + Br- →\to→ HOBr + H2O (slow) HOBr + H+ + Br- →\to→ Br2 + H2O (fast) What is the overall reaction equation for this process?

The units of the rate of reaction depend on the order of the reaction.

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

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

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 compound RX3 decomposes according to the equation 3RX3 \(\to\0 R + R2X3 + 3X2 In an experiment the following data were collected for the decomposition at 100°C.What is the average rate of reaction over the entire experiment?

When the reaction A →\to→ 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?

The rate constant for the reaction 3A →\to→ 4B is 6.00 ×\times× 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?

The reaction A →\to→ B is first-order overall and first-order with respect to the reactant A.The result of doubling the initial concentration of A will be to

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

A chemical reaction of the general type A →\to→ 2B is first-order,with a rate constant of 1.52 ×\times× 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.

A reactant R is being consumed in a first-order reaction.What fraction of the initial R is consumed in 4.0 half-lives?

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

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

Briefly list the features/properties common to all catalysts and how they work.Draw a labeled reaction energy diagram as part of your answer.

The kinetics of the decomposition of dinitrogen pentaoxide is studied at 50°C and at 75°C.Which of the following statements concerning the studies is correct?

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

Filters

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?

When the reaction A $\to$ 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?

The rate constant for the reaction 3A $\to$ 4B is 6.00 $\times$ 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?

The reaction A $\to$ B is first-order overall and first-order with respect to the reactant A.The result of doubling the initial concentration of A will be to

A chemical reaction of the general type A $\to$ 2B is first-order,with a rate constant of 1.52 $\times$ 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.

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