Consider the reaction 2A + 2B + C → 2D + E If the rate law for this reaction is Rate = k[A][B]2, what will be the effect on the rate if the concentrations of A, B and C are all doubled at the same time?

A) The rate will increase by a factor of 2. B) The rate will increase by a factor of 4. C) The rate will increase by a factor of 6. D) The rate will increase by a factor of 8. E) More information is needed before this question can be answered. A) The rate will increase by a factor of 2. B) The rate will increase by a factor of 4. C) The rate will increase by a factor of 6. D) The rate will increase by a factor of 8. E) More information is needed before this question can be answered. D

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

A) -Δ[H2O]/Δt B) 3Δ[BrO3-]/Δt C) -5Δ[Br-]/Δt D) -0.6Δ[Br-]/Δt E) None of these choices are correct. A) -Δ[H2O]/Δt B) 3Δ[BrO3-]/Δt C) -5Δ[Br-]/Δt D) -0.6Δ[Br-]/Δt E) None of these choices are correct. D

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

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

A) Unimolecular B) Bimolecular C) Termolecular D) Tetramolecular E) Need to know the reaction order before molecularity can be determined. A) Unimolecular B) Bimolecular C) Termolecular D) Tetramolecular E) Need to know the reaction order before molecularity can be determined.

Ammonium cyanate (NH4CNO) reacts to form urea (NH2CONH2). At 65°C the rate constant, k, is 3.60 L mol-1s-1.What is the rate law for this reaction?

A) Rate = 3.60 L mol-1s-1[NH4CNO] B) Rate = 3.60 L mol-1s-1 [NH4CNO]2 C) Rate = 0.28 mol L-1s-1 [NH4CNO] D) Rate = 0.28 mol L-1s-1[NH4CNO]2 E) Rate = 3.60 L mol-1s-1 [NH2CONH2]-1 A) Rate = 3.60 L mol-1s-1[NH4CNO] B) Rate = 3.60 L mol-1s-1 [NH4CNO]2 C) Rate = 0.28 mol L-1s-1 [NH4CNO] D) Rate = 0.28 mol L-1s-1[NH4CNO]2 E) Rate = 3.60 L mol-1s-1 [NH2CONH2]-1

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- → HOBr + H2O (slow) HOBr + H+ + Br- → Br2 + H2O (fast) What is the overall reaction equation for this process?

A) 2H2O+-OH + 2Br- → H2O2 + Br2 + 2H2O B) 2H+ + 2Br- + H2O2 → Br2 + 2H2O C) 2H+ + H2O2 + Br- + HOBr → H2O+-OH + Br2 + H2O D) H2O+-OH + Br- + H+ → Br2 + H2O E) None of these choices are correct. A) 2H2O+-OH + 2Br- → H2O2 + Br2 + 2H2O B) 2H+ + 2Br- + H2O2 → Br2 + 2H2O C) 2H+ + H2O2 + Br- + HOBr → H2O+-OH + Br2 + H2O D) H2O+-OH + Br- + H+ → Br2 + H2O E) None of these choices are correct.

Sulfur trioxide can undergo decomposition according to the equation 2SO3 → 2SO2 + O2 For this reaction, rate = -0.5Δ[SO3 ]/Δt = k[SO3]2. If the reaction rate is 1.75 × 10-7 mol L-1 min-1 when the concentration of sulfur trioxide is 5.4 × 10-3 mol L-1, what is the value of the rate constant k?

A) 3.2 × 10-5 L mol-1 min-1 B) 1.6 × 10-5 L mol-1 min-1 C) 6.0 × 10-3 L mol-1 min-1 D) 3.0 × 10-3 L mol-1 min-1 E) 1.6 × 10-2 L mol-1 min-1 A) 3.2 × 10-5 L mol-1 min-1 B) 1.6 × 10-5 L mol-1 min-1 C) 6.0 × 10-3 L mol-1 min-1 D) 3.0 × 10-3 L mol-1 min-1 E) 1.6 × 10-2 L mol-1 min-1

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- → HOBr + H2O (slow) HOBr + H+ + Br- → 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-]

Exam 16: Kinetics Rates and Mechanisms of Chemical Reactions

Consider the reaction 2A + 2B + C → 2D + E If the rate law for this reaction is Rate = k[A][B]², what will be the effect on the rate if the concentrations of A, B and C are all doubled at the same time?

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(Multiple Choice)

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Question 1

Correct Answer:

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

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and ΔH°_rxn = + 55 kJ/mol. What is the activation energy for the reverse reaction?

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

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 4

What is the molecularity of the following elementary reaction? NH₂Cl(aq) + OH_- (aq) → NHCl_- (aq) + H₂O(l)

(Multiple Choice)

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Question 5

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

(True/False)

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Question 6

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)

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Question 7

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

(True/False)

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Question 8

Ammonium cyanate (NH₄CNO) reacts to form urea (NH₂CONH₂). At 65°C the rate constant, k, is 3.60 L mol^-1s^-1.What is the rate law for this reaction?

(Multiple Choice)

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Question 9

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

(True/False)

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Question 10

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)

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Question 11

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^- → HOBr + H₂O (slow) HOBr + H⁺ + Br^- → Br₂ + H₂O (fast) What is the overall reaction equation for this process?

(Multiple Choice)

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Question 12

Sulfur trioxide can undergo decomposition according to the equation 2SO₃ → 2SO₂ + O₂ For this reaction, rate = -0.5Δ[SO₃ ]/Δt = k[SO₃]². If the reaction rate is 1.75 × 10^-7 mol L^-1 min^-1 when the concentration of sulfur trioxide is 5.4 × 10^-3 mol L^-1, what is the value of the rate constant k?

(Multiple Choice)

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Question 13

2NOBr(g) → 2NO(g) + Br₂(g) [NOBr](mol L^-1) Rate (molL^-1s^-1) 0)0450 1.62 × 10^-3 0)0310 7.69 × 10^-4 0)0095 7.22 × 10^-5 Based on the initial rate data above, what is the value of the rate constant?

(Multiple Choice)

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Question 14

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

(Multiple Choice)

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Question 15

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. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L·min)) 1 0)125 0.200 7.25 2 0)375 0.200 21.75 3 0)250 0.400 14.50 4 0)375 0.400 21.75

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Question 16

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

(True/False)

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Question 17

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^- → HOBr + H₂O (slow) HOBr + H⁺ + Br^- → Br₂ + H₂O (fast) Which of the following rate laws is consistent with the mechanism?

(Multiple Choice)

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Question 18

When the reaction A → B + C is studied, a plot of ln[A]_t vs. time gives a straight line with a negative slope. What is the order of the reaction?

(Multiple Choice)

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Question 19

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?

(Multiple Choice)

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Question 20

Showing 1 - 20 of 78

Consider the reaction 2A + 2B + C → 2D + E If the rate law for this reaction is Rate = k[A][B]², what will be the effect on the rate if the concentrations of A, B and C are all doubled at the same time?

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

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and ΔH°_rxn = + 55 kJ/mol. What is the activation energy for the reverse 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?

What is the molecularity of the following elementary reaction? NH₂Cl(aq) + OH_- (aq) → NHCl_- (aq) + H₂O(l)

The units of the rate of reaction depend on the order of the 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)?

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

Ammonium cyanate (NH₄CNO) reacts to form urea (NH₂CONH₂). At 65°C the rate constant, k, is 3.60 L mol^-1s^-1.What is the rate law for this reaction?

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

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

2NOBr(g) → 2NO(g) + Br₂(g) [NOBr](mol L^-1) Rate (molL^-1s^-1) 0)0450 1.62 × 10^-3 0)0310 7.69 × 10^-4 0)0095 7.22 × 10^-5 Based on the initial rate data above, what is the value of the rate constant?

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

When the reaction A → B + C is studied, a plot of ln[A]_t vs. time gives a straight line with a negative slope. What is the order of the reaction?

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?

Keys to Studying Chemistry Definitions, Units, and Problem Solving

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 16: Kinetics Rates and Mechanisms of Chemical Reactions

Consider the reaction 2A + 2B + C → 2D + E If the rate law for this reaction is Rate = k[A][B]2, what will be the effect on the rate if the concentrations of A, B and C are all doubled at the same time?

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

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and ΔH°rxn = + 55 kJ/mol. What is the activation energy for the reverse 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?

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

The units of the rate of reaction depend on the order of the 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)?

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

Ammonium cyanate (NH4CNO) reacts to form urea (NH2CONH2). At 65°C the rate constant, k, is 3.60 L mol-1s-1.What is the rate law for this reaction?

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

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

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- → HOBr + H2O (slow) HOBr + H+ + Br- → Br2 + H2O (fast) What is the overall reaction equation for this process?

Sulfur trioxide can undergo decomposition according to the equation 2SO3 → 2SO2 + O2 For this reaction, rate = -0.5Δ[SO3 ]/Δt = k[SO3]2. If the reaction rate is 1.75 × 10-7 mol L-1 min-1 when the concentration of sulfur trioxide is 5.4 × 10-3 mol L-1, what is the value of the rate constant k?

2NOBr(g) → 2NO(g) + Br2(g) [NOBr](mol L-1) Rate (molL-1s-1) 0)0450 1.62 × 10-3 0)0310 7.69 × 10-4 0)0095 7.22 × 10-5 Based on the initial rate data above, what is the value of the rate constant?

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

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- → HOBr + H2O (slow) HOBr + H+ + Br- → Br2 + H2O (fast) Which of the following rate laws is consistent with the mechanism?

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

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?

Keys to Studying Chemistry Definitions, Units, and Problem Solving

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Consider the reaction 2A + 2B + C → 2D + E If the rate law for this reaction is Rate = k[A][B]², what will be the effect on the rate if the concentrations of A, B and C are all doubled at the same time?

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

The decomposition of dinitrogen pentaoxide has an activation energy of 102 kJ/mol and ΔH°_rxn = + 55 kJ/mol. What is the activation energy for the reverse 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?

What is the molecularity of the following elementary reaction? NH₂Cl(aq) + OH_- (aq) → 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)?

Ammonium cyanate (NH₄CNO) reacts to form urea (NH₂CONH₂). At 65°C the rate constant, k, is 3.60 L mol^-1s^-1.What is the rate law for this reaction?

2NOBr(g) → 2NO(g) + Br₂(g) [NOBr](mol L^-1) Rate (molL^-1s^-1) 0)0450 1.62 × 10^-3 0)0310 7.69 × 10^-4 0)0095 7.22 × 10^-5 Based on the initial rate data above, what is the value of the rate constant?

When the reaction A → B + C is studied, a plot of ln[A]_t vs. time gives a straight line with a negative slope. What is the order of the reaction?

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?