The rate law for the chemical reaction 5Br-(aq)+ BrO3-(aq)+ 6H+(aq)→ 3Br2(aq)+ 3H2O(l) Has been determined experimentally to be Rate = k[Br-][BrO3-][H+]2.What is the overall order of the reaction?

A) 3 B) 5 C) 4 D) 2 E) 1 A) 3 B) 5 C) 4 D) 2 E) 1

The reaction 3NO → N2O + NO2 is found to obey the rate law Rate = k[NO]2.If the first half-life of the reaction is found to be 2.0 s,what is the length of the fourth half-life?

A) 4.0 s B) 8.0 s C) 2.0 s D) 16.0 s E) 12.0 s A) 4.0 s B) 8.0 s C) 2.0 s D) 16.0 s E) 12.0 s

For the reaction IO3-(aq)+ 5I-(aq)+ 6H+(aq)→ 3I2(aq)+ 3H2O(l) The rate of disappearance of I O3-(aq)at a particular time and concentration is 2.5× 10-3 mol/(L · s).What is the rate of appearance of I2(aq)?

A) 8.3 × 10-3 mol/(L ∙ s) B) 3 × 10-3 mol/(L ∙ s) C) -8 × 10-3 mol/(L ∙ s) D) 8 × 10-3 mol/(L ∙ s) E) 1 × 10-3 mol/(L ∙ s) A) 8.3 × 10-3 mol/(L ∙ s) B) 3 × 10-3 mol/(L ∙ s) C) -8 × 10-3 mol/(L ∙ s) D) 8 × 10-3 mol/(L ∙ s) E) 1 × 10-3 mol/(L ∙ s)

For the reaction (CH3)3CCl(aq)+ OH-(aq)→ (CH3)3COH(aq)+ Cl-(aq) It is found experimentally that doubling the initial concentration of (CH3)3CCl causes the initial reaction rate to double,but doubling the initial concentration of OH- has no effect on the rate.What is the rate law?

A) Rate = k[(CH3)3CCl]2[OH-] B) Rate = k[(CH3)3CCl][OH-] C) Rate = k D) Rate = k[(CH3)3COH][Cl-] E) Rate = k[(CH3)3CCl] A) Rate = k[(CH3)3CCl]2[OH-] B) Rate = k[(CH3)3CCl][OH-] C) Rate = k D) Rate = k[(CH3)3COH][Cl-] E) Rate = k[(CH3)3CCl]

The OH· radical disproportionates according to the elementary chemical reaction This reaction is second-order in OH·.The rate constant for the reaction is 2.0 × 10-12 cm3/molecules at room temperature.If the initial OH· concentration is 1.4 × 1013 molecules/cm3,what is the first half-life for the reaction?

A) 2.8 × 101 s B) 3.6 × 10-2 s C) 1.8 × 10-2 s D) 3.5 × 1011 s E) 7.1 × 10-14 s A) 2.8 × 101 s B) 3.6 × 10-2 s C) 1.8 × 10-2 s D) 3.5 × 1011 s E) 7.1 × 10-14 s

Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according to the following chemical equation: O3(g)+ 2NO2(g)→ O2(g)+ N2O5(g) The rate law for this reaction is Rate = k[O3][NO2].If concentration is measured in moles per liter and time is measured in seconds,what are the units of k?

A) L ∙ mol-1 ∙ s B) L2 ∙ mol-2 ∙ s-1 C) L ∙ mol-1 ∙ s-1 D) mol ∙ L-1 ∙ s-1 E) mol2 ∙ L-2 ∙ s-1 A) L ∙ mol-1 ∙ s B) L2 ∙ mol-2 ∙ s-1 C) L ∙ mol-1 ∙ s-1 D) mol ∙ L-1 ∙ s-1 E) mol2 ∙ L-2 ∙ s-1

Exam 13: Rates of Reaction

The rate law for the chemical reaction 5Br^-(aq)+ BrO₃^-(aq)+ 6H⁺(aq)→ 3Br₂(aq)+ 3H₂O(l) Has been determined experimentally to be Rate = k[Br^-][BrO₃^-][H⁺]².What is the overall order of the reaction?

(Multiple Choice)

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Question 61

The reaction 3NO → N₂O + NO₂ is found to obey the rate law Rate = k[NO]².If the first half-life of the reaction is found to be 2.0 s,what is the length of the fourth half-life?

(Multiple Choice)

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Question 62

The acid-catalyzed reaction of acetone,CH₃COCH₃,with iodine can be represented by the following net reaction: CH₃COCH₃ + I₂ CH₂ICOCH₃ + H⁺ + I^- It is found experimentally that the rate law for this reaction is Rate = k[CH₃COCH₃][H⁺].Suppose that in trial 1,the initial rate of the reaction is measured with the initial concentrations of acetone,iodine,and hydrogen ion all equal to 0.10 M.Then,in trial 2,the initial rate of the reaction is measured with the initial concentrations all equal to 0.20 M.The initial rate of trial 2 will be larger than the initial rate of trial 1 by a factor of

(Multiple Choice)

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Question 63

When the concentrations of the reactants are increased,the rate of the reaction increases.This is best explained by

(Multiple Choice)

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Question 64

For the reaction IO₃^-(aq)+ 5I^-(aq)+ 6H⁺(aq)→ 3I₂(aq)+ 3H₂O(l) The rate of disappearance of I O₃^-(aq)at a particular time and concentration is 2.5× 10^-3 mol/(L · s).What is the rate of appearance of I₂(aq)?

(Multiple Choice)

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Question 65

Which of the following reactions is not an example of homogeneous catalysis?

(Multiple Choice)

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Question 66

In a first-order reaction,the half-life is 139 minutes.What is the rate constant?

(Multiple Choice)

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Question 67

The rate constant for a first-order reaction is 1.5× 10^-2 s^-1 at 710 K and 4.1 × 10^-2 s^-1 at 884 K.What is the activation energy? (R = 8.31 J/(mol · K))

(Multiple Choice)

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Question 68

For the reaction (CH₃)₃CCl(aq)+ OH^-(aq)→ (CH₃)₃COH(aq)+ Cl^-(aq) It is found experimentally that doubling the initial concentration of (CH₃)₃CCl causes the initial reaction rate to double,but doubling the initial concentration of OH^- has no effect on the rate.What is the rate law?

(Multiple Choice)

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Question 69

For the reaction 2N₂O₅(g)→ 4NO₂(g)+ O₂(g) Which of the following expressions is equal to the rate of the reaction?

(Multiple Choice)

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Question 70

For which order reaction is the half-life of the reaction proportional to 1/k (k is the rate constant)?

(Multiple Choice)

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Question 71

Which of the following experimental methods cannot be used to measure the rate of a reaction?

(Multiple Choice)

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Question 72

The OH· radical disproportionates according to the elementary chemical reaction This reaction is second-order in OH·.The rate constant for the reaction is 2.0 × 10^-12 cm³/molecules at room temperature.If the initial OH· concentration is 1.4 × 10¹³ molecules/cm³,what is the first half-life for the reaction?

(Multiple Choice)

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Question 73

Which of the following statements best describes the condition(s)needed for a successful formation for a product according to the collision model?

(Multiple Choice)

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Question 74

The reaction between selenous acid and the iodide ion in acid solution is H₂SeO₃(aq)+ 6I^-(aq)+ 4H⁺(aq)→ Se(s)+ 2I₃^-(aq)+ 3H₂O(l) The data in the following table were measured at 0°C. Experiment [H₂SeO₃]₀ (M) [H⁺]₀ (M) [I^-]₀ (M) Initial Rate [mol/(L ∙ s)] 1 1)00 × 10^-4 2)00 × 10^-2 3)00 × 10^-2 5)30 × 10^-7 2 2)00 × 10^-4 2)00 × 10^-2 3)00 × 10^-2 1)06 × 10^-6 3 3)00 × 10^-4 4)00 × 10^-2 3)00 × 10^-2 6)36 × 10^-6 4 3)00 × 10^-4 8)00 × 10^-2 3)00 × 10^-2 2)54 × 10^-5 5 3)00 × 10^-4 8)00 × 10^-2 6)00 × 10^-2 2)04 × 10^-4 6 2)00 × 10^-4 2)00 × 10^-2 6)00 × 10^-2 8)48 × 10^-6 What is the rate constant for this reaction?

(Multiple Choice)

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Question 75

For which of the following hypothetical rate laws would the units of the rate constant have the general form M^-3·time−1?

(Multiple Choice)

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Question 76

Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according to the following chemical equation: O₃(g)+ 2NO₂(g)→ O₂(g)+ N₂O₅(g) The rate law for this reaction is Rate = k[O₃][NO₂].If concentration is measured in moles per liter and time is measured in seconds,what are the units of k?

(Multiple Choice)

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Question 77

If a reaction is first-order with respect to a particular reactant,when the concentration of that reactant is increased by a factor of 2,the reaction rate will _____.

(Multiple Choice)

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Question 78

For the hypothetical reaction aA → products,the concentration of A was monitored with time.Given the following graph of the experimental data,what is the rate constant for the loss of reactant A?

(Multiple Choice)

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Question 79

The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system.The increase in rate as the temperature increases is best explained by

(Multiple Choice)

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Question 80

Showing 61 - 80 of 113

The rate law for the chemical reaction 5Br^-(aq)+ BrO₃^-(aq)+ 6H⁺(aq)→ 3Br₂(aq)+ 3H₂O(l) Has been determined experimentally to be Rate = k[Br^-][BrO₃^-][H⁺]².What is the overall order of the reaction?

The reaction 3NO → N₂O + NO₂ is found to obey the rate law Rate = k[NO]².If the first half-life of the reaction is found to be 2.0 s,what is the length of the fourth half-life?

When the concentrations of the reactants are increased,the rate of the reaction increases.This is best explained by

For the reaction IO₃^-(aq)+ 5I^-(aq)+ 6H⁺(aq)→ 3I₂(aq)+ 3H₂O(l) The rate of disappearance of I O₃^-(aq)at a particular time and concentration is 2.5× 10^-3 mol/(L · s).What is the rate of appearance of I₂(aq)?

Which of the following reactions is not an example of homogeneous catalysis?

In a first-order reaction,the half-life is 139 minutes.What is the rate constant?

The rate constant for a first-order reaction is 1.5× 10^-2 s^-1 at 710 K and 4.1 × 10^-2 s^-1 at 884 K.What is the activation energy? (R = 8.31 J/(mol · K))

For the reaction (CH₃)₃CCl(aq)+ OH^-(aq)→ (CH₃)₃COH(aq)+ Cl^-(aq) It is found experimentally that doubling the initial concentration of (CH₃)₃CCl causes the initial reaction rate to double,but doubling the initial concentration of OH^- has no effect on the rate.What is the rate law?

For the reaction 2N₂O₅(g)→ 4NO₂(g)+ O₂(g) Which of the following expressions is equal to the rate of the reaction?

For which order reaction is the half-life of the reaction proportional to 1/k (k is the rate constant)?

Which of the following experimental methods cannot be used to measure the rate of a reaction?

Which of the following statements best describes the condition(s)needed for a successful formation for a product according to the collision model?

For which of the following hypothetical rate laws would the units of the rate constant have the general form M^-3·time−1?

If a reaction is first-order with respect to a particular reactant,when the concentration of that reactant is increased by a factor of 2,the reaction rate will _____.

For the hypothetical reaction aA → products,the concentration of A was monitored with time.Given the following graph of the experimental data,what is the rate constant for the loss of reactant A?

The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system.The increase in rate as the temperature increases is best explained by

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Exam 13: Rates of Reaction

The rate law for the chemical reaction 5Br-(aq)+ BrO3-(aq)+ 6H+(aq)→ 3Br2(aq)+ 3H2O(l) Has been determined experimentally to be Rate = k[Br-][BrO3-][H+]2.What is the overall order of the reaction?

The reaction 3NO → N2O + NO2 is found to obey the rate law Rate = k[NO]2.If the first half-life of the reaction is found to be 2.0 s,what is the length of the fourth half-life?

When the concentrations of the reactants are increased,the rate of the reaction increases.This is best explained by

For the reaction IO3-(aq)+ 5I-(aq)+ 6H+(aq)→ 3I2(aq)+ 3H2O(l) The rate of disappearance of I O3-(aq)at a particular time and concentration is 2.5× 10-3 mol/(L · s).What is the rate of appearance of I2(aq)?

Which of the following reactions is not an example of homogeneous catalysis?

In a first-order reaction,the half-life is 139 minutes.What is the rate constant?

The rate constant for a first-order reaction is 1.5× 10-2 s-1 at 710 K and 4.1 × 10-2 s-1 at 884 K.What is the activation energy? (R = 8.31 J/(mol · K))

For the reaction (CH3)3CCl(aq)+ OH-(aq)→ (CH3)3COH(aq)+ Cl-(aq) It is found experimentally that doubling the initial concentration of (CH3)3CCl causes the initial reaction rate to double,but doubling the initial concentration of OH- has no effect on the rate.What is the rate law?

For the reaction 2N2O5(g)→ 4NO2(g)+ O2(g) Which of the following expressions is equal to the rate of the reaction?

For which order reaction is the half-life of the reaction proportional to 1/k (k is the rate constant)?

Which of the following experimental methods cannot be used to measure the rate of a reaction?

Which of the following statements best describes the condition(s)needed for a successful formation for a product according to the collision model?

For which of the following hypothetical rate laws would the units of the rate constant have the general form M-3·time−1?

If a reaction is first-order with respect to a particular reactant,when the concentration of that reactant is increased by a factor of 2,the reaction rate will _____.

For the hypothetical reaction aA → products,the concentration of A was monitored with time.Given the following graph of the experimental data,what is the rate constant for the loss of reactant A?

The rates of most chemical reactions are sensitive to a change in the temperature of the reaction system.The increase in rate as the temperature increases is best explained by

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Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

Organic Chemistry

Polymer Materials: Synthetic and Biological

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The rate law for the chemical reaction 5Br^-(aq)+ BrO₃^-(aq)+ 6H⁺(aq)→ 3Br₂(aq)+ 3H₂O(l) Has been determined experimentally to be Rate = k[Br^-][BrO₃^-][H⁺]².What is the overall order of the reaction?

The reaction 3NO → N₂O + NO₂ is found to obey the rate law Rate = k[NO]².If the first half-life of the reaction is found to be 2.0 s,what is the length of the fourth half-life?

For the reaction IO₃^-(aq)+ 5I^-(aq)+ 6H⁺(aq)→ 3I₂(aq)+ 3H₂O(l) The rate of disappearance of I O₃^-(aq)at a particular time and concentration is 2.5× 10^-3 mol/(L · s).What is the rate of appearance of I₂(aq)?

The rate constant for a first-order reaction is 1.5× 10^-2 s^-1 at 710 K and 4.1 × 10^-2 s^-1 at 884 K.What is the activation energy? (R = 8.31 J/(mol · K))

For the reaction (CH₃)₃CCl(aq)+ OH^-(aq)→ (CH₃)₃COH(aq)+ Cl^-(aq) It is found experimentally that doubling the initial concentration of (CH₃)₃CCl causes the initial reaction rate to double,but doubling the initial concentration of OH^- has no effect on the rate.What is the rate law?

For the reaction 2N₂O₅(g)→ 4NO₂(g)+ O₂(g) Which of the following expressions is equal to the rate of the reaction?

For which of the following hypothetical rate laws would the units of the rate constant have the general form M^-3·time−1?