The activation energy for the reaction CH3CO $\rarr$ CH3 + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

A) 0.40 B) 1.1 C) 2.5 D) 4.0 E) 5.0 A) 0.40 B) 1.1 C) 2.5 D) 4.0 E) 5.0

Peroxodisulfate ion can oxidize iodide ions to iodine according to the balanced equation S2O82- + 2I - $\rarr$2SO42- + I2. The reaction is catalyzed by certain chemical species. Identify the catalyst in the following mechanism: Step 1: Fe3+ + 2I - $\rarr$ Fe2+ + I2 Step 2: S2O82- + Fe2+ $\rarr$ 2SO42- + Fe3+

A) Fe3+ B) I - C) S2O82- D) Fe2+ E) SO42- A) Fe3+ B) I - C) S2O82- D) Fe2+ E) SO42-

Nitric acid is formed by the gas-phase hydrolysis of N2O5. Draw an energy profile curve for the reaction N2O5 + H2O$\rarr$2HNO3 given that Ea(forward)= 15 kJ and Ea(reverse)= 51 kJ/mol. Label the activation energies of the forward and reverse reactions and label $\Delta$H for the reaction.

The answer of Nitric acid is formed by the gas-phase...

The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr. If one begins with 600. mmHg of pure SO2Cl2 in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr A) 6.45 hr B) 11.1 hr C) 3.91 hr D) 20.3 hr E) 6.91 hr

Exam 14: Chemical Kinetics

The rate constant for a certain first-order reaction is 0.40/min. What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

(Short Answer)

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Question 21

The isomerization of cyclopropane follows first order kinetics. The rate constant at 700 K is 6.20 * 10^-4min^-1, and the half-life at 760 K is 29.0 min. Calculate the activation energy for this reaction.

(Multiple Choice)

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Question 22

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?

(Multiple Choice)

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Question 23

The isomerization of methyl isocyanide, CH₃NC $\rarr$ CH₃CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction.

(Multiple Choice)

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Question 24

A certain reaction A $\rarr$ products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete?

(Multiple Choice)

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Question 25

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate should be expressed as

(Multiple Choice)

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Question 26

The activation energy for the reaction CH₃CO $\rarr$ CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

(Multiple Choice)

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Question 27

An increase in the temperature of the reactants causes an increase in the rate of reaction. The best explanation for this behavior is that as the temperature increases,

(Multiple Choice)

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Question 28

Peroxodisulfate ion can oxidize iodide ions to iodine according to the balanced equation S₂O₈^2-+ 2I^- $\rarr$ 2SO₄^2- + I₂. The reaction is catalyzed by certain chemical species. Identify the catalyst in the following mechanism: Step 1: Fe³⁺ + 2I^- $\rarr$ Fe²⁺ + I₂ Step 2: S₂O₈^2- + Fe²⁺ $\rarr$ 2SO₄^2- + Fe³⁺

(Multiple Choice)

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Question 29

In which of the forms listed below would 0.5 g aluminum react the fastest with gaseous chlorine at 25°C?

(Multiple Choice)

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Question 30

Nitric acid is formed by the gas-phase hydrolysis of N₂O₅. Draw an energy profile curve for the reaction N₂O₅ + H₂O $\rarr$ 2HNO₃ given that E_a(forward)= 15 kJ and E_a(reverse)= 51 kJ/mol. Label the activation energies of the forward and reverse reactions and label $\Delta$ H for the reaction.

(Essay)

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Question 31

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate of appearance of C given by ( $\Delta$ [C]/ $\Delta$ t)may also be expressed as

(Multiple Choice)

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Question 32

For a second order reaction, the half-life is equal to

(Multiple Choice)

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Question 33

For the reaction X + Y $\rarr$ Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. $For the reaction X + Y \rarr Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. What is the rate law for this reaction?$ What is the rate law for this reaction?

(Multiple Choice)

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Question 34

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day^-1. How long will it take for half of the toxin to decompose?

(Multiple Choice)

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Question 35

The rate constant of a first-order reaction, A $\rarr$ products, can be determined from a graph of ln[A] versus t.

(True/False)

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Question 36

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr. If one begins with 600. mmHg of pure SO₂Cl₂ in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

(Multiple Choice)

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Question 37

It takes 42.0 min for the concentration of a reactant in a first-order reaction to drop from 0.45 M to 0.32 M at 25°C. How long will it take for the reaction to be 90% complete?

(Multiple Choice)

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Question 38

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H₂S(g)+ O₂(g) $\rarr$ 2S(s)+ 2H₂O(l)

(Multiple Choice)

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Question 39

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 * 10^-3 min^-1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 114

The rate constant for a certain first-order reaction is 0.40/min. What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

The isomerization of cyclopropane follows first order kinetics. The rate constant at 700 K is 6.20 * 10^-4min^-1, and the half-life at 760 K is 29.0 min. Calculate the activation energy for this reaction.

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?

The isomerization of methyl isocyanide, CH₃NC $\rarr$ CH₃CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction.

A certain reaction A $\rarr$ products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete?

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate should be expressed as

The activation energy for the reaction CH₃CO $\rarr$ CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

An increase in the temperature of the reactants causes an increase in the rate of reaction. The best explanation for this behavior is that as the temperature increases,

In which of the forms listed below would 0.5 g aluminum react the fastest with gaseous chlorine at 25°C?

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate of appearance of C given by ( $\Delta$ [C]/ $\Delta$ t)may also be expressed as

For a second order reaction, the half-life is equal to

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day^-1. How long will it take for half of the toxin to decompose?

The rate constant of a first-order reaction, A $\rarr$ products, can be determined from a graph of ln[A] versus t.

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr. If one begins with 600. mmHg of pure SO₂Cl₂ in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

It takes 42.0 min for the concentration of a reactant in a first-order reaction to drop from 0.45 M to 0.32 M at 25°C. How long will it take for the reaction to be 90% complete?

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H₂S(g)+ O₂(g) $\rarr$ 2S(s)+ 2H₂O(l)

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 * 10^-3 min^-1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 14: Chemical Kinetics

The rate constant for a certain first-order reaction is 0.40/min. What is the initial rate in mole/L·min, if the initial concentration of the compound involved is 0.50 mol/L?

The isomerization of cyclopropane follows first order kinetics. The rate constant at 700 K is 6.20 * 10-4 min-1, and the half-life at 760 K is 29.0 min. Calculate the activation energy for this reaction.

The reaction A + 2B →\rarr→ products has the rate law, rate = k[A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?

The isomerization of methyl isocyanide, CH3NC →\rarr→ CH3CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction.

A certain reaction A →\rarr→ products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete?

For the hypothetical reaction A + 3B →\rarr→ 2C, the rate should be expressed as

The activation energy for the reaction CH3CO →\rarr→ CH3 + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

An increase in the temperature of the reactants causes an increase in the rate of reaction. The best explanation for this behavior is that as the temperature increases,

In which of the forms listed below would 0.5 g aluminum react the fastest with gaseous chlorine at 25°C?

Nitric acid is formed by the gas-phase hydrolysis of N2O5. Draw an energy profile curve for the reaction N2O5 + H2O →\rarr→ 2HNO3 given that Ea(forward)= 15 kJ and Ea(reverse)= 51 kJ/mol. Label the activation energies of the forward and reverse reactions and label Δ\DeltaΔ H for the reaction.

For the hypothetical reaction A + 3B →\rarr→ 2C, the rate of appearance of C given by ( Δ\DeltaΔ [C]/ Δ\DeltaΔ t)may also be expressed as

For a second order reaction, the half-life is equal to

For the reaction X + Y →\rarr→ Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. What is the rate law for this reaction?

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day-1. How long will it take for half of the toxin to decompose?

The rate constant of a first-order reaction, A →\rarr→ products, can be determined from a graph of ln[A] versus t.

The first-order decomposition of SO2Cl2 to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr. If one begins with 600. mmHg of pure SO2Cl2 in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

It takes 42.0 min for the concentration of a reactant in a first-order reaction to drop from 0.45 M to 0.32 M at 25°C. How long will it take for the reaction to be 90% complete?

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g)+ O2(g) →\rarr→ 2S(s)+ 2H2O(l)

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 * 10-3 min-1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

The isomerization of cyclopropane follows first order kinetics. The rate constant at 700 K is 6.20 * 10^-4min^-1, and the half-life at 760 K is 29.0 min. Calculate the activation energy for this reaction.

The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?

The isomerization of methyl isocyanide, CH₃NC $\rarr$ CH₃CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction.

A certain reaction A $\rarr$ products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete?

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate should be expressed as

The activation energy for the reaction CH₃CO $\rarr$ CH₃ + CO is 71 kJ/mol. How many times greater is the rate constant for this reaction at 170°C than at 150°C?

For the hypothetical reaction A + 3B $\rarr$ 2C, the rate of appearance of C given by ( $\Delta$ [C]/ $\Delta$ t)may also be expressed as

A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. Fortunately, this toxin decomposes to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day^-1. How long will it take for half of the toxin to decompose?

The rate constant of a first-order reaction, A $\rarr$ products, can be determined from a graph of ln[A] versus t.

The first-order decomposition of SO₂Cl₂ to sulfur dioxide gas and chlorine gas at 320°C has a half-life of 8.75 hr. If one begins with 600. mmHg of pure SO₂Cl₂ in a 5.00-L flask at 320°C, how long does it take for the total pressure in the flask to rise to 1.000 atm?

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H₂S(g)+ O₂(g) $\rarr$ 2S(s)+ 2H₂O(l)

At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 * 10^-3 min^-1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C?