Exhibit 12-1 The following question(s) relate to the reaction between water and a complex ion of Co2+; the rate varies with concentration as follows. (The rate has no dependence on [H2O].) Refer to Exhibit 12-1. The value and units of the rate constant are:

A) 3.6 × 103 M min-1. B) 2.8 × 10-4 M min-1. C) 3.6 × 103 min-1. D) 2.8 × 10-4 min-1. E) 3.6 × 103 M-1 min-1. A) 3.6 × 103 M min-1. B) 2.8 × 10-4 M min-1. C) 3.6 × 103 min-1. D) 2.8 × 10-4 min-1. E) 3.6 × 103 M-1 min-1.

Exam 12: Chemical Kinetics: Rates of Reactions

The decomposition of N₂O(g) to nitrogen and oxygen has the rate law $The decomposition of N2O(g) to nitrogen and oxygen has the rate law where k = 1.1 × 10-3 M-1 s-1 at 565 \circ C. If the initial concentration of a sample of N2O is 0.50 M, what is the concentration after one hour at 565 \circ C?$ where k = 1.1 × 10^-3 M^-1 s^-1 at 565^$\circ$C. If the initial concentration of a sample of N₂O is 0.50 M, what is the concentration after one hour at 565^$\circ$C?

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Question 1

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Which statement, comparing catalyzed and uncatalyzed versions of a reaction, is incorrect?

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Question 2

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Consider this proposed mechanism for the reaction of NO₂ and CO: a. Write the overall reaction represented by this mechanism. b. What are the intermediates in this reaction, if any? c. What are the catalysts in this reaction, if any? d. Write the rate law predicted by the mechanism above. e. Write the rate law you would predict if the reaction went in a single step.

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Question 3

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a. NO₂ + CO ® NO + CO₂
b. NO₃ is an intermediate; it is generated in the first step and used up in the second step.
c. One of the NO₂ molecules is a catalyst, since it is used up in the first step and regenerated in the second step.
d. Since the first step is slow (i.e., rate-determining), the rate law is
rate = k[NO₂]₂
e. Rate = k[NO₂][CO].

A certain reaction is studied at room temperature, and gives a straight line plot for 1/[reactant] versus time. Which one of the following statements is true?

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Question 4

Which of the following factors will affect the rate of a homogeneous reaction?

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Question 5

The activation energy in the Arrhenius equation can best be described as

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Question 6

Which of the following factors will affect the rate of a reaction only if it is heterogeneous?

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Question 7

Which unit is appropriate for describing reaction rates?

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Question 8

The rate law for a given reaction is rate = k[reactant]², with k = 2.64 × 10^-4 M^-1 min^-1. If the initial concentration is 0.0250 M, what is the initial rate, with the correct units?

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Question 9

If the rate law for an elementary reaction is second order, we can conclude that

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Question 10

For a reaction that is zeroth-order with respect to reactant A, and nth-order overall

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Question 11

The kinetics of a reaction are observed to be third-order. The least likely mechanism

(Multiple Choice)

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Question 12

Which statement about a rate constant is correct?

(Multiple Choice)

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Question 13

The frequency factor in the Arrhenius equation can best be described as

(Multiple Choice)

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Question 14

The units for the rate constant k must always include

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Question 15

If a reaction is first-order with respect to each of its two reactants, then the rate of the reaction is

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Question 16

Phosgene, COCl₂, is formed from Cl₂ and CO at high temperatures. The mechanism is thought to be: What is the rate law predicted for this mechanism?

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Question 17

A heterogeneous reaction mixture may contain

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Question 18

For a zero-, first- or second-order reaction the order of reaction with respect to reactant A may be determined

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Question 19

Exhibit 12-1 The following question(s) relate to the reaction between water and a complex ion of Co²⁺; the rate varies with concentration as follows. (The rate has no dependence on [H₂O].) Refer to Exhibit 12-1. The value and units of the rate constant are:

(Multiple Choice)

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Question 20

Showing 1 - 20 of 66

Which statement, comparing catalyzed and uncatalyzed versions of a reaction, is incorrect?

A certain reaction is studied at room temperature, and gives a straight line plot for 1/[reactant] versus time. Which one of the following statements is true?

Which of the following factors will affect the rate of a homogeneous reaction?

The activation energy in the Arrhenius equation can best be described as

Which of the following factors will affect the rate of a reaction only if it is heterogeneous?

Which unit is appropriate for describing reaction rates?

The rate law for a given reaction is rate = k[reactant]², with k = 2.64 × 10^-4 M^-1 min^-1. If the initial concentration is 0.0250 M, what is the initial rate, with the correct units?

If the rate law for an elementary reaction is second order, we can conclude that

For a reaction that is zeroth-order with respect to reactant A, and nth-order overall

The kinetics of a reaction are observed to be third-order. The least likely mechanism

Which statement about a rate constant is correct?

The frequency factor in the Arrhenius equation can best be described as

The units for the rate constant k must always include

If a reaction is first-order with respect to each of its two reactants, then the rate of the reaction is

Phosgene, COCl₂, is formed from Cl₂ and CO at high temperatures. The mechanism is thought to be: What is the rate law predicted for this mechanism?

A heterogeneous reaction mixture may contain

For a zero-, first- or second-order reaction the order of reaction with respect to reactant A may be determined

Exhibit 12-1 The following question(s) relate to the reaction between water and a complex ion of Co²⁺; the rate varies with concentration as follows. (The rate has no dependence on [H₂O].) Refer to Exhibit 12-1. The value and units of the rate constant are:

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Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

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Exam 12: Chemical Kinetics: Rates of Reactions

The decomposition of N2O(g) to nitrogen and oxygen has the rate law where k = 1.1 × 10-3 M-1 s-1 at 565 ∘\circ∘ C. If the initial concentration of a sample of N2O is 0.50 M, what is the concentration after one hour at 565 ∘\circ∘ C?

Which statement, comparing catalyzed and uncatalyzed versions of a reaction, is incorrect?

A certain reaction is studied at room temperature, and gives a straight line plot for 1/[reactant] versus time. Which one of the following statements is true?

Which of the following factors will affect the rate of a homogeneous reaction?

The activation energy in the Arrhenius equation can best be described as

Which of the following factors will affect the rate of a reaction only if it is heterogeneous?

Which unit is appropriate for describing reaction rates?

The rate law for a given reaction is rate = k[reactant]2, with k = 2.64 × 10-4 M-1 min-1. If the initial concentration is 0.0250 M, what is the initial rate, with the correct units?

If the rate law for an elementary reaction is second order, we can conclude that

For a reaction that is zeroth-order with respect to reactant A, and nth-order overall

The kinetics of a reaction are observed to be third-order. The least likely mechanism

Which statement about a rate constant is correct?

The frequency factor in the Arrhenius equation can best be described as

The units for the rate constant k must always include

If a reaction is first-order with respect to each of its two reactants, then the rate of the reaction is

Phosgene, COCl2, is formed from Cl2 and CO at high temperatures. The mechanism is thought to be: What is the rate law predicted for this mechanism?

A heterogeneous reaction mixture may contain

For a zero-, first- or second-order reaction the order of reaction with respect to reactant A may be determined

Exhibit 12-1 The following question(s) relate to the reaction between water and a complex ion of Co2+; the rate varies with concentration as follows. (The rate has no dependence on [H2O].) Refer to Exhibit 12-1. The value and units of the rate constant are:

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

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The rate law for a given reaction is rate = k[reactant]², with k = 2.64 × 10^-4 M^-1 min^-1. If the initial concentration is 0.0250 M, what is the initial rate, with the correct units?

Phosgene, COCl₂, is formed from Cl₂ and CO at high temperatures. The mechanism is thought to be: What is the rate law predicted for this mechanism?

Exhibit 12-1 The following question(s) relate to the reaction between water and a complex ion of Co²⁺; the rate varies with concentration as follows. (The rate has no dependence on [H₂O].) Refer to Exhibit 12-1. The value and units of the rate constant are: