The radioactive nuclide 14C decays with a t1/2 of 5730 yrs. An archaeologist is studying a woven mat using radiocarbon dating. If calculations related to the mat's original 14C content reveal that there was 5.83 × 1022 atoms of 14C present in the plant used to weave the mat, how long ago was the mat woven if modern spectroscopy was used to determine that 7.11 × 1020 atoms of 14C now exist in the sample?

A) 8.3 × 104 yrs B) 4.1 × 102 yrs C) 3.6 × 104 yrs D) 5.0 × 106 yrs A) 8.3 × 104 yrs B) 4.1 × 102 yrs C) 3.6 × 104 yrs D) 5.0 × 106 yrs C

According to the differential rate law: rate = k[X]m[Y]n. If m = 2 and n = 1, the overall reaction order is:

A) 3 B) 2 C) 1 D) 0 A) 3 B) 2 C) 1 D) 0 A

The production of nitric oxide is governed by the reaction: 4 NH3( g ) + 5 O2( g ) → 4 NO( g ) + 6 H2O( g ) If the rate at which NO is produced is 6.35 × 10 −2 mol L − 1s − 1, at what rate is O2 consumed?

A) 8.29 × 10 − 3 mol L − 1s − 1 B) 1.59 × 10 − 2 mol L − 1s − 1 C) 6.35 × 10 −2 mol L − 1s − 1 D) 7.94 × 10 −2 mol L − 1s − 1 A) 8.29 × 10 − 3 mol L − 1s − 1 B) 1.59 × 10 − 2 mol L − 1s − 1 C) 6.35 × 10 −2 mol L − 1s − 1 D) 7.94 × 10 −2 mol L − 1s − 1

Consider the production of oxygen from ozone. The mechanism includes two elementary steps: O3 + Cl → ClO + O2 ClO + O3 → Cl + 2O2 Which species is a reactive intermediate?

A) O3 B) ClO C) Cl D) both ClO and Cl A) O3 B) ClO C) Cl D) both ClO and Cl

Exam 11: Chemical Kinetics

The radioactive nuclide ¹⁴C decays with a t_1/2 of 5730 yrs. An archaeologist is studying a woven mat using radiocarbon dating. If calculations related to the mat's original ¹⁴C content reveal that there was 5.83 × 10²² atoms of ¹⁴C present in the plant used to weave the mat, how long ago was the mat woven if modern spectroscopy was used to determine that 7.11 × 10²⁰ atoms of ¹⁴C now exist in the sample?

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Question 1

Correct Answer:

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Consider the reaction: A + 2B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

According to the differential rate law: rate = k[X]^m[Y]ⁿ. If m = 2 and n = 1, the overall reaction order is:

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

The synthesis of ammonia from hydrogen and nitrogen produced the following kinetic data: What is the average rate in mL/min for the first five minutes of the reaction?

(Multiple Choice)

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Question 4

If a reaction is second order with respect to [A], doubling the concentration of [A] will result in:

(Multiple Choice)

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Question 5

Consider the elementary step: A + B → C. What type of elementary step is this?

(Multiple Choice)

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Question 6

The production of ozone begins with:

(Multiple Choice)

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Question 7

For a first-order reaction, a plot of concentration vs time provides a line with a slope equal to − k.

(True/False)

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Question 8

Consider the reaction: 2A + B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

(Multiple Choice)

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Question 9

The production of nitric oxide is governed by the reaction: 4 NH₃( g ) + 5 O₂( g ) → 4 NO( g ) + 6 H₂O( g ) If the rate at which NO is produced is 6.35 × 10⁻² mol L^{− 1}s^{− 1}, at what rate is O₂ consumed?

(Multiple Choice)

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Question 10

Consider the production of oxygen from ozone. The mechanism includes two elementary steps: O₃ + Cl → ClO + O₂ClO + O₃ → Cl + 2O₂ Which species is a reactive intermediate?

(Multiple Choice)

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Question 11

For a zero order reaction, a plot of concentration with respect to time produces a plot that is:

(Multiple Choice)

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Question 12

If a reaction is first order with respect to [A], doubling the concentration of [A] will result in:

(Multiple Choice)

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Question 13

For a first-order reaction, t_1/2 = ln 2/ k

(True/False)

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Question 14

If a reaction is zero order with respect to [B], tripling the concentration of [B] will result in:

(Multiple Choice)

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Question 15

Stirring a reaction increases the rate of the reaction by raising the energy of activation.

(True/False)

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Question 16

The rate of a reaction may be expressed as the disappearance of reactants with respect to time.

(True/False)

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Question 17

The instantaneous rate of a reaction is determined using the slope of a line tangent to the curve of the change of concentration versus time.

(True/False)

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Question 18

During the formation of MgO from the burning of Mg metal, what steps will result in an increase in the rate of reaction?

(Multiple Choice)

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Question 19

A reaction mechanism is a collection of elementary steps.

(True/False)

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Question 20

Showing 1 - 20 of 40

Consider the reaction: A + 2B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

According to the differential rate law: rate = k[X]^m[Y]ⁿ. If m = 2 and n = 1, the overall reaction order is:

The synthesis of ammonia from hydrogen and nitrogen produced the following kinetic data: What is the average rate in mL/min for the first five minutes of the reaction?

If a reaction is second order with respect to [A], doubling the concentration of [A] will result in:

Consider the elementary step: A + B → C. What type of elementary step is this?

The production of ozone begins with:

For a first-order reaction, a plot of concentration vs time provides a line with a slope equal to − k.

Consider the reaction: 2A + B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

The production of nitric oxide is governed by the reaction: 4 NH₃( g ) + 5 O₂( g ) → 4 NO( g ) + 6 H₂O( g ) If the rate at which NO is produced is 6.35 × 10⁻² mol L^{− 1}s^{− 1}, at what rate is O₂ consumed?

Consider the production of oxygen from ozone. The mechanism includes two elementary steps: O₃ + Cl → ClO + O₂ClO + O₃ → Cl + 2O₂ Which species is a reactive intermediate?

For a zero order reaction, a plot of concentration with respect to time produces a plot that is:

If a reaction is first order with respect to [A], doubling the concentration of [A] will result in:

For a first-order reaction, t_1/2 = ln 2/ k

If a reaction is zero order with respect to [B], tripling the concentration of [B] will result in:

Stirring a reaction increases the rate of the reaction by raising the energy of activation.

The rate of a reaction may be expressed as the disappearance of reactants with respect to time.

The instantaneous rate of a reaction is determined using the slope of a line tangent to the curve of the change of concentration versus time.

During the formation of MgO from the burning of Mg metal, what steps will result in an increase in the rate of reaction?

A reaction mechanism is a collection of elementary steps.

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Exam 11: Chemical Kinetics

Consider the reaction: A + 2B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

According to the differential rate law: rate = k[X]m[Y]n. If m = 2 and n = 1, the overall reaction order is:

The synthesis of ammonia from hydrogen and nitrogen produced the following kinetic data: What is the average rate in mL/min for the first five minutes of the reaction?

If a reaction is second order with respect to [A], doubling the concentration of [A] will result in:

Consider the elementary step: A + B → C. What type of elementary step is this?

The production of ozone begins with:

For a first-order reaction, a plot of concentration vs time provides a line with a slope equal to − k.

Consider the reaction: 2A + B → C, And a kinetics study on this reaction yielded: What order is the reaction with respect to ([A], [B])?

The production of nitric oxide is governed by the reaction: 4 NH3( g ) + 5 O2( g ) → 4 NO( g ) + 6 H2O( g ) If the rate at which NO is produced is 6.35 × 10 −2 mol L − 1s − 1, at what rate is O2 consumed?

Consider the production of oxygen from ozone. The mechanism includes two elementary steps: O3 + Cl → ClO + O2 ClO + O3 → Cl + 2O2 Which species is a reactive intermediate?

For a zero order reaction, a plot of concentration with respect to time produces a plot that is:

If a reaction is first order with respect to [A], doubling the concentration of [A] will result in:

For a first-order reaction, t1/2 = ln 2/ k

If a reaction is zero order with respect to [B], tripling the concentration of [B] will result in:

Stirring a reaction increases the rate of the reaction by raising the energy of activation.

The rate of a reaction may be expressed as the disappearance of reactants with respect to time.

The instantaneous rate of a reaction is determined using the slope of a line tangent to the curve of the change of concentration versus time.

During the formation of MgO from the burning of Mg metal, what steps will result in an increase in the rate of reaction?

A reaction mechanism is a collection of elementary steps.

Introduction to Chemistry

Atoms and Molecules

Molecules Moles Chemical Equations

Stoichiometry

Gases

The Periodic Table and Atomic Structure

Chemical Bonding and Molecular Structure

Molecules and Materials

Energy and Chemistry

Entropy and the Second Law of Thermodynamics

Chemical Equilibrium

Electrochemistry

Filters

According to the differential rate law: rate = k[X]^m[Y]ⁿ. If m = 2 and n = 1, the overall reaction order is:

The production of nitric oxide is governed by the reaction: 4 NH₃( g ) + 5 O₂( g ) → 4 NO( g ) + 6 H₂O( g ) If the rate at which NO is produced is 6.35 × 10⁻² mol L^{− 1}s^{− 1}, at what rate is O₂ consumed?

Consider the production of oxygen from ozone. The mechanism includes two elementary steps: O₃ + Cl → ClO + O₂ClO + O₃ → Cl + 2O₂ Which species is a reactive intermediate?

For a first-order reaction, t_1/2 = ln 2/ k