Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 13, Problem 40RQ
What is the definition of an elementary process? How are elementary processes related to the mechanism of a reaction?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 13 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 13 - The iodate ion reacts with sulfite ions in the...Ch. 13 - Hydrogen sulfide burns in oxygen ro form sulfur...Ch. 13 - Use the graph in Figure 13.5 to estimate the rare...Ch. 13 - Practice Exercise 13.4 Use the graph in Figure...Ch. 13 - Prob. 5PECh. 13 - The rate law for the decomposition of HItoI2andH2...Ch. 13 - The reaction, BrO3-+3SO32-Br-+3SO42- has the rate...Ch. 13 - Practice Exercise 13.8
A certain reaction has an...Ch. 13 - Practice Exercise 13.9
For the reaction of with...Ch. 13 - Use the data from the other four experiments in...
Ch. 13 - Practice Exercise 13.11
Use the rate law...Ch. 13 - The following reaction is investigated to...Ch. 13 - Ordinary sucrose (table sugar) reacts with water...Ch. 13 - Practice Exercise 13.14 A certain reaction has the...Ch. 13 - When designing a consumer product, it is desirable...Ch. 13 - Practice Exercise 13.16
In Practice Exercise...Ch. 13 - Practice Exercise 13.17
In Practice Exercise...Ch. 13 -
Practice Exercise 13.15
From the answer to...Ch. 13 - Practice Exercise 13.19 The radioactive isotope,...Ch. 13 - Prob. 20PECh. 13 - Prob. 21PECh. 13 - For the reaction in Example 13.10, determine how...Ch. 13 - Practice Exercise 13.23
A sample of nitrosyl...Ch. 13 - Practice Exercise 13.24
The reaction is second...Ch. 13 - Suppose that the value of t1/2 for a certain...Ch. 13 - The reaction CH3I+HICH4+I2 was observed to have...Ch. 13 - Practice Exercise 13.27
Ozone decomposes to form...Ch. 13 - Prob. 28PECh. 13 - Practice Exercise 13.29
Select the reactions below...Ch. 13 - Ozone, O3, reacts with nitric oxide, NO, to form...Ch. 13 - Practice Exercise 13.31
The mechanism for the...Ch. 13 - Why are chemical reactions usually carried out in...Ch. 13 - 13.2 Give an example from everyday experience of...Ch. 13 - 13.3 What is a homogeneous reaction? What is a...Ch. 13 - How does particle size affect the rate of a...Ch. 13 - Prob. 5RQCh. 13 - 13.6 The rate of hardening of epoxy glue depends...Ch. 13 - 13.7 A PolaroidTM instant photograph develops...Ch. 13 - Prob. 8RQCh. 13 - 13.9 Persons who have been submerged in very cold...Ch. 13 - How does an instantaneous rate of reaction differ...Ch. 13 - What is the difference between the rate of...Ch. 13 - Explain how the initial instantaneous rate of...Ch. 13 - 13.13 What are the units of reaction rate? What is...Ch. 13 - 13.14 Describe how to determine the instantaneous...Ch. 13 - What are the units of the rate constant for (a) a...Ch. 13 - Prob. 16RQCh. 13 - Prob. 17RQCh. 13 - If the concentration of a reactant is doubled and...Ch. 13 - If the concentration of a reactant is doubled and...Ch. 13 - If the concentration of a reactant is doubled, by...Ch. 13 - In an experiment, the concentration of a reactant...Ch. 13 - Biological reactions usually involve the...Ch. 13 - Rearrange the integrated rate equations for (a) a...Ch. 13 - 13.24 How is the half-life of a first-order...Ch. 13 - 13.25 How is the half-life of a second-order...Ch. 13 - How is the half-life of a zero-order reaction...Ch. 13 - 13.27 Derive the equations for for first- and...Ch. 13 - 13.28 The integrated rate law for a zero-order...Ch. 13 - Which of the following graphs represents the data...Ch. 13 - 13.30 What is the basic postulate of collision...Ch. 13 - What two factors influence the effectiveness of...Ch. 13 - In terms of the kinetic theory, why does an...Ch. 13 - Prob. 33RQCh. 13 - Prob. 34RQCh. 13 - Draw a potential energy diagram for an exothermic...Ch. 13 - 13.36 Some might say that the “transition state...Ch. 13 - What is the activation energy? How is the...Ch. 13 - 13.38 The decomposition of carbon dioxide,
has an...Ch. 13 - 13.39 Draw the potential energy diagram for an...Ch. 13 - What is the definition of an elementary process?...Ch. 13 - What is a rate-determining step?Ch. 13 - What is an intermediate in the context of reaction...Ch. 13 - Free radicals are discussed in Chemistry Outside...Ch. 13 - Suppose we compared two reactions, one requiring...Ch. 13 - In what way is the rate law for a reaction related...Ch. 13 - How does an elementary process relate to (a) the...Ch. 13 - How does a catalyst increase the rate of a...Ch. 13 - 13.48 What is a homogeneous catalyst? How does it...Ch. 13 - What is the purpose of the catalytic converter...Ch. 13 - Tell how you would recognize a catalyst in a...Ch. 13 - Prob. 51RQCh. 13 - Why should leaded gasoline not be used in cars...Ch. 13 - The following data were collected at a certain...Ch. 13 - 13.54 The following data were collected for the...Ch. 13 - For the reaction, 2A+B3C, it was found that the...Ch. 13 - In the reaction, 3H2+N22NH3, how does the rate of...Ch. 13 - In the combustion of hexane (a low-boiling...Ch. 13 - At a certain moment in the reaction 2N2O54NO2+O2...Ch. 13 - Consider the reaction,...Ch. 13 - 13.60 The decomposition of phosphine, a very toxic...Ch. 13 - 13.61 Estimate the rate of the reaction,
given...Ch. 13 - 13.62 Estimate the rate of the reaction,
given...Ch. 13 - The oxidation of NO (released in small amounts in...Ch. 13 - The rate law for the decomposition of N2O5 is rate...Ch. 13 - The rate law for a certain enzymatic reaction is...Ch. 13 - 13.66 Radon-220 is radioactive, and decays into...Ch. 13 - The following data were collected for the reaction...Ch. 13 - Cyclopropane, C3H6, is a gas used as a general...Ch. 13 - 13.69 The reaction of iodide ion with hypochlorite...Ch. 13 - 13.70 The formation of small amounts of nitrogen...Ch. 13 - At a certain temperature, the following data were...Ch. 13 - The following data were obtained for the reaction...Ch. 13 - Data for the decomposition of SO2Cl2 according to...Ch. 13 - Prob. 74RQCh. 13 - The decomposition of SO2Cl2 described in Problem...Ch. 13 - 13.76 The decomposition of acetaldehyde, was...Ch. 13 - If it takes 75.0 min for the concentration of a...Ch. 13 - It takes 15.4 minutes for the concentration of a...Ch. 13 - The concentration of a drug in the body is often...Ch. 13 - 13.80 Phosphine, , decomposes into phosphorus, ,...Ch. 13 - Hydrogen iodide decomposes according to the...Ch. 13 - 13.82 The reaction of to form is second...Ch. 13 - Using the information determined in Problem 13.79,...Ch. 13 - The second-order rate constant for the...Ch. 13 - The half-life of a certain first-order reaction is...Ch. 13 - Strontium-90 has a half-life of 28 years. How long...Ch. 13 - 13.87 Using the graph from Problem 13.53,...Ch. 13 - Using the graph from Problem 13.54, determine how...Ch. 13 - Hydrogen peroxide, which decomposes in a...Ch. 13 - SO2Cl2 decomposes in a first-order process with a...Ch. 13 - Prob. 91RQCh. 13 - A tree killed by being buried under volcanic ash...Ch. 13 - Prob. 93RQCh. 13 - Prob. 94RQCh. 13 - The following data were collected for a reaction:...Ch. 13 - Rate constants were measured at various...Ch. 13 - NOCl decomposes as:...Ch. 13 - 13.98. The conversion of cyclopropane, an...Ch. 13 - The decomposition of N2O5 has an activation energy...Ch. 13 - At 35C, the rate constant for the reaction...Ch. 13 - The oxidation of NO to NO2, one of the reactions...Ch. 13 - A reaction has the following mechanism:...Ch. 13 - If the reaction NO2+CONO+CO2 occured by a one-step...Ch. 13 - If the reaction 2NO2(g)+F2(g)2NO2F(g) occurred by...Ch. 13 - Consider the general reaction AB+CAC+B If this...Ch. 13 - Nitrogen dioxide reacts with carbon monoxide to...Ch. 13 - 13.107. The oxidation of nitrogen monoxide with...Ch. 13 - The reaction of chloroform and chlorine forms...Ch. 13 - The following data were collected for the reaction...Ch. 13 - The age of wine can be determined by measuring the...Ch. 13 - 13.111 On the following graph, label the products,...Ch. 13 - Carbon-14 dating can be used to estimate the age...Ch. 13 - *13.113 What percentage of cesium chloride made...Ch. 13 - For the following reactions, predict how the rate...Ch. 13 - One of the reactions that occurs in polluted air...Ch. 13 - * 13.116 Suppose a reaction occurs with the...Ch. 13 - The decomposition of urea, (NH2)2CO,in0.10MHCl...Ch. 13 - Show that for a reaction that obeys the general...Ch. 13 - 13.119 The rates of many reactions approximately...Ch. 13 - If the rate constant for a first-order reaction is...Ch. 13 - For the following potential energy diagram, which...Ch. 13 - Prob. 122RQCh. 13 - Prob. 123RQCh. 13 -
*13.124 The cooking of an egg involves the...Ch. 13 -
*13.125 The following question is based on...Ch. 13 - Prob. 126RQCh. 13 - The experimental rate law for the reaction...Ch. 13 - Radioactive samples are considered to become...Ch. 13 - Use a spreadsheet to generate a graph for the data...Ch. 13 - 13.130 Use a spreadsheet to generate separate...Ch. 13 - Prob. 131RQCh. 13 - The catalyzed decomposition of ethanol at 327C has...Ch. 13 - *13.133 On December 19, 2007, the T2 Laboratories,...Ch. 13 - Prob. 134RQCh. 13 - Prob. 135RQCh. 13 - Can a reaction have a negative activation energy?...Ch. 13 - *13.137 Assume you have a three-step mechanism....Ch. 13 - 13.138 What range of ages can dating reliably...Ch. 13 - 13.139 Why are initial reaction rates used to...Ch. 13 - If a reaction is reversible (i.e., the products...Ch. 13 - Prob. 141RQCh. 13 - *13.142 How would you measure the rate of an...Ch. 13 - * 13.143 For a reaction done on the ton scale,...Ch. 13 - 13.44 Can we use molality instead of molarity in...
Additional Science Textbook Solutions
Find more solutions based on key concepts
2. A schedule of experiments for a laboratory indicates that the 1-bromobutane preparation is paired with the p...
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
Calculate the lattice energy of CaCl2 using a Born-Haber cycle and data from Appendices F and L and Table 7.5. ...
Chemistry & Chemical Reactivity
The solution on both sides of a membrane have to be compared. Concept introduction: Solution is a homogeneous m...
Chemistry: Matter and Change
1.2 Ask two of your friends (not in class) to define the terms in problem1.1.
Do their answers agee with the d...
Chemistry: An Introduction to General, Organic, and Biological Chemistry (12th Edition) - Standalone book
Consider the reaction between sulfur trioxide and water: So3(g)+H2O(l)H2SO4(aq) A chemist allows 61.5 g of SO3 ...
Introductory Chemistry (6th Edition)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forwardIn Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.arrow_forwardCan a reaction mechanism ever be proven correct? Can it be proven incorrect?arrow_forward
- Compare the functions of homogeneous and heterogeneous catalysts.arrow_forwardDetermine a rate law for the chlorination of methane assuming that the second step is the rate-determining step and that the first step can be approximated by the steady-state approximation. What is the difference between the answer here and the answer for the previous exercise?arrow_forwardNitrosyl bromide decomposes to nitrogen oxide and bromine. Use the following data to determine the order of the decomposition of nitrosyl bromide.arrow_forward
- Given the following mechanism for a chemical reaction: H2O2+IH2O+IOH2O2+IOH2O+O2+I a Write the overall reaction. b Identify the catalyst and the reaction intermediate. c With the information given in this problem, can you write the rate law? Explain.arrow_forwardTwo mechanisms are proposed for the reaction 2NO(g)+O2(g)2NO2(g)Mechanism 1: NO+O2NO3(fast) NO3+NO2NO2(slow) Mechanism 2: NO+ON2O2(fast) N2O2+O22NO2(slow) Show that each of these mechanisms is consistent with the observed rate law: rate=k[ NO2 ]2[ O2 ].arrow_forwardMany biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.arrow_forward
- A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?arrow_forwardConsider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5arrow_forward11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Kinetics: Initial Rates and Integrated Rate Laws; Author: Professor Dave Explains;https://www.youtube.com/watch?v=wYqQCojggyM;License: Standard YouTube License, CC-BY