Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
9th Edition
ISBN: 9781285462530
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 14, Problem 46PS
The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2:
Step 1: Slow
NO2(g) + NO2(g) → NO(g) + NO3(g)
Step 2: Fast
NO3(g) + CO(g) → NO2(g) + CO2(g)
- (a) Show that the elementary steps add up to give the overall, stoichiometric equation.
- (b) What is the molecularity of each step?
- (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation?
- (d) Identify any intermediates in tins reaction.
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 14 Solutions
Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
Ch. 14.1 - Sucrose decomposes to fructose and glucose in acid...Ch. 14.1 - What are the relative rates of appearance or...Ch. 14.1 - Prob. 1RCCh. 14.1 - 2. Use the graph provided in Example 14.1 to...Ch. 14.2 - 1. Which of the following will not usually...Ch. 14.3 - The initial rate ( [NO]/ t] of the reaction of...Ch. 14.3 - The rate constant, k, at 25 C is 0.27/h for the...Ch. 14.3 - The reaction NO(g) + 1/2 Cl2(g) NOCl(g) is...Ch. 14.4 - Sucrose, a sugar, decomposes in acid solution to...Ch. 14.4 - Gaseous azomethane (CH3N2CH3) decomposes to ethane...
Ch. 14.4 - Prob. 3CYUCh. 14.4 - The catalyzed decomposition of hydrogen peroxide...Ch. 14.4 - Americium is used in smoke detectors and in...Ch. 14.4 - The decomposition of N2O5 is a first-order...Ch. 14.4 - Which of the following will confirm that the...Ch. 14.4 - 3. The equation for the decomposition of NO2(g) at...Ch. 14.5 - Prob. 1CYUCh. 14.5 - The colorless gas N2O4, decomposes to the brown...Ch. 14.5 - Prob. 1RCCh. 14.5 - Prob. 2RCCh. 14.6 - Nitrogen monoxide is reduced by hydrogen to give...Ch. 14.6 - Prob. 2CYUCh. 14.6 - One possible mechanism for the decomposition of...Ch. 14.6 - The rate equation for a reaction A + B C was...Ch. 14.6 - A reaction is believed to occur by the following...Ch. 14.6 - Prob. 1QCh. 14.6 - Prob. 2QCh. 14.6 - Prob. 3QCh. 14.6 - Prob. 4QCh. 14.6 - Prob. 5QCh. 14.6 - Determine the activation energy for the reaction...Ch. 14 - Give the relative rates of disappearance of...Ch. 14 - Give the relative rates of disappearance of...Ch. 14 - In the reaction 2 O3(g) 3 O2(g), the rate of...Ch. 14 - In the synthesis of ammonia, if [H2]/t = 4.5 104...Ch. 14 - Experimental data are listed here for the reaction...Ch. 14 - 6. Phenyl acetate, an ester, reacts with water...Ch. 14 - Using the rate equation Rate = k[A]2[B], define...Ch. 14 - A reaction has the experimental rate equation Rate...Ch. 14 - The reaction between ozone and nitrogen dioxide at...Ch. 14 - Nitrosyl bromide, NOBr, is formed from NO and Br2:...Ch. 14 - The data in the table are for the reaction of NO...Ch. 14 - The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)...Ch. 14 - Data for the reaction NO(g) + O2(g) NO2(g) are...Ch. 14 - Data for the following reaction are given in the...Ch. 14 - The rate equation for the hydrolysis of sucrose to...Ch. 14 - The decomposition of N2O5 in CCl4 is a first-order...Ch. 14 - The decomposition of SO2Cl2 is a first-order...Ch. 14 - The conversion of cyclopropane to propene (Example...Ch. 14 - Hydrogen peroxide, H2O2(aq), decomposes to H2O()...Ch. 14 - The decomposition of nitrogen dioxide at a high...Ch. 14 - At 573 K, gaseous NO2(g) decomposes, forming NO(g)...Ch. 14 - The dimerization of butadiene, C4H6, to form...Ch. 14 - The decomposition of ammonia on a metal surface to...Ch. 14 - Hydrogen iodide decomposes when heated, forming...Ch. 14 - The rate equation for the decomposition of N2O5...Ch. 14 - Gaseous azomethane, CH3N=NCH3, decomposes in a...Ch. 14 - The decomposition of SO2Cl2 SO2Cl2(g) SO2(g) +...Ch. 14 - The compound Xe(CF3)2 decomposes in a first-order...Ch. 14 - The radioactive isotope 64Cu is used in the form...Ch. 14 - Radioactive gold-198 is used in the diagnosis of...Ch. 14 - Prob. 31PSCh. 14 - Ammonia decomposes when heated according to the...Ch. 14 - Gaseous NO2 decomposes at 573 K. NO2(g) NO(g) + ...Ch. 14 - The decomposition of HOF occurs at 25 C. HOF(g) ...Ch. 14 - Prob. 35PSCh. 14 - Prob. 36PSCh. 14 - Calculate the activation energy, Ea, for the...Ch. 14 - If the rate constant for a reaction triples when...Ch. 14 - When healed lo a high temperature, cyclobutane,...Ch. 14 - When heated, cyclopropane is converted to propene...Ch. 14 - The reaction of H2 molecules with F atoms H2(g) +...Ch. 14 - Prob. 42PSCh. 14 - What is the rate law for each of the following...Ch. 14 - What is the rate law for each of the following...Ch. 14 - Ozone, O3, in the Earths upper atmosphere...Ch. 14 - The reaction of NO2(g) and CO(g) is thought to...Ch. 14 - A proposed mechanism for the reaction of NO2 and...Ch. 14 - The mechanism for the reaction of CH3OH and HBr is...Ch. 14 - A reaction has the following experimental rate...Ch. 14 - For a first-order reaction, what fraction of...Ch. 14 - Prob. 51GQCh. 14 - Data for the following reaction are given in the...Ch. 14 - Formic acid decomposes at 550 C according to the...Ch. 14 - Isomerization of CH3NC occurs slowly when CH3NC is...Ch. 14 - When heated, tetrafluoroethylene dimerizes to form...Ch. 14 - Data in the table were collected at 540 K for the...Ch. 14 - Ammonium cyanate, NH4NCO, rearranges in water to...Ch. 14 - Prob. 58GQCh. 14 - At temperatures below 500 K, the reaction between...Ch. 14 - Nitryl fluoride can be made by treating nitrogen...Ch. 14 - The decomposition of dinitrogen pentaoxide N2O5(g)...Ch. 14 - The data in the table give the temperature...Ch. 14 - The decomposition of gaseous dimethyl ether at...Ch. 14 - The decomposition of phosphine, PH3, proceeds...Ch. 14 - The thermal decomposition of diacetylene, C4H2,...Ch. 14 - Prob. 66GQCh. 14 - The ozone in the Earths ozone layer decomposes...Ch. 14 - Hundreds of different reactions occur in the...Ch. 14 - Data for the reaction [Mn(CO)5(CH3CN)]+ + NC5H5 ...Ch. 14 - The gas-phase reaction 2 N2O5(g) 4 NO2(g) + O2(g)...Ch. 14 - Prob. 71GQCh. 14 - The decomposition of SO2Cl2 to SO2 and Cl2 is...Ch. 14 - The decomposition of nitrogen dioxide at a high...Ch. 14 - Prob. 74GQCh. 14 - Egg protein albumin is precipitated when an egg is...Ch. 14 - A The compound 1,3-butadiene (C4H6) forms...Ch. 14 - Hypofluorous acid, HOF, is very unstable,...Ch. 14 - We know that the decomposition of SO2Cl2 is...Ch. 14 - Nitramide, NO2NH2, decomposes slowly in aqueous...Ch. 14 - Prob. 80GQCh. 14 - Prob. 83ILCh. 14 - Prob. 84ILCh. 14 - The oxidation of iodide ion by the hypochlorite...Ch. 14 - The acid-catalyzed iodination of acetone...Ch. 14 - Prob. 87SCQCh. 14 - The following statements relate to the reaction...Ch. 14 - Chlorine atoms contribute to the destruction of...Ch. 14 - Prob. 91SCQCh. 14 - Prob. 92SCQCh. 14 - The reaction cyclopropane propene occurs on a...Ch. 14 - Prob. 94SCQCh. 14 - Examine the reaction coordinate diagram given...Ch. 14 - Draw a reaction coordinate diagram for an...
Additional Science Textbook Solutions
Find more solutions based on key concepts
6. How can you use the features found in each chapter?
Human Anatomy & Physiology (2nd Edition)
An obese 55-year-old woman consults her physician about minor chest pains during exercise. Explain the physicia...
Biology: Life on Earth with Physiology (11th Edition)
How could you separate a mixture of the following compounds? The reagents available to you are water, either, 1...
Organic Chemistry (8th Edition)
45. Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium. Assume a total pre...
Chemistry: Structure and Properties (2nd 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
- The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardWrite a rate law for NO3(g) + O2(g) NO2(g) + O3(g) if measurements show the reaction is first order in nitrogen trioxide and second order in oxygen.arrow_forwardOne possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?arrow_forward
- Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?arrow_forwardThe decomposition of iodoethane in the gas phase proceeds according to the following equation: C2H5I(g)C2H4(g)+HI(g) At 660. K, k = 7.2 104 sl; at 720. K, k = 1.7 102 sl. What is the value of the rate constant for this first-order decomposition at 325C? If the initial pressure of iodoethane is 894 torr at 245C, what is the pressure of iodoethane after three half-lives?arrow_forwardGaseous azomethane (CH3N2CH3) decomposes to ethane and nitrogen when heated: CH3N2CH3(g) CH3CH3(g) + N2(g) The decomposition of azomethane is a first-order reaction with k = 3.6 104 s1 at 600 K. (a) A sample of gaseous CH3N2CH3 is placed in a flask and heated at 600 K for 150 seconds. What fraction of the initial sample remains after this time? (b) How long must a sample be heated so that 99% of the sample has decomposed?arrow_forward
- At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardAt 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment involving this reaction: t(s) [C4H6] (mol/L) 0 0.01000 1000.. 0.00629 2000. 0.00459 3000. 0.00361 a. Determine the order of the reaction in butadiene. b. In how many seconds is the dimerization 1.0% complete? c. In how many seconds is the dimerization 10.0% complete? d. What is the half-life for the reaction if the initial concentration of butadiene is 0.0200 M? e. Use the results from this problem and Exercise 45 to calculate the activation energy for the dimerization of butadiene.arrow_forwardBased on the kinetic theory of matter, what would the action of a catalyst do to a reaction that is the reverse of some reaction that we say is catalyzed?arrow_forward
- Many 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_forwardA reaction is believed to occur by the following mechanism: Stepl: 2AI (Fast equilibrium) Step 2: I + B C (Slow) Overall: 2 A + B C What experimentally determined rate law would lead to this mechanism? (a) Rate = k[A][B] (b) Rate = k[A]2[B] (c) Rate = k[A]2 (d) Rate = k[I][B]arrow_forwardYou are studying the kinetics of the reaction H2(g) + F2(g) 2HF(g) and you wish to determine a mechanism for the reaction. You run the reaction twice by keeping one reactant at a much higher pressure than the other reactant (this lower-pressure reactant begins at 1.000 atm). Unfortunately, you neglect to record which reactant was at the higher pressure, and you forget which it was later. Your data for the first experiment are: Pressure of HF (atm) Time(min) 0 0 0.300 30.0 0.600 65.8 0.900 110.4 1.200 169.1 1.500 255.9 When you ran the second experiment (in which the higher pressure reactant was run at a much higher pressure), you determine the values of the apparent rate constants to be the same. It also turns out that you find data taken from another person in the lab. This individual found that the reaction proceeds 40.0 times faster at 55C than at 35C. You also know, from the energy-level diagram, that there are three steps to the mechanism, and the first step has the highest activation energy. You look up the bond energies of the species involved and they are (in kJ/mol): H8H (432), F8F (154), and H8F (565). a. Sketch an energy-level diagram (qualitative) that is consistent with the one described previously. Hint: See Exercise 106. b. Develop a reasonable mechanism for the reaction. c. Which reactant was limiting in the experiments?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32; Author: Crash Course;https://www.youtube.com/watch?v=7qOFtL3VEBc;License: Standard YouTube License, CC-BY