Chemistry: Structure and Properties
1st Edition
ISBN: 9780321834683
Author: Nivaldo J. Tro
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15, Problem 93E
The reaction
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 15 Solutions
Chemistry: Structure and Properties
Ch. 15 - This graph shows the concentration of the reactant...Ch. 15 - Prob. 2SAQCh. 15 - Prob. 3SAQCh. 15 - Prob. 4SAQCh. 15 - Prob. 5SAQCh. 15 - Prob. 6SAQCh. 15 - Prob. 7SAQCh. 15 - Prob. 8SAQCh. 15 - The rate constant of a reaction is measured at...Ch. 15 - Prob. 10SAQ
Ch. 15 - The mechanism shown here is proposed for the...Ch. 15 - Prob. 12SAQCh. 15 - These images represent the first-order reaction AB...Ch. 15 - Prob. 14SAQCh. 15 - Prob. 15SAQCh. 15 - Explain why lizards become sluggish in cold...Ch. 15 - Why are reaction rates important (both practically...Ch. 15 - Using the idea that reactions occur as a result of...Ch. 15 - Using the idea that reactions occur as a result of...Ch. 15 - What units are typically used to express the rate...Ch. 15 - Why is the reaction rate for reactants defined as...Ch. 15 - Explain the difference between the average rate of...Ch. 15 - Consider a simple reaction in which a reactant A...Ch. 15 - How is the order of a reaction generally...Ch. 15 - For a reaction with multiple reactants, how is the...Ch. 15 - Explain the difference between the rate law for a...Ch. 15 - Write integrated rate laws for zero-order,...Ch. 15 - What does the term half-life mean? Write the...Ch. 15 - How do reaction rates typically depend on...Ch. 15 - Prob. 15ECh. 15 - What is an Arrhenius plot? Explain the...Ch. 15 - Explain the meaning of the orientation factor in...Ch. 15 - Explain the difference between a normal chemical...Ch. 15 - In a reaction mechanism, what is an elementary...Ch. 15 - What are the two requirements for a proposed...Ch. 15 - What is an intermediate within a reaction...Ch. 15 - What is a catalyst? How does a catalyst increase...Ch. 15 - Explain the difference between homogeneous...Ch. 15 - What are the four basic steps involved in...Ch. 15 - What are enzymes? What is the active site of an...Ch. 15 - What is the general two-step mechanism by which...Ch. 15 - Consider the reaction. 2HBr(g)H2(g)+Br2(g) Express...Ch. 15 - Consider the reaction 2N2O(g)2N2(g)+O2(g) Express...Ch. 15 - For the reaction 2A(g)+B(g)3C(g) determine the...Ch. 15 - For the reaction A(g)+12B(g)2C(g) determine the...Ch. 15 - Consider the reaction. Cl2(g)+3F2(g)2ClF3(g)...Ch. 15 - Consider the reaction. 8H2S(g)+4O2(g)8H2O(g)+S8(g)...Ch. 15 - Consider the reaction: C4H8(g)2C2H4(g) The...Ch. 15 - Consider the reaction: NO2(g)NO(g)+12O2(g) The...Ch. 15 - Consider the reaction. H2(g)+Br2(g)2HBr(g) The...Ch. 15 - Consider the reaction. 2H2O2(aq)2H2O(l)+O2(g) The...Ch. 15 - This graph shows a plot of the rate of a reaction...Ch. 15 - This graph shows a plot of the rate of a reaction...Ch. 15 - What are the units of k for each type of reaction?...Ch. 15 - This reaction is first order in N2O5:...Ch. 15 - A reaction in which A, B, and C react to form...Ch. 15 - A reaction in which A, B, and C react to form...Ch. 15 - Consider the tabulated data showing initial rate...Ch. 15 - Consider the tabulated data showing initial rate...Ch. 15 - The tabulated data were collected for this...Ch. 15 - The tabulated data were collected for this...Ch. 15 - Indicate the order of reaction consistent with...Ch. 15 - Indicate the order of reaction consistent with...Ch. 15 - The tabulated data show the concentration of AB...Ch. 15 - The tabulated data show the concentration of N2O5...Ch. 15 - The tabulated data show the concentration of...Ch. 15 - Prob. 52ECh. 15 - This reaction was monitored as a function of time:...Ch. 15 - This reaction was monitored as a function of time:...Ch. 15 - Prob. 55ECh. 15 - Prob. 56ECh. 15 - Prob. 57ECh. 15 - Prob. 58ECh. 15 - The diagram shows the energy of a reaction as the...Ch. 15 - Prob. 60ECh. 15 - Prob. 61ECh. 15 - Prob. 62ECh. 15 - Prob. 63ECh. 15 - The rate constant (k) for a reaction is measured...Ch. 15 - The tabulated data shown here were collected for...Ch. 15 - Prob. 66ECh. 15 - The tabulated data were collected for the...Ch. 15 - Prob. 68ECh. 15 - A reaction has a rate constant of 0.0117/s at...Ch. 15 - A reaction has a rate constant of 0.000122/s at...Ch. 15 - Prob. 71ECh. 15 - Prob. 72ECh. 15 - Prob. 73ECh. 15 - Prob. 74ECh. 15 - Prob. 75ECh. 15 - Prob. 76ECh. 15 - Consider this three-step mechanism for a...Ch. 15 - Prob. 78ECh. 15 - Prob. 79ECh. 15 - Prob. 80ECh. 15 - Suppose that a catalyst lowers the activation...Ch. 15 - The activation barrier for the hydrolysis of...Ch. 15 - The tabulated data were collected for this...Ch. 15 - Prob. 84ECh. 15 - Consider the reaction: A+B+CD The rate law for...Ch. 15 - Consider the reaction: 2O3(g)3O2(g) The rate law...Ch. 15 - At 700 K acetaldehyde decomposes in the gas phase...Ch. 15 - Prob. 88ECh. 15 - Dinitrogen pentoxide decomposes in the gas phase...Ch. 15 - Cyclopropane (C3H6) reacts to form propene (C3H6)...Ch. 15 - Iodine atoms combine to form I2 in liquid hexane...Ch. 15 - Prob. 92ECh. 15 - The reaction AB(aq)A(g)+B(g) is second order in AB...Ch. 15 - The reaction 2H2O2(aq)2H2O(l)+O2(g) is first order...Ch. 15 - Consider this energy diagram: a. How many...Ch. 15 - Consider the reaction in which HCI adds across the...Ch. 15 - The desorption of a single molecular layer of...Ch. 15 - The evaporation of a 120-nm film of n-pentane from...Ch. 15 - Prob. 99ECh. 15 - Prob. 100ECh. 15 - Prob. 101ECh. 15 - Consider the two reactions: O+N2NO+NEa= 315 kJ/mol...Ch. 15 - Anthropologists can estimate the age of a bone or...Ch. 15 - Prob. 104ECh. 15 - Consider the gas-phase reaction: H2(g)+I2(g)2HI(g)...Ch. 15 - Consider the reaction:...Ch. 15 - Prob. 107ECh. 15 - Prob. 108ECh. 15 - A certain substance X decomposes. Fifty percent of...Ch. 15 - Prob. 110ECh. 15 - Prob. 111ECh. 15 - Prob. 112ECh. 15 - Prob. 113ECh. 15 - Prob. 114ECh. 15 - Prob. 115ECh. 15 - Prob. 116ECh. 15 - Phosgene (Cl2CO), a poison gas used in World War...Ch. 15 - The rate of decomposition of N2O3(g) to NO2(g) and...Ch. 15 - At 473 K, for the elementary reaction...Ch. 15 - Prob. 120ECh. 15 - Prob. 121ECh. 15 - A particular reaction, Aproducts has a rate that...
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
- 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_forwardThe 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_forwardThe reaction NO(g) + 1/2 Cl2(g) NOCl(g) is first-order in [Cl2] and second-order with respect to [NO]. Under a given set of conditions, the initial rate of this reaction is 620 106 mol/L s. What is the rate of this reaction if the concentration of NO is doubled and the concentration of Cl2 is reduced to half the original value? (a) 6.20 106 mol/L s (b) 124 105 mol/L s (c) 2.48 105 mol/L s (d) 4.96 105 mol/L sarrow_forward
- Gaseous 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_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_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
- Explain why half-lives are not normally used to describe reactions other than first order.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_forwardIsomerization 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_forward
- At 500 K in the presence of a copper surface, ethanol decomposes according to the equation C2H5OH(g)CH3CHO(g)+H2(g) The pressure of C2H5OH was measured as a function of time and the following data were obtained: Time(s) PC2H5OH(torr) 0 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the above data, deduce the rate law, the integrated rate law, and the value of the rate constant, all in terms of pressure units in atm and time in seconds. Predict the pressure of C2H5OH after 900. s from the start of the reaction. (Hint: To determine the order of the reaction with respect to C2H5OH, compare how the pressure of C2H5OH decreases with each time listing.)arrow_forwardSucrose, a sugar, decomposes in acid solution to give glucose and fructose. The reaction is first-order in sucrose, and the rate constant at 25 C is k = 0.21 h1. If the initial concentration of sucrose is 0.010 mol/L, what is its concentration after 5.0 h?arrow_forwardThe hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher: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 & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: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