Chemistry
3rd Edition
ISBN: 9780073402734
Author: Julia Burdge
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Chapter 14, Problem 102AP
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36. The gas-phase reaction
H+ D2 → HD + D
is the exchange of isotopes of hydrogen of atomic mass
1 (H) and 2 (D, deuterium). The following data were
obtained for the rate constant k of this reaction:
Temperature (K)
k (L mol-1 s-1)
299
1.56 x 104
327
3.77 x 104
346
7.6 x 104
440
106
549
1.07 × 105
745
8.7 x 107
Given a reaction between an organic molecule, denoted as A, and NaSH, we observe the following observations. Using the observations, write a rate law for the reaction.(a) The rate triples when the concentration of [A] is tripled and the concentration of [NaSH] is held constant.(b) The rate is decreased when the concentration of [A] is doubled and the concentration of [NaSH] is cut by a factor of 3.(c) The rate doubles when the concentration of [A] is cut in half and the concentration of [NaSH] is quadrupled.(d) The rate increases with an increase in temperature.
write the rate law
The rate law for the reaction NO₂ (g)+CO(g) → NO(g)+CO₂ (g) is rate k[NO₂]² ; one possible mechanism is shown on p. 717.(a) Draw a reaction energy diagram for that mechanism, giventhat ΔH°overall =-226 kJ/mol.(b) Consider the following alternative mechanism:Is the alternative mechanism consistent with the rate law? Isone mechanism more reasonable physically?
Chapter 14 Solutions
Chemistry
Ch. 14.1 - Practice Problem ATTEMPT
Write the rate...Ch. 14.1 - Practice ProblemBUILD Write the balanced equation...Ch. 14.1 - Prob. 1PPCCh. 14.1 - 14.1.1 Which expressions are correct for the rate...Ch. 14.1 - 14.1.2 In the same reaction:
if the concentration...Ch. 14.2 - Practice Problem ATTEMPT Consider the reaction:...Ch. 14.2 - Practice Problem BUILD Consider the following...Ch. 14.2 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...
Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...Ch. 14.2 - 14.2.5 The diagrams represent three experiments in...Ch. 14.3 - Prob. 1PPACh. 14.3 - Practice Problem BUILD
For the following general...Ch. 14.3 - Practice Problem CONCEPTUALIZE
Three initial-rate...Ch. 14.3 - The first-order decomposition of dinitrogen...Ch. 14.3 - The first-order decomposition of dinitrogen...Ch. 14.3 - 14.3.3 Consider the first-order reaction in which...Ch. 14.3 - Which figure below represents the numbers of...Ch. 14.3 - 14.3.5 Of the plots shown here, ___________...Ch. 14.4 - Practice Problem ATTEMPT
The rate constant for the...Ch. 14.4 - Practice Problem BUILD
Refer again to the reaction...Ch. 14.4 - Practice Problem CONCEPTUALIZE
The diagrams on...Ch. 14.4 - Use the table of data collected for a first-order...Ch. 14.4 - Prob. 2CPCh. 14.4 - Prob. 3CPCh. 14.5 - Practice Problem ATTEMPT Ethyl iodide ( C 2 H 5 I)...Ch. 14.5 - Practice Problem BUILD Use the calculated k from...Ch. 14.5 - Practice Problem CONCEPTUALIZE
Use the graph in...Ch. 14.5 - Use the following information to answer questions...Ch. 14.5 - Use the following information to answer questions...Ch. 14.5 - Use the following information to answer questions...Ch. 14.5 - 14.5.4 A plausible mechanism for the reaction:
Ch. 14.6 - Practice ProblemATTEMPT Calculate the half-life of...Ch. 14.6 - Practice ProblemBUILD Calculate the rate constant...Ch. 14.6 - Practice Problem CONCEPTUALIZE
The diagrams show a...Ch. 14.7 - Practice Problem ATTEMPT
The reaction is second...Ch. 14.7 - Practice Problem BUILD
Determine the initial...Ch. 14.7 - Practice ProblemCONCEPTUALIZE The diagrams below...Ch. 14.8 - Practice ProblemATTEMPT The second-order rate...Ch. 14.8 - Practice Problem BUILD Use the graph to determine...Ch. 14.8 - Prob. 1PPCCh. 14.9 - Practice ProblemATTEMPT Use the data in the...Ch. 14.9 - Practice ProblemBUILD Based on the data shown in...Ch. 14.9 - Practice Problem CONCEPTUALIZE
According to the...Ch. 14.10 - Practice ProblemATTEMPT Calculate the rate...Ch. 14.10 - Practice ProblemBUILD Calculate the rate constant...Ch. 14.10 - Practice ProblemCONCEPTUALIZE According to the...Ch. 14.11 - Practice Problem ATTEMPT
The reaction between and...Ch. 14.11 - Practice ProblemBUILD Propose a plausible...Ch. 14.11 - Practice Problem CONCEPTUALIZE
How many steps are...Ch. 14.12 - Practice Problem ATTEMPT
Show that the following...Ch. 14.12 - Practice Problem BUILD
The reaction proceeds via...Ch. 14.12 - Practice Problem CONCEPTUALIZE
The reaction of is...Ch. 14 - Prob. 1KSPCh. 14 - Prob. 2KSPCh. 14 - Prob. 3KSPCh. 14 - Prob. 4KSPCh. 14 - 14.1 What is meant by the rate of a chemical...Ch. 14 - Distinguish between average rate and instantaneous...Ch. 14 - What are the advantages of measuring the initial...Ch. 14 - Identify two reactions that are very slow (take...Ch. 14 - Write the reaction rate expressions for the...Ch. 14 - Write the reaction rate expressions for the...Ch. 14 - Consider the reaction: 2NO ( g ) + O 2 ( g ) → 2NO...Ch. 14 - 14.8 Consider the reaction:
Suppose that at a...Ch. 14 - 14.9 Explain what is meant by the rate law of a...Ch. 14 - Prob. 10QPCh. 14 - What are the units for the rate constants of...Ch. 14 - 14.12 Consider the zeroth-order reaction: a ...Ch. 14 - 14.13 The rate constant of a first-order reaction...Ch. 14 - Identify two reactions that are very slow (take...Ch. 14 - The rate law for the reaction: N H 4 + ( a q )+N O...Ch. 14 - Use the data in Table 14.2 to calculate the rate...Ch. 14 - 14.17 Consider the reaction:
From the following...Ch. 14 - Consider the reaction: X + Y → Z From the...Ch. 14 - Determine the overall orders of the reactions to...Ch. 14 - 14.20 Consider the reaction:
The rate of the...Ch. 14 - Cyclobutane decomposes to ethylene according to...Ch. 14 - The following gas-phase reaction was studied at...Ch. 14 - Write an equation relating the concentration of a...Ch. 14 - 14.24 Define half-life. Write the equation...Ch. 14 - Prob. 25QPCh. 14 - 14.26 For a first-order reaction, how long will it...Ch. 14 - What is the half-life of a compound if 75 percent...Ch. 14 - 14.28 The thermal decomposition of phosphine into...Ch. 14 - The rate constant for the second-order reaction:...Ch. 14 - The rate constant for the second-order reaction:...Ch. 14 - 14.31 The second-order rate constant for the...Ch. 14 - Prob. 32QPCh. 14 - 14.33 The reaction shown here follows first-order...Ch. 14 - 14 34 Define activation energy. What role does...Ch. 14 - Prob. 35QPCh. 14 - Prob. 36QPCh. 14 - The burning of methane in oxygen is a highly...Ch. 14 - Sketch a potential-energy versus reaction progress...Ch. 14 - The reaction H+H 2 → H 2 +H has been studied for...Ch. 14 - Over the range of about ±3°C from normal body...Ch. 14 - For the reaction: NO ( g ) + O 3 ( g ) → NO 2 ( g...Ch. 14 - The rate constant of a first-order reaction is 4...Ch. 14 - The rate constants of some reactions double with...Ch. 14 - 14.44 The rate at which tree crickets chirp is ...Ch. 14 - The rate of bacterial hydrolysis of fish muscle is...Ch. 14 - Prob. 46QPCh. 14 - Given the same reactant concentrations, the...Ch. 14 - 14.48 Variation of the rate constant with...Ch. 14 - 14.49 Diagram A describes the initial state of...Ch. 14 - 14 50 What do we mean by the mechanism of a...Ch. 14 - 14.51 What is an elementary step? What is the...Ch. 14 - 14.52 Classify the following elementary reactions...Ch. 14 - Reactions can be classified as unimolecular,...Ch. 14 - Determine the molecularity, and write the rate law...Ch. 14 - 14.55 What is the rate-determining step of a...Ch. 14 - 14.56 The equation for the combustion of ethane ...Ch. 14 - Specify which of the following species cannot be...Ch. 14 - Classify each of the following elementary steps as...Ch. 14 - 14.59 The rate law for the reaction:
is given by...Ch. 14 - For the reaction x 2 + y + z → x y + x z , it is...Ch. 14 - The rate law for the reaction: 2H 2 ( g ) + 2NO (...Ch. 14 - 14.62 The rate law for the decomposition of ozone...Ch. 14 - 14.63 How does a catalyst increase the rate of a...Ch. 14 - 14.64 What are the characteristics of a...Ch. 14 - A certain reaction is known to proceed slowly at...Ch. 14 - Most reactions, including enzyme-catalyzed...Ch. 14 - 14.67 Are enzyme-catalyzed reactions examples of...Ch. 14 - The concentrations of enzymes in cells are usually...Ch. 14 - When fruits such as apples and pears are cut. the...Ch. 14 - The first-order rate constant for the dehydration...Ch. 14 - Which two potential-energy profiles represent the...Ch. 14 - Consider the following mechanism for the...Ch. 14 - List four factors that influence the rate of a...Ch. 14 - 14.71 Suggest experimental means by which the...Ch. 14 - 14.75 “The rate constant for the reaction:
is .”...Ch. 14 - Prob. 76APCh. 14 - The following diagrams represent the progress of...Ch. 14 - The following diagrams show the progress of the...Ch. 14 - Prob. 79APCh. 14 - Prob. 80APCh. 14 - 14.81 When methyl phosphate is heated in acid...Ch. 14 - The rate of the reaction: CH 3 COOC 2 H 5 ( a q )...Ch. 14 - Explain why most metals used in catalysis are...Ch. 14 - Prob. 84APCh. 14 - The bromination of acetone is acid-catalyzed: CH 3...Ch. 14 - The decomposition of N 2 O to N 2 and O 2 is a...Ch. 14 - 14.87 The reaction proceeds slowly in aqueous...Ch. 14 - Prob. 88APCh. 14 - The integrated rate law for the zeroth-order...Ch. 14 - 14.90 A flask contains a mixture of compounds A...Ch. 14 - Prob. 91APCh. 14 - 14.92 The rate law for the reaction . Which of the...Ch. 14 - 14.93 The reaction of to form 2EG is exothermic,...Ch. 14 - 14.94 The activation energy for the decomposition...Ch. 14 - Prob. 95APCh. 14 - 14.96 When 6 g of granulated Zn is added to a...Ch. 14 - Prob. 97APCh. 14 - 14.98 A certain first-order reaction is 35.5...Ch. 14 - 14.99 The decomposition of dinitrogen pentoxide...Ch. 14 - 14.100 The thermal decomposition of obeys...Ch. 14 - 14.101 When a mixture of methane and bromine is...Ch. 14 - 14.102 The rate of the reaction between to form...Ch. 14 - The rate constant for the gaseous reaction: H 2 (...Ch. 14 - A gas mixture containing CH 3 fragments. C 2 H 6...Ch. 14 - Consider the following elementary step: X + 2Y →...Ch. 14 - 14.106 The following scheme in which A is...Ch. 14 - 14.107 (a) Consider two reactions, A and B. If the...Ch. 14 - The rate law for the following reaction: CO ( g )...Ch. 14 - Consider the following elementary steps for a...Ch. 14 - Prob. 110APCh. 14 - Consider the following potential-energy profile...Ch. 14 - The rate of a reaction was followed by the...Ch. 14 - 14.113 The first-order rate constant for the...Ch. 14 - 14.114 Many reactions involving heterogeneous...Ch. 14 - Thallium(I) is oxidized by cerium(IV) as follows:...Ch. 14 - The activation energy for the reaction: N 2 O ( g...Ch. 14 - Δ H ° for the reaction in Problem 14.116 is -164...Ch. 14 - 14.118 At a certain elevated temperature, ammonia...Ch. 14 - 14.119 The following expression shows the...Ch. 14 - In a certain industrial process involving a...Ch. 14 - Strontium-90, a radioactive isotope, is a major...Ch. 14 - Prob. 122APCh. 14 - Prob. 123APCh. 14 - A factory that specializes in the refinement of...Ch. 14 - 14.125 When the concentration of A in the reaction...Ch. 14 - 14.126 The activity of a radioactive sample is the...Ch. 14 - Prob. 127APCh. 14 - Prob. 128APCh. 14 - Prob. 129APCh. 14 - Prob. 130APCh. 14 - Prob. 131APCh. 14 - Prob. 132APCh. 14 - Prob. 133APCh. 14 - 14.134 At a certain elevated temperature, ammonia...Ch. 14 - Polyethylene is used in many items, including...Ch. 14 - In recent years, ozone in the stratosphere has...Ch. 14 - Metastron, an aqueous solution of 89 SrCl 2 , is a...Ch. 14 - Metastron, an aqueous solution of 89 SrCl 2 , is a...Ch. 14 - Metastron, an aqueous solution of 89 SrCl 2 , is a...Ch. 14 - Metastron, an aqueous solution of 89 SrCl 2 , is a...
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- The addition of NO accelerates the decomposition ofN2O, possibly by the following mechanism:NO(g) + N2O(g)--->N2(g) + NO2(g)2 NO2(g)--->2 NO(g) + O2(g)(a) What is the chemical equation for the overall reaction?Show how the two steps can be added to give theoverall equation. (b) Is NO serving as a catalyst or an intermediatein this reaction? (c) If experiments show thatduring the decomposition of N2O, NO2 does not accumulatein measurable quantities, does this rule out the proposedmechanism?arrow_forwardWhat will the outcome of this reaction be? Please explain why the correct answer is D and give a drawing explanation of the mechanism of the reaction.arrow_forwardFor the reaction: 2N205(g) -->4NO(g) + O2(g) (a) write the mathematical rate expression in terms of (i) the disappearance of N2O5 (Reactant); (ii) the formation of NO (Product); (iii) the formation of O2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)arrow_forward
- 1. Which of the following statements is incorrect? (A) The reaction in which the rate equation corresponds to a stoichiometric equation is called an elementary reaction. (B) Molecularity of a reaction may not be equal to the order of reaction. (C) With increase in temperature, the rate constant obeying Arrhenius equation decreases. (D) Rate of a chemical reaction is independent of the concentration of the reactants for a zero order reaction. 2. The rate of a gas phase reaction is given by, kCACB. If the volume of the reaction vessel is reduced to l/3rd of its initial volume, then the reaction rate compared to the original rate will be _____ times. (A) 3 (C) 6 (B) 9 (D) 12 3. A given number of molecules (i.e., moles) of a particular chemical species have reacted or disappeared when any of the following occurs except (A) Combination (C) Isomerization (B) Decomposition (D) Isolation Please Answer all!arrow_forwardAssume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?arrow_forwardCleavage of C2H6 to produce two CH3· radicals is a gas-phase reaction that occurs at 700 °C. This reaction is first order, with k = 5.46 × 10−4 s−1. Write down the chemical equation for the cleavage reaction and the rate equations. How long will it take for the reaction to go to 15% completion? Show your workings.arrow_forward
- Which of the following is correct? (A) The activation energy changes when temperature changes. (B) The Arrhenius equation only applies to 1st order reactions. (C) The rate constants at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction. (D) The rates of reaction at higher temperatures are ALWAYS larger than at low temperatures for the same chemical reaction.arrow_forwardWhen the rate of the reversible reaction A + BSC is studied under a certain set of conditions, it is found that the rate of the forward reaction is kA]. What can be concluded about the rate law for the reverse reaction under these conditions? (A) Rate = k-[C] %3D (B) Rate = k [B] (C) The rate law of the reverse reaction cannot be determined from the information given. (D) An crror must have been made, since if the reaction is reversible, the forward rate law must be Rate = k{A][B]. %3Darrow_forwardThe reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3H2(g) → 2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 mol L-1 s-1. At what rate is hydrogen consumed?arrow_forward
- Some reactions proceed through a chain mechanism involving radicals, which are highly reactive species with one or more unpaired electrons. The radicals are produced in initiation steps, through either thermal or photodissociation. Reactions in which the radical centre is transferred are called propagation steps. The radicals are lost in termination steps. Consider the following chain mechanism:(1) AH → A + H·(2) A → B· + C(3) AH + B· → A + D(4) A + B· → P(a) Identify the initiation, propagation, and termination steps.(b) Use the steady-state approximation to deduce that the decompositionof AH is f irst-order in AH.arrow_forward(a) Describe the term “integrated rate law” and briefly explain how it can be used tographically obtain the order of a reaction. (4)(b) Define the term “half-life of a substance” and briefly explain how it be used todetermine the order of the reaction and the rate constant for a first-order reaction. (4)arrow_forwardThe iodate ion is reduced by sulfite according to the followingreaction:IO3-(aq) + 3 SO32-(aq) -----> I-(aq) + 3 SO42-(aq)The rate of this reaction is found to be first order in IO3-,first order in SO32-, and first order in H+.(a) Write the rate law for the reaction.(b) By what factor will the rate of the reaction change ifthe pH is lowered from 5.00 to 3.50? Does the reactionproceed more quickly or more slowly at the lower pH?(c) Explain how the reaction can be pH-dependent even thoughH+ does not appear in the overall reaction.arrow_forward
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