Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 14, Problem 12QP
Consider the zeroth-order reaction: a
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Consider the following reaction:
2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)
(a) The rate law for this reaction is second order in NO(g) and first-order in H2(g). What is the rate law for this reaction?
(b) If the rate constant for this reaction at a certain temperature is 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M?Rate = M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?Rate = M/s
Consider the following reaction:
1.
2 N,O5 (g) → 4 NO, (g) + O, (g)
The initial concentration of N2O5 was 0.48
mol/L, and 25 minutes after initiating the
reaction, all of the N,Os has been consumed.
(a) Calculate the average rate of the reaction
over this 25-minute time interval.
(b) Is it correct to assume that the rate law is
Rate = k[N,O5]² based on the balanced
chemical equation? Briefly explain your
answer.
Consider the following reaction:
2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)
(a) The rate law for this reaction is second order in NO(g) and first order in H2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 79200, what is the reaction rate when [NO(g)] = 0.0852 M and [H2(g)] = 0.137 M?Rate =____ M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.170 M while the concentration of H2(g) is 0.137 M?Rate = ____ M/s
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 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_forward(a) For a reaction, A + B → Product, the rate law is given by, Rate = k[A]1[B]2. What is the order of the reaction?(b) Write the unit of rate constant ‘k’ for the first order reaction.arrow_forwardConsider the following reaction:2 NO(g) + 2 H2(g)--->N2(g) + 2 H2O(g)(a) The rate law for this reaction is first order in H2 andsecond order in NO. Write the rate law. (b) If the rateconstant for this reaction at 1000 K is 6.0 x 104 M-2 s-1,what is the reaction rate when [NO] = 0.035 M and[H2] = 0.015 M? (c) What is the reaction rate at 1000 Kwhen the concentration of NO is increased to 0.10 M,while the concentration of H2 is 0.010 M? (d) What is thereaction rate at 1000 K if [NO] is decreased to 0.010 M and[H2] is increased to 0.030 M?arrow_forward
- The reaction 2 NO(g) + Cl2(g) → 2 NOCl has the following rate law: Rate = k[NO]2 [Cl2]. The initial speed of the reaction was found to be 5.72×10‒6 M/s when the reaction was carried out at 25 °C with initial concentrations of 0.500 M NO and 0.250 M Cl2. What is the value of k?(a) 1.83×10‒4(b) 1.09×104(c) 9.15×10‒5(d) 5.72×10‒6arrow_forward(a) For a reaction, A + B > Product, the rate law is given by,Rate = k [A]1 [B]2 . What is the order of reaction?(b) Write the unit of rate constat ‘k’ for the first order reaction.arrow_forwardConsider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/sarrow_forward
- Assume 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_forwardThe following data was obtained from the reaction: (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2~] = 0.1 M and [NH4+] = 0.1 Marrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?arrow_forward
- 25. For the reaction, 2H,S(g)+ O,(g) = 2S(s) + 2H,0(1), which one of the following statements is absolutely true? (a) The reaction is first order with respect to H2S and second order with respect to 02. (b) The reaction is fourth order overall. (c) The rate law is: rate = k[H2S}²[O2]. (d) The rate law is: rate = k[H2S][O2]. (e) The rate law cannot be determined from the information given.arrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?arrow_forward5*) a) The reaction A B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of [A] of 0.100 M. What is the initial rate at [A]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)arrow_forward
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