Connect 1-semester Access Card For Chemistry
4th Edition
ISBN: 9781259636936
Author: Julia Burdge
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 14.4, Problem 1PPB
Practice ProblemBUILD
Refer again to the reaction
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
II. Instruction: Writing the Reaction Quotient and Finding K for an Overall Reaction
2. The following sequence of steps has been proposed for the overall reaction between H2 and Br2 to form HBr:
(1) Br2(g) ↔ 2Br(g)
(2) Br (g) + H2(g) ↔HBr (g) + H(g)
(3) H (g) + Br (g) ↔HBr(g)
Write the overall balanced equation and show that the overall Qc is the product of the Qc expressions for the individual steps.
II. Instruction: Writing the Reaction Quotient and Finding K for an Overall Reaction
Nitrogen dioxide is a toxic pollutant that contributes to photochemical smog. One way it forms is through the following sequence:
(1) N2(g) + O2(g) ↔ 2NO(g) Kc1 5 4.3x1025
(2) 2NO(g) + O2(g) ↔ 2NO2(g) Kc2 5 6.4x109
(a) Show that the overall Qc for this reaction sequence is the same as the product of the Qc expressions for the individual reactions.
(b) Given that both reactions occur at the same temperature, find Kc for the overall reaction.
Which of the following is a concerted reaction with a ΔG < 0? (Hint: Exergonic reaction)
Chapter 14 Solutions
Connect 1-semester Access Card For 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...
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
- A chemical equilibrium A ⇄ 2B has a forward rate constant, kf = 12 M –1 s–1, and a reverse rate constant, kr = 18 s–1. If the system has a concentration of [A] = 0.15 M at equilibrium, what is the concentration of B at equilibrium? (no scientific notation)arrow_forwardAt 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g) is 2.25 × 10−4. If [H2S] = 4.80 × 10−3 M and [H2] = 1.40 × 10−3 M, calculate [S2]. Please write to text formet answerarrow_forwardChemistry 13. a) Challenge problem. Nitric oxide gas reacts with bromine gas to form nitrosyl bromide gas. 3NO(g) -> N2O(g) + NO2(g) As 25C, the equilibrium concentrations of dinitrogen monoxide and nitrogen dioxide are 0.170 M and 0.250 M, respectively. A)Using thermodynamic data from the cover sheet, calculate the equilibrium concentration of nitric oxide b) You add 0.75 mL of 0.175 M sodium hydroxide to 10.00 mL 0.108 M hypobromous acid. Calculate the pH of the resulting solution. Ka of hypobromous is 2.8 * 10 ^-9arrow_forward
- A chemical equilibrium 2 A ⇄ 2B has a forward rate constant, kf = 8 M –1 s–1, and a reverse rate constant, kr = 22 s–1. If the system has a concentration of [A] = 0.22 M at equilibrium, what is the concentration of B at equilibrium? (can't be in scientific notation)arrow_forwardplease answer fast! Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AIC13 to form methylcyclopentane (MCP) according to the equation: C_{6}*H_{12} = MCP If K_{C} = 0.143 at 25°C for this reaction, predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.200 M and 0.100 M, respectively. The system A) will shift right B) will shift left. C) is already at equilibrium. D) is not at equilibrium and will remain in an unequilibrated state.arrow_forwardThe Kp for the reaction A (g) ⇌ 2 B (g) is 0.0730. What is Kp for the reaction 4 B (g) ⇌ 2 A (g)? Answer numericla ______arrow_forward
- Solve all part please. Consider the equilibrium reaction N2O4 (g) ⇌ 2 NO2 (g)a. Using appendix C, find H and S for this reaction (you will need this for b,c). delta s= 176.6J delta H=5802kJb. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PNO2 = PN2O4 = 1.0 atm.c. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PT = 10.0 atm and PNO2 = 2 PN2O4.arrow_forwardII. Instruction: Writing the Reaction Quotient and Finding K for an Overall Reaction 3. Given the following reaction sequence, write the overall balanced equation and show that the overall Qc is the product of the Qc expressions for the individual steps: (1) H2(g) + ICl(g) ↔ HI(g) +HCl(g) (2) HI(g) + ICl(g) ↔ I2(g) +HCl(g)arrow_forwardQUESTION 5 Consider the reaction below at 100oC. T2U (g) -> 2 T (g) + U (g) If given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed? A. 0.486 M B. 0.243 M C. 0.00724 M D. 0.121 Marrow_forward
- At a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N2O4 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium? (no scientific notation)N2O4(g) ⇄ 2NO2(g)arrow_forwardBe sure to answer all parts. The minerals hematite (Fe2O3) and magnetite (Fe3O4) exist in equilibrium with atmospheric oxygen: 4 Fe3O4(s) + O2(g) ⇌ 6 Fe2O3(s) Kp = 2.5 ×1087 at 298 K a) Determine PO2 at equilibriium (b) Given that PO2 in air is 0.21 atm, in which direction will the reaction proceed to reach equilibrium? toward reactants no change toward productsarrow_forwardWhich of the following are intermediates in the following reaction? (Select all that apply)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: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY