CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
14th Edition
ISBN: 9780134863016
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 14.6, Problem 14.13.1PE
Practice Exercise 1
Consider the following reaction: 2 A+ B→ X + 2 Y. you are told that the first step in the mechanism of this reaction has the following rate law: Rate Rate = k[A][B]. which of the following could be the first step in the reaction mechanism (note that substances Z is an intermediate)?
- A + A → Y+ Z
- A → X + Z
- A + A + B → X + Y + Y
- B → X + Y
- A + B → X + Z
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Question 13 of 32
Using the information in the table, the rate law for the reaction 2 A(g) + B(g) →
C(g) + D(g) is
Rate
[A], (M)
[B], (M)
(M/s)
A) Rate = k[A][B]
0.100
2.50
0.460
B) Rate = k[B]
C) Rate = k[A]°[B]
0.200
2.50
0.920
D) Rate = k[A]
0.300
1.25
1.38
"pe here to search
View Policies
Current Attempt in Progress
The decomposition of ozone, O3, is believed to occur by the two-step mechanism
O3→ 02 + O
(slow)
O+ O3→ 202 (fast)
203 → 302
(net reaction)
If this is the mechanism, what is the reaction's rate law?
Rate = k[O][O3]
O Rate = k[O2]²
Rate = k[O3]
O Rate = k[O][O2]
O Rate = k[O3]2
O Rate = k[O2]3
%3D
%3D
O None of these or more informtion is required.
eTextbook and Media
Step 1
Step 2
What is the rate law for the proposed mechanism?
H₂(g) + 2NO(g) N₂O(g) + H₂O(g)
(slow)
4
N₂O(g) + H₂(g) → N₂(g) + H₂O(g)
(fast)
A) rate k[H₂][NO]
B) rate= K[H₂]³[NO]
C) rate= K[H₂][NO].
D) rate= K[H₂][NO]
E) rate k[H₂][N₂O]
=
Chapter 14 Solutions
CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
Ch. 14.2 - If the experiment in Figure 14.2 is run for 60 s,...Ch. 14.2 - Prob. 14.1.2PECh. 14.2 - Which of the following could be the instantaneous...Ch. 14.2 - Using Figure 14.3, determine the instantaneous...Ch. 14.2 - At a certain time in a reaction, substance A is...Ch. 14.2 - Prob. 14.3.2PECh. 14.3 - Suppose the rate law for the reaction in this...Ch. 14.3 - Assuming that rate = k[A][B], rank the mixtures...Ch. 14.3 - Prob. 14.5.1PECh. 14.3 - Prob. 14.5.2PE
Ch. 14.3 - Consider the reaction examined above in the Sample...Ch. 14.3 - The following data were measured for the reaction...Ch. 14.4 - At 25 ° C, the decomposition of dinitrogen...Ch. 14.4 - Practice Exercise 2 The decomposition of dimethyl...Ch. 14.4 - Practice Exercise 1 For a certain reaction A ...Ch. 14.4 - Prob. 14.8.2PECh. 14.4 - Practice Exercise 1 We noted in an earlier...Ch. 14.4 - Practice Exercise 2 Using Equation 14.17,...Ch. 14.5 - Practice Exercise 1 This of the following change...Ch. 14.5 - Practice Exercise 2 Rank the rate constants of the...Ch. 14.5 - Practice Exercise 1 Using the data in Sample...Ch. 14.5 - Practice Exercise 2 To one significant figure,...Ch. 14.6 - Practice Exercise 1 Consider the following...Ch. 14.6 - For the reaction Mo(CO)6 +P(CH3)3 Mo(CO)5P(CH3)3...Ch. 14.6 - Practice Exercise 1 Consider the following...Ch. 14.6 - Practice Exercise 2 Consider the following...Ch. 14.6 - Practice Exercise 1 An Alternative two-step...Ch. 14.6 - Prob. 14.14.2PECh. 14.6 - Practice Exercise 1
Consider the...Ch. 14.6 - Prob. 14.15.2PECh. 14 - Prob. 1DECh. 14 - An automotive fuel injector dispenses a fine spray...Ch. 14 - Consider the following graph of the concentration...Ch. 14 - You study the rate of a reaction, measuring both...Ch. 14 - Suppose that for the reaction K+L M, you monitor...Ch. 14 - Prob. 5ECh. 14 - A friend studies a first-order reaction and...Ch. 14 - Prob. 7ECh. 14 - Which of the following linear plots do you expect...Ch. 14 - Prob. 9ECh. 14 - Prob. 10ECh. 14 - The following graph shows two different reaction...Ch. 14 - Prob. 12ECh. 14 - Prob. 13ECh. 14 - Draw a possible transition state for the...Ch. 14 - The following diagram represents an imaginary...Ch. 14 - 14.16 Draw a graph showing the reaction pathway...Ch. 14 - Prob. 17ECh. 14 - 14.18 (a) what are the units usually used to...Ch. 14 - Prob. 19ECh. 14 - A flask is charged with 0.100 mol of A and allowed...Ch. 14 - The isomerization of methyl isontrile (CH3NC) to...Ch. 14 - Prob. 22ECh. 14 - Prob. 23ECh. 14 - For each of the following gas-phase reactions,...Ch. 14 - (a) Consider the combustion of hydrogen, 2H2 (g) +...Ch. 14 - Prob. 26ECh. 14 - A reaction A+B C obeys the following rate law:...Ch. 14 - Prob. 28ECh. 14 - 14.29 The decomposition reaction of N2O5 in carbon...Ch. 14 - Prob. 30ECh. 14 - Prob. 31ECh. 14 - The reaction between ethyl bromide (C2H5Br) and...Ch. 14 - Prob. 33ECh. 14 - The reaction 2ClO2 (aq) + 2OH- (aq) ClO3- (aq) +...Ch. 14 - The following data were measured for the reaction...Ch. 14 - The following data were collected for the rate of...Ch. 14 - Consider the gas-phase reaction between nitric...Ch. 14 - Prob. 38ECh. 14 - Prob. 39ECh. 14 - Prob. 40ECh. 14 - Prob. 41ECh. 14 - Molecular iodine, I2 (g), dissociates into iodine...Ch. 14 - Prob. 43ECh. 14 - Prob. 44ECh. 14 - The reaction SO2Cl2 (g) O2 (g) + Cl2 (g) is first...Ch. 14 - Prob. 46ECh. 14 - Prob. 47ECh. 14 - Prob. 48ECh. 14 - Prob. 49ECh. 14 - Prob. 50ECh. 14 - (a) what factors determine whether a collision...Ch. 14 - (a) in which of the following reactions you expect...Ch. 14 - Calculate the fraction of atoms in a sample of...Ch. 14 - (a) the activation energy for the isomerization of...Ch. 14 - The gas-phase reaction CL (g) + HBr (g) + HCl (g)...Ch. 14 - Prob. 56ECh. 14 - Indicate whether each statement is true or false....Ch. 14 - Indicate whether each statement is true or false....Ch. 14 - Based on their activation energies and energy...Ch. 14 - Prob. 60ECh. 14 - Prob. 61ECh. 14 - Prob. 62ECh. 14 - The rate of the reaction CH3COOC2H5 (aq) + OH- ...Ch. 14 - Prob. 64ECh. 14 - Prob. 65ECh. 14 - Prob. 66ECh. 14 - What is the molecularity of each of the following...Ch. 14 - Prob. 68ECh. 14 - (a) based on the following reaction profile, how...Ch. 14 - Prob. 70ECh. 14 - Prob. 71ECh. 14 - Prob. 72ECh. 14 - The reaction 2NO (g) + CL2 (g) 2NOCl (g) was...Ch. 14 - You have studied the gas-phase oxidation of HBr by...Ch. 14 - Prob. 75ECh. 14 - Prob. 76ECh. 14 - Prob. 77ECh. 14 - Prob. 78ECh. 14 - Prob. 79ECh. 14 - The addition of No accelerates the decomposition...Ch. 14 - 14.81b Many metallic catalysts, particularly the...Ch. 14 - Prob. 82ECh. 14 - When D2 reacts with ethylene (C2H4) in the...Ch. 14 - Prob. 84ECh. 14 - Prob. 85ECh. 14 - The enzyme urease catalyzez the reaction of urea,(...Ch. 14 - Prob. 87ECh. 14 - Prob. 88ECh. 14 - Prob. 89AECh. 14 - Prob. 90AECh. 14 - Prob. 91AECh. 14 - Prob. 92AECh. 14 - Prob. 93AECh. 14 - Prob. 94AECh. 14 - Prob. 95AECh. 14 - Prob. 96AECh. 14 - [14.97]A first order reaction A B has the rate...Ch. 14 - Prob. 98AECh. 14 - Prob. 99AECh. 14 - Prob. 100AECh. 14 - Prob. 101AECh. 14 - Prob. 102AECh. 14 - Cyclopentadiene (C5H6) reacts with itself to form...Ch. 14 - Prob. 104AECh. 14 - At 280C, raw milk sours in 4.0 h but takes 48 h to...Ch. 14 - Prob. 106AECh. 14 - Prob. 107AECh. 14 - Prob. 108AECh. 14 - Prob. 109AECh. 14 - The following mechanism has been proposed for the...Ch. 14 - Prob. 111AECh. 14 - Prob. 112AECh. 14 - Platinum nanoparticles of diameter ~2 nm are...Ch. 14 - 14.114 One of the many remarkable enzymes in the...Ch. 14 - 14.115N Suppose that, in the absence of catalyst,...Ch. 14 - Prob. 116AECh. 14 - Dinitrogen pentoxide (N2O5) decomposes in...Ch. 14 - The reaction between ethyl iodide and hydroxide...Ch. 14 - Prob. 119IECh. 14 - Prob. 120IECh. 14 - Prob. 121IECh. 14 - The rates of many atmospheric reactions are...Ch. 14 - Prob. 123IECh. 14 - Prob. 124IECh. 14 - Prob. 125IE
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
- rate = k[CH3CI]2[(H2O] %3D Question 43 The reaction A+ 2B → products was found to be first-order to A and second- order to B. While holding the concentration of A constant, the concentration of B is increased to 10 times its initial value. By what factor does the rate of reaction increase? Please report an integer, without unit. Question 44arrow_forwardQUESTION 18 A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 A Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] B Rate = 36 M-1s-1 [S2O82⁻][I⁻] C Rate = 86 M-2s-1 [S2O82⁻][I⁻] D Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] E Rate = 120 M-2s-1 [S2O82⁻]2[I⁻]arrow_forwardWhat is the correct rate law for the following reaction? * A + 5B + 6C → 3D + 3E Experiment 1 2 3 4 Option 1 rate = [A] (M) Option 3 0.35 0.70 0.70 0.70 [B] (M) 0.35 0.35 rate = k[A] [B] [C] 0.70 0.35 k [A]² [B] [C] (M) Initial Rate (M/s) 0.35 8.0 x 10-4 3.2 x 10-3 6.4 x 10-3 3.2 x 10-3 0.35 0.35 0.70 rate = Option 2 k [A] [B]² [C] rate = k [A] [B]² [C] Option 4arrow_forward
- Question 11 of 26 Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) –→ C(g) + 2 D(g) is Rate [A], (M) [B], (M) (M/min) A) 13.4 M3 min1 0.300 0.180 0.0234 B) 0.13 min1 C) 0.259 min1 0.300 0.360 0.0934 D) 0.26 M'min1 0.150 0.180 0.0234 E) 0.722 M'min1 Sho age2.pdf bank SelfCert dis....pdf A SelfCert.pdf PromNote.pdfarrow_forwardThe table shown below contains concentration and rate data for this reaction A + 2B ---> C Determine the rate law for this reaction. Experiment Initial [A] Initial [B] Initial Rate 1 0.23 0.17 0.33 2 0.46 0.17 2.64 3 0.23 0.51 0.33 Group of answer choices a) R = k[A]4 b) R = k[A]3[B] c) Rate = k[A]3 d) R = k[A]4[B]arrow_forwardWhich of the choices below properly express the rate of the following reaction? CH4(g) + 20,(g) → CO2(g) + 2H,O(g) Check all that apply. 1A[02] F) rate = A[CH4] A[H,O] A) rate K) rate = At 2 At At A[CH4] A[CO2] A[H,0] B) rate = G) rate L) rate = 2- At At At A[02] C) rate = -2- At A[CO2] H) rate = At A[O2] 1 A[H,O] D) rate = I) rate At At 1 4[02] 2 At 1 A[H,O] E) rate = J) rate = Atarrow_forward
- 3:17 Question 15 of 15 A) Rate = 0.25 M-¹ s¯¹[A] What is the rate law for the reaction A → Bif the rate constant, k, is 0.25 M¹s¹ at 75 °C? B) Rate = 0.25 M-¹ s¹[A]² C) Rate = 4.0 M-¹ s¯¹[A]² D) Rate = 0.25 M-¹ s¹[B] E) Rate = 0.25 M₁¹ s¹[B]² ..5GW Tap here or pull up for additional resources Submitarrow_forwardCHAP 14 EXERCISES 6 & 7 • iven the initial rate data for the reaction A + B –→ C, determine the rate expression for the reaction. The reaction is catalyzed by the molecule D. [A]. M 0.10 [B]. M [D]. M 0.10 A[CJ/At (mol/L•s) 0.20 2.58 0.10 0.10 0.10 1.29 0.24 0.10 0.10 0.20 2.58 0.20 0.20 5.16 Data values are given at 660 K for the reaction 2NO(g) + O2(g)→ 2NO2(g) What is the rate law for the reaction? Reactant concentrations (mol/L) Rate of Disappearance of NO (mol/L•sec) [NO] [O2] 0.020 0.010 1.0х 104 0.040 0.010 4.0 x 10-4 0.020 0.040 4.0 x 10-4 50arrow_forwardNitrosyl chloride is produced from the reaction of nitrogen(II)oxide and chlorine. 2 NO(g) + Cl2(g) 2 NOCI(g) The following initial rates at a given temperature were obtained for the concentrations given below: Experiment 1 2 3 What is the Rate Law? Rate (mol/L.hr). 2.21 8.83 17.5 NO (mol/L) 0.25 0.50 0.50 Cl₂_(mol/L) 0.25 0.25 0.50arrow_forward
- Consider the reaction below: A → products Using a spectrophotometer, the concentration of A as a function of time is measured. If a plot of 1/[A] vs. t is linear, what can be concluded regarding the reaction? Question 6 options: A) Rate = k B) Rate = k[A] C) Rate = k[A]2 D) No conclusion can be made since the temperature was not varied during the experiment.arrow_forwardIf the reaction X + 2 Y → XY, occurs by the proposed mechanism, what is the rate 2 law? Step 1 X + Y= XY (slow) Step 2 XY + Y → XY2 (fast) A) rate = k[X] B) rate = k[Y] C) rate = k[Y]? D) rate = k[X][Y] E) rate = k[X][Y]?arrow_forwardDetermine the rate law for the following reaction using the experimental data given below. 2NO+ O2 →→→→→→→ 2NO2 Experiment 1 2 3 O rate=k[NO][0₂] O rate=k[NO]²[0₂] rate=k[NO]²[0₂]² rate=k[NO]²[0₂]³ O rate=k[NO]4[0₂]³ [NO] (M) 0.0503 0.0247 0.0503 [0₂] (M) 0.0202 0.0202 0.0609 Rate (M/s) 0.355 0.0888 1.07arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
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