Chemistry: The Central Science (13th Edition)
13th Edition
ISBN: 9780321910417
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 22.4, Problem 21.4.1PE
Practice Exercise 1
For a certain reaction A → products, a plot of In [A] versus time produces a straight line with a slope of -3.0 × 10-2s-1. Which of the following statements is or are true?
- The reaction follows first-order kinetics.
- The rate constant for the reaction is 3.0 × 10-2 s-1.
- The initial concentration of [A] was 1.0 M.
- Only one of the statements is true.
- Statements (i) and (ii) are true.
- Statements (i) and (iii) are true.
- Statements (ii) and (iii) are true.
- All three statements are true.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
For the given equation at 600 oC:CO(g) + Cl2(g) à COCl2(g), the following data were collected:
Experiment[CO] (M)[Cl2] (M)Rate of appearance COCl2 (M/s)
1 0.24 0.400.121
2 0.48 0.400.241
3 0.24 0.800.483
Determine the Rate Law and the value of the Rate constant (with appropriate units).
Please check!
1.Determine the overall reaction order for the reaction, A+B→2C using the table of data below:
Experiment
Initial [A]/M
Initial [B]/M
Initial rate/M s-1
1
0.010
0.040
0.0031
2
0.010
0.020
0.0015
3
0.020
0.020
0.0032
a. 0
b. 1
c. 2 <-- I think it's this one b/c the numbers are doubled in the table.
d. 3
2. The overall order for the reaction, A+B→C, is 2. A student tests this by measuring the reaction rate at one concentration of A and B, then doubling both concentrations at the same time and re-measuring the rate, which quadrupled. The student concludes that the data support the hypothesis that the above rate law is rate=k[A][B]. Analyze this.
a. The data do support the hypothesis but each trial should be repeated.
b. The data contradict the hypothesis because the rate should have doubled, not quadrupled. <--
c. The data support the hypothesis but a trial holding one reactant constant is needed.
b. The data contradict the hypothesis but testing by…
Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO2(aq) + 2OH–(aq) → ClO2–(aq) + ClO3–(aq) + H2O A kinetic study of this reaction under a certain set of conditions yielded the data below.
Experiment
[ClO2] (M)
[OH-] (M)
Rate (M/s)
1
0.0500
0.100
5.75 x 10-2
2
0.100
0.100
2.30 x 10-1
3
0.100
0.0500
1.15 x 10-1
What is the rate law?
Chapter 22 Solutions
Chemistry: The Central Science (13th Edition)
Ch. 22.1 - Prob. 21.1.1PECh. 22.1 - Prob. 21.1.2PECh. 22.1 - Prob. 21.2.1PECh. 22.1 - Prob. 21.2.2PECh. 22.3 - At 25 ° C, the decomposition of dinitrogen...Ch. 22.3 - Practice Exercise 2 The decomposition of dimethyl...Ch. 22.4 - Practice Exercise 1 For a certain reaction A ...Ch. 22.4 - Prob. 21.4.2PECh. 22.7 - Prob. 21.7.1PECh. 22.7 - Prob. 21.7.2PE
Ch. 22.10 - Prob. 21.10.1PECh. 22.10 - Prob. 21.10.2PECh. 22.10 - Prob. 21.7.1PECh. 22.10 - Prob. 21.7.2PECh. 22 - Prob. 1DECh. 22 - Prob. 1ECh. 22 - Prob. 2ECh. 22 - Prob. 3ECh. 22 - Prob. 4ECh. 22 - The gas-phase reaction CL (g) + HBr (g) + HCl (g)...Ch. 22 - What is the molecularity of each of the following...Ch. 22 - Prob. 7ECh. 22 - Prob. 8ECh. 22 - Cyclopentadiene (C5H6) reacts with itself to form...Ch. 22 - Practice Exercise 1 An Alternative two-step...Ch. 22 - Prob. 11ECh. 22 - Practice Exercise 1
Consider the...Ch. 22 - Prob. 13ECh. 22 - Prob. 14ECh. 22 - Prob. 15ECh. 22 - Prob. 16ECh. 22 - You study the rate of a reaction, measuring both...Ch. 22 - Suppose that for the reaction K+L M, you monitor...Ch. 22 - Prob. 19ECh. 22 - Prob. 20ECh. 22 - Prob. 21ECh. 22 - The following graph shows two different reaction...Ch. 22 - Prob. 23ECh. 22 - Prob. 24ECh. 22 - Prob. 25ECh. 22 - Prob. 26ECh. 22 - Prob. 27ECh. 22 - Prob. 28ECh. 22 - Prob. 29ECh. 22 - Prob. 30ECh. 22 - Prob. 31ECh. 22 - Prob. 32ECh. 22 - Prob. 33ECh. 22 - Prob. 34ECh. 22 - Prob. 35ECh. 22 - Prob. 36ECh. 22 - Prob. 37ECh. 22 - Prob. 38ECh. 22 - Prob. 39ECh. 22 - Prob. 40ECh. 22 - Prob. 41ECh. 22 - Prob. 42ECh. 22 - Prob. 43ECh. 22 - Prob. 44ECh. 22 - Prob. 45ECh. 22 - Prob. 46ECh. 22 - Prob. 47ECh. 22 - Prob. 48ECh. 22 - Prob. 49ECh. 22 - Prob. 50ECh. 22 - Prob. 51ECh. 22 - Prob. 52ECh. 22 - Prob. 53ECh. 22 - Prob. 54ECh. 22 - Prob. 55ECh. 22 - Prob. 56ECh. 22 - Prob. 57ECh. 22 - Prob. 58ECh. 22 - Prob. 59ECh. 22 - Prob. 60ECh. 22 - Prob. 61ECh. 22 - Prob. 62ECh. 22 - Prob. 63ECh. 22 - Prob. 64ECh. 22 - Prob. 65ECh. 22 - Prob. 66ECh. 22 - Prob. 67ECh. 22 - Prob. 68ECh. 22 - Prob. 69ECh. 22 - Prob. 70ECh. 22 - Prob. 71ECh. 22 - Prob. 72ECh. 22 - Prob. 73ECh. 22 - Prob. 74ECh. 22 - Prob. 75ECh. 22 - Prob. 76ECh. 22 - Prob. 77ECh. 22 - Prob. 78ECh. 22 - Prob. 79ECh. 22 - Prob. 80ECh. 22 - Prob. 81AECh. 22 - Prob. 82AECh. 22 - Prob. 83AECh. 22 - Prob. 84AECh. 22 - Prob. 85AECh. 22 - Prob. 86AECh. 22 - Prob. 87AECh. 22 - Prob. 88AECh. 22 - Prob. 89AECh. 22 - Prob. 90AECh. 22 - Prob. 91AECh. 22 - Prob. 92IECh. 22 - Prob. 93IECh. 22 - Prob. 94IECh. 22 - Prob. 95IECh. 22 - Prob. 96IECh. 22 - Prob. 97IECh. 22 - Prob. 98IECh. 22 - Prob. 99IECh. 22 - Prob. 100IECh. 22 - Prob. 101IECh. 22 - Prob. 102IECh. 22 - Prob. 103IECh. 22 - Prob. 104IECh. 22 - Prob. 105IECh. 22 - Prob. 106IECh. 22 - Prob. 107IE
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
- The iodide-ion-catalyzed decomposition of hydrogen peroxide, H2O2, is believed to follow the mechanism H2O2+Ik1H2O+IO(slow)H2O2+IOk2H2O+O2+I(fast) What rate law is predicted by this mechanism? Explain.arrow_forwardA reaction believed to be either first or second order has a half-life of 20 s at the beginning of the reaction but a half-life of 40 s sometime later. What is the order of the reaction?arrow_forwardConsider the following potential-energy curves for two different reactions: a. Which reaction has a higher activation energy for the forward reaction? b. If both reactions were run at the same temperature and have the same orientation requirements to react, which one would have the larger rate constant? c. Are these reactions exothermic or endothermic?arrow_forward
- Acetaldehyde, CH3CHO, decomposes when heated. CH3CHO(g)CH4(g)+CO(g) The rate constant for the decomposition is 1.05 103/(M1/2 s)at 759 K and 2.14 102/(M1/2 s) at 836 K. What is the activation energy for this decomposition? What is the rate constant at 865 K?arrow_forwardConsider the following reaction and the experimental data in the table below.2 ??(?) + ?2(?) → 2 ??2(?)Experiment [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.10 0.10 0.18 2 0.10 0.20 0.35 3 0.20 0.20 1.42Calculate the rate of the reaction when [NO] = 0.35 M and [O2] = 0.65 Marrow_forwardExperiment number [A](M) [B](M) Initial Rate (M/s) 1 0.451 0.885 1.13 2 0.451 1.77 1.13 3 1.35 0.885 10.17 What is the order of the reaction in A?arrow_forward
- Exercises20A.1(a) Predict how the total pressure varies during the gas-phase reaction2 ICl(g)+H2(g)→I2(g)+2 HCl(g) in a constant-volume container.20A.1(b) Predict how the total pressure varies during the gas-phase reactionN2(g)+3 H2(g)→2 NH3(g) in a constant-volume container.20A.2(a) The rate of the reaction A+2 B→3 C+D was reported as2.7moldm−3 s−1. State the rates of formation and consumption of theparticipants.20A.2(b) The rate of the reaction A+3 B→C+2 D was reported as2.7moldm−3 s−1. State the rates of formation and consumption of theparticipants.20A.3(a) The rate of formation of C in the reaction 2 A+B→2 C+3 Dis 2.7moldm−3 s−1. State the reaction rate, and the rates of formation orconsumption of A, B, and D.20A.3(b) The rate of consumption of B in the reaction A+3 B→C+2 Dis 2.7moldm−3 s−1. State the reaction rate, and the rates of formation orconsumption of A, C, and D.20A.4(a) The rate law for the reaction in Exercise 20A.2(a) was found to bev=kr[A][B]. What are the units of kr…arrow_forwardExperiment Initial [Br–] (M) Initial [BrO3–] (M) Initial [H+] (M) Rate of Disappearance of BrO3– (M s-1) 1 0.00100 0.00500 0.100 2.50x10-4 2 0.00200 0.00500 0.100 5.00x10-4 3 0.00100 0.00750 0.100 3.75x10-4 4 0.00100 0.01500 0.200 3.00x10-3 Determine the order of the reaction for [H+]arrow_forwardA chemical reaction has a rate constant value of 15.8 M-1·hr-1 at 175.0°C and an activation energy of 55.0 kJ/mol. How many degrees Celsius must the temperature be increased in order for the reaction rate to increase by a factor of 5.0?Answer °C increase in temperaturearrow_forward
- Consider the reaction to produce a block co-polymer below. A and B are different monomers. For example A could be limonene and B could be styrene. 2A + 3B → products If the rate law for the reaction is first order in A and second order in B, which of the following is the rate law for the reaction? Question 4 options: Rate = k[A][B] Rate = k[A]2[B]3 Rate = k[A][B]2 Rate = k[A]2[B] Rate = k[A]2[B]2arrow_forwardWhat is the half-life of this reaction. calculate the value of the rate constant K. predict the concentration of Cl2O5 in the engineers reaction vessel after .210 seconds have passed. Please round for answers only. 2 sig figs. Please check work. Thank youarrow_forwardIssue 5The data in the table below was compiled for the following reaction. A + B → C + D At temperature T, the following initial velocity data was obtained. Experience [A] (mol/L) [B] (mol/L) Initial speed (mol/L s) 1 0,020 0,020 5,0 x 10-3 2 0,040 0,020 1,0 x 10-2 3 0,040 0,060 4,5 x 10-2 Determine the rate law equation and the rate constant at temperature T with the appropriate units.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
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