CHEMISTRY:CENTRAL SCI.,V.1-PKG.>CUSTOM<
15th Edition
ISBN: 9781323444535
Author: Brown
Publisher: PEARSON C
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 22.3, Problem 21.3.2PE
Practice Exercise 2
The decomposition of dimethyl ether, (CH3)2O, at 510 ° C is a first-order process with a rate constant of 6.8 × 10-4 s-1:
(CH3)2O(g) → CH4(g) + H2(g) + CO(g)
If the initial pressure of (CH3)2O is 135 torr, what is its pressure after 1420 s?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents 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).
QUESTION 20
The rate constant for the first- order decomposition of N2O is 3.40 s -1 . What is the half- life of the decomposition?
A
0.424 s
B
0.204 s
C
0.491 s
D
0.294 s
E
0.236 s
Consider the reaction:
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(l)
If the rate of formation of N2 is 0.20 Ms-1 at a particular time, what is the rate of disappearance of O2 in molar per second?
please break down math.
Chapter 22 Solutions
CHEMISTRY:CENTRAL SCI.,V.1-PKG.>CUSTOM<
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_forwardQUESTION 16 The first- order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10 -3 s -1 . If the initial concentration of N2O5 is 1.32 M, what is the concentration of N2O5 after 300 seconds? A 0.124 M B 2.82 M C 0.174 M D 0.793 M E 0.355 Marrow_forward
- What are the units of the rate constant, k, in a second- order equation if rate is measured in mol/(L s) and all concentrations are in mol/L? answer options: s–1 L/(mol*s) L2/(mol2*s) mol2/(L2*s)arrow_forwardThe photochemical reaction (i.e., the reaction of hydrogen gas and chlorine gas to produce hydrochloric acid is a zero order reaction. If the concentration of Cl2 gas is 0.029 M at 31.6 seconds, and the rate constant at a certain temperature is 0.00562 M/s, what was the initial concentration of Cl2 gas? (answer in 2 significant figures)arrow_forwardChlorine 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?arrow_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_forwardExperiment. Initial [A]. (mol/L) Initial [B] (mol/L). Disappearance of [A] 1. 0.16. 0.15 0.08 2. 0.16. 0.30. 0.30 3. 0.08. 0.30 0.08 what is the magnitude of the rate constant for the reaction?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
- A solution of a drug was freshly prepared at a concentration of 300 mg/mL. After 30 days at 25°C, the drug concentration in the solution was 75 mg/mL. Assuming first-order kinetics, when will the drug decline to one-half of the original concentration? Assuming zero-order kinetics, when will the drug decline to one-half of the original concentration? Answer #1 = Blank 1 days Answer #2 = Blank 2 daysarrow_forwardPick the letter of the correct answer. 1. Raising the temperature increases the rate of a chemical reaction by increasing ______. a) the frequency of collisions only b) the effectiveness of collisions only c) both the frequency and effectiveness of collisions d) neither the frequency nor the effectiveness of collisions 2. If the rate law of the reaction is rate = k [H2]2[O2]2, what is the order of the reaction? a) zero order b) second order c) third order d) fourth orderarrow_forwardPlease 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…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