Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Question
Chapter 11, Problem 19QRT
(a)
Interpretation Introduction
Interpretation:
The change in rate has to be explained after changing the reactant concentration.
Concept Introduction:
The relationship between rate and initial concentration of reactant is described by rate law.
Where,
(b)
Interpretation Introduction
Interpretation:
The change in rate has to be explained after changing the reactant concentration.
Concept Introduction:
The relationship between rate and initial concentration of reactant is described by rate law.
Where,
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
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 reaction A + B ¡ C + D. Is each of the following statements true or false? (a) The rate law for the reaction must be Rate = k3A43B4. (b) If the reaction is an elementary reaction, the rate law is second order. (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order. (d) The activation energy for the reverse reaction must be greater than that for the forward reaction.
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) 5.72×10‒6
Chapter 11 Solutions
Chemistry: The Molecular Science
Ch. 11.1 - For the reaction of crystal violet with NaOH(aq),...Ch. 11.1 - (a) From data in Table 11.1, calculate the rate of...Ch. 11.1 - For the reaction 4NO2(g)+O2(g)2N2O5(g) (a) express...Ch. 11.1 - Instantaneous rates for the reaction of hydroxide...Ch. 11.1 - Prob. 11.3CECh. 11.2 - Prob. 11.4ECh. 11.2 - Prob. 11.3PSPCh. 11.2 - Prob. 11.5ECh. 11.3 - Prob. 11.4PSPCh. 11.3 - Prob. 11.5PSP
Ch. 11.3 - Prob. 11.6PSPCh. 11.3 - Prob. 11.7PSPCh. 11.4 - Prob. 11.6ECh. 11.4 - Prob. 11.7CECh. 11.4 - Prob. 11.8PSPCh. 11.4 - Prob. 11.8CECh. 11.5 - Prob. 11.9PSPCh. 11.5 - The frequency factor A is 6.31 108 L mol1 s1 and...Ch. 11.6 - Prob. 11.10CECh. 11.7 - Prob. 11.11ECh. 11.7 - The Raschig reaction produces the industrially...Ch. 11.7 - Prob. 11.12ECh. 11.8 - The oxidation of thallium(I) ion by cerium(IV) ion...Ch. 11.9 - Prob. 11.11PSPCh. 11.9 - Prob. 11.14CECh. 11 - An excellent way to make highly pure nickel metal...Ch. 11 - Prob. 1QRTCh. 11 - Prob. 2QRTCh. 11 - Prob. 3QRTCh. 11 - Prob. 4QRTCh. 11 - Prob. 5QRTCh. 11 - Prob. 6QRTCh. 11 - Prob. 7QRTCh. 11 - Prob. 8QRTCh. 11 - Prob. 9QRTCh. 11 - Prob. 10QRTCh. 11 - Prob. 11QRTCh. 11 - Cyclobutane can decompose to form ethylene:
The...Ch. 11 - Prob. 13QRTCh. 11 - Prob. 14QRTCh. 11 - For the reaction 2NO2(g)2NO(g)+O2(g) make...Ch. 11 - Prob. 16QRTCh. 11 - Prob. 17QRTCh. 11 - Ammonia is produced by the reaction between...Ch. 11 - Prob. 19QRTCh. 11 - Prob. 20QRTCh. 11 - The reaction of CO(g) + NO2(g) is second-order in...Ch. 11 - Nitrosyl bromide, NOBr, is formed from NO and Br2....Ch. 11 - Prob. 23QRTCh. 11 - Prob. 24QRTCh. 11 - Prob. 25QRTCh. 11 - For the reaction
these data were obtained at 1100...Ch. 11 - Prob. 27QRTCh. 11 - Prob. 28QRTCh. 11 - Prob. 29QRTCh. 11 - Prob. 30QRTCh. 11 - Prob. 31QRTCh. 11 - Prob. 32QRTCh. 11 - For the reaction of phenyl acetate with water the...Ch. 11 - When phenacyl bromide and pyridine are both...Ch. 11 - The compound p-methoxybenzonitrile N-oxide, which...Ch. 11 - Prob. 36QRTCh. 11 - Radioactive gold-198 is used in the diagnosis of...Ch. 11 - Prob. 38QRTCh. 11 - Prob. 39QRTCh. 11 - Prob. 40QRTCh. 11 - Prob. 41QRTCh. 11 - Prob. 42QRTCh. 11 - Prob. 43QRTCh. 11 - Prob. 44QRTCh. 11 - Prob. 45QRTCh. 11 - Prob. 46QRTCh. 11 - Prob. 47QRTCh. 11 - Prob. 48QRTCh. 11 - Prob. 49QRTCh. 11 - Prob. 50QRTCh. 11 - Prob. 51QRTCh. 11 - Prob. 52QRTCh. 11 - For the reaction of iodine atoms with hydrogen...Ch. 11 - Prob. 54QRTCh. 11 - The activation energy Ea is 139.7 kJ mol1 for the...Ch. 11 - Prob. 56QRTCh. 11 - Prob. 57QRTCh. 11 - Prob. 58QRTCh. 11 - Prob. 59QRTCh. 11 - Prob. 60QRTCh. 11 - Prob. 61QRTCh. 11 - Prob. 62QRTCh. 11 - Prob. 63QRTCh. 11 - Which of the reactions in Question 62 would (a)...Ch. 11 - Prob. 65QRTCh. 11 - Prob. 66QRTCh. 11 - Prob. 67QRTCh. 11 - Prob. 68QRTCh. 11 - Prob. 69QRTCh. 11 - Prob. 70QRTCh. 11 - Prob. 71QRTCh. 11 - For the reaction the rate law is Rate=k[(CH3)3CBr]...Ch. 11 - Prob. 73QRTCh. 11 - Prob. 74QRTCh. 11 - Prob. 75QRTCh. 11 - For this reaction mechanism,
write the chemical...Ch. 11 - Prob. 77QRTCh. 11 - Prob. 78QRTCh. 11 - Prob. 79QRTCh. 11 - When enzymes are present at very low...Ch. 11 - Prob. 81QRTCh. 11 - The reaction is catalyzed by the enzyme succinate...Ch. 11 - Prob. 83QRTCh. 11 - Many biochemical reactions are catalyzed by acids....Ch. 11 - Prob. 85QRTCh. 11 - Prob. 86QRTCh. 11 - Prob. 87QRTCh. 11 - Prob. 88QRTCh. 11 - Prob. 89QRTCh. 11 - Prob. 90QRTCh. 11 - Prob. 91QRTCh. 11 - Prob. 92QRTCh. 11 - Prob. 93QRTCh. 11 - Prob. 94QRTCh. 11 - Nitryl fluoride is an explosive compound that can...Ch. 11 - Prob. 96QRTCh. 11 - Prob. 97QRTCh. 11 - For a reaction involving the decomposition of a...Ch. 11 - Prob. 99QRTCh. 11 - Prob. 100QRTCh. 11 - Prob. 101QRTCh. 11 - This graph shows the change in concentration as a...Ch. 11 - Prob. 103QRTCh. 11 - Prob. 104QRTCh. 11 - Prob. 105QRTCh. 11 - Prob. 106QRTCh. 11 - Prob. 107QRTCh. 11 - Prob. 108QRTCh. 11 - Prob. 109QRTCh. 11 - Prob. 110QRTCh. 11 - Prob. 111QRTCh. 11 - Prob. 112QRTCh. 11 - Prob. 113QRTCh. 11 - Prob. 114QRTCh. 11 - Prob. 115QRTCh. 11 - Prob. 116QRTCh. 11 - Prob. 118QRTCh. 11 - Prob. 119QRTCh. 11 - In a time-resolved picosecond spectroscopy...Ch. 11 - If you know some calculus, derive the integrated...Ch. 11 - If you know some calculus, derive the integrated...Ch. 11 - (Section 11-5) A rule of thumb is that for a...Ch. 11 - Prob. 11.BCPCh. 11 - Prob. 11.CCPCh. 11 - Prob. 11.DCP
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 following kinetic data are collected for the initial rates of a reaction 2 X + Z→ products: Experiment [X ]o(M) [Z]o(M) Rate (M/s) 0.25 0.25 4.0 x 10! 0.50 0.50 3.2 x 102 0.50 0.75 7.2 x 102 (a) What is the rate law for this reaction? (b) What is the value of the rate constant with proper units? (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M? 2. 3.arrow_forward(a) For a reaction A + B —> P, the rate is given by Rate = k[A]2 [B](i) How is the rate of reaction affected if the concentration of A is doubled?(ii) What is the overall order of reaction if B is present in large excess?(b) A first order reaction takes 23.1 minutes for 50% completion. Calculate the time required for 75% completion of this reaction.(Given: log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)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 reaction?(b) Write the unit of rate constat ‘k’ for the first order reaction.arrow_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_forwardConsider the following reaction: O2(g) + 2 NO(g) 2 NO2(g)(a) The rate law for this reaction is first order in O2(g) and second order in NO(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 7840, what is the reaction rate when [O2(g)] = 0.0162 M and [NO(g)] = 0.0299 M?Rate = _____ M/s.(c) What is the reaction rate when the concentration of O2(g) is doubled, to 0.0324 M while the concentration of NO(g) is 0.0299 M?Rate = _____ M/sarrow_forwardThe decomposition of XY is second order in XY and has a rate constant of 7.41 × 10−3 L·mol−1·s−1 at a certain temperature, the half-life for this reaction at an initial concentration of 0.101 mol·L−1 1336. A) If the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?, B) If the initial concentration of XY is 0.080 mol·L−1, what is the concentration of XY after 75 s ?arrow_forward
- Consider 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_forwardConsider 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/sarrow_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_forward
- Consider 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_forwardConsider 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.arrow_forwardConsider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(9)] (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂05(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/sarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
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