Organic Chemistry
6th Edition
ISBN: 9781936221349
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
expand_more
expand_more
format_list_bulleted
Question
Chapter 9, Problem 9.72AP
Interpretation Introduction
Interpretation:
The reason for the fact that the
Concept introduction:
The replacement or substitution of one
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
1 Rate constants for the first-order decomposition of acetonedicarboxylic acid
CO(CH2COOH)2(aq) → CO(CH3)2(aq) + 2 CO2(g)
acetonedicarboxylic acidacetone
are k = 4.75 ×10–4 s–1 at 293 K and k = 1.63 ×10–3 at 303 K. What is the activation energy, Ea, for this reaction?
Select one:
a.
71KJ/mol
b.
81KJ/mol
c.
51KJ/mol
d.
91kJ/mol
(a)
What is the rate equation for the elementary termolecular reaction
2 A + B → products? (Rate expressions take the general form: rate = k . [A]a . [B]b.)
(b)
What is the rate equation for the elementary bimolecular reaction
A + B → products?
The enzyme urease catalyzes the reaction of urea, 1NH2CONH22, with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 * 10-5 s-1 at 100 °C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 * 104 s-1 at 21 °C. (a) Write out the balanced equation for the reaction catalyzed by urease.
Chapter 9 Solutions
Organic Chemistry
Ch. 9 - Prob. 9.1PCh. 9 - Prob. 9.2PCh. 9 - Prob. 9.3PCh. 9 - Prob. 9.4PCh. 9 - Prob. 9.5PCh. 9 - Prob. 9.6PCh. 9 - Prob. 9.7PCh. 9 - Prob. 9.8PCh. 9 - Prob. 9.9PCh. 9 - Prob. 9.10P
Ch. 9 - Prob. 9.11PCh. 9 - Prob. 9.12PCh. 9 - Prob. 9.13PCh. 9 - Prob. 9.14PCh. 9 - Prob. 9.15PCh. 9 - Prob. 9.16PCh. 9 - Prob. 9.17PCh. 9 - Prob. 9.18PCh. 9 - Prob. 9.19PCh. 9 - Prob. 9.20PCh. 9 - Prob. 9.21PCh. 9 - Prob. 9.22PCh. 9 - Prob. 9.23PCh. 9 - Prob. 9.24PCh. 9 - Prob. 9.25PCh. 9 - Prob. 9.26PCh. 9 - Prob. 9.27PCh. 9 - Prob. 9.28PCh. 9 - Prob. 9.29PCh. 9 - Prob. 9.30PCh. 9 - Prob. 9.31PCh. 9 - Prob. 9.32PCh. 9 - Prob. 9.33PCh. 9 - Prob. 9.34PCh. 9 - Prob. 9.35PCh. 9 - Prob. 9.36PCh. 9 - Prob. 9.37PCh. 9 - Prob. 9.38PCh. 9 - Prob. 9.39PCh. 9 - Prob. 9.40PCh. 9 - Prob. 9.41PCh. 9 - Prob. 9.42PCh. 9 - Prob. 9.43PCh. 9 - Prob. 9.44APCh. 9 - Prob. 9.45APCh. 9 - Prob. 9.46APCh. 9 - Prob. 9.47APCh. 9 - Prob. 9.48APCh. 9 - Prob. 9.49APCh. 9 - Prob. 9.50APCh. 9 - Prob. 9.51APCh. 9 - Prob. 9.52APCh. 9 - Prob. 9.53APCh. 9 - Prob. 9.54APCh. 9 - Prob. 9.55APCh. 9 - Prob. 9.56APCh. 9 - Prob. 9.57APCh. 9 - Prob. 9.58APCh. 9 - Prob. 9.59APCh. 9 - Prob. 9.60APCh. 9 - Prob. 9.61APCh. 9 - Prob. 9.62APCh. 9 - Prob. 9.63APCh. 9 - Prob. 9.64APCh. 9 - Prob. 9.65APCh. 9 - Prob. 9.66APCh. 9 - Prob. 9.67APCh. 9 - Prob. 9.68APCh. 9 - Prob. 9.69APCh. 9 - Prob. 9.70APCh. 9 - Prob. 9.71APCh. 9 - Prob. 9.72APCh. 9 - Prob. 9.73APCh. 9 - Prob. 9.74APCh. 9 - Prob. 9.75APCh. 9 - Prob. 9.76APCh. 9 - Prob. 9.77APCh. 9 - Prob. 9.78APCh. 9 - Prob. 9.79APCh. 9 - Prob. 9.80APCh. 9 - Prob. 9.81APCh. 9 - Prob. 9.82APCh. 9 - Prob. 9.83APCh. 9 - Prob. 9.84APCh. 9 - Prob. 9.85APCh. 9 - Prob. 9.86APCh. 9 - Prob. 9.87AP
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
- One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?arrow_forwardThe Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardThe acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.arrow_forward
- Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.arrow_forwardThe rate law for the reaction of phenolphthalein with NaOH was determined to be Rate = k[P2−][OH−]. What are the units on the value of the rate constant, k?arrow_forward(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion.Reactions involving very unstable combinations of chemicals have large rate constants.Concentrations of homogeneous catalysts have no effect on reaction rates.Reaction rate constants are independent of temperature.The slowest step in a reaction is called the rate-determining step.A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.Slow reactions can be speeded up by raising the temperature.arrow_forward
- Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A +B −−→ P and the reactants are initially present in (a) their stoichiometric proportions, (b) with Bpresent initially in twice the amount.arrow_forwardThe equation for the iodination of acetone in acidic solution isCH3 COCH3(aq) + I2(aq) → CH3 COCH2(aq) + H+(aq) + I- (aq) The rate of the reaction is found to be dependent not only on the concentration of the reactants but also on the hydrogen ion centration. Hence the rate expression of this reaction is: rate = k [CH3COCH3]m [I2 ]n [H+]p The rate is obtained by the following the disappearance of iodine using starch as an indicator. The following data are obtained: [CH3COCH3] [H+] [I2] Initial Rate (mol/L.s) 0.80 0.20 0.001 4.2 x 10-6 1.6 0.20 0.001 8.2 x 10-6 0.80 0.40 0.001 8.7 x 10-6 0.80 0.20 0.0005 4.3 x 10-6 1. What is the order of the reaction with respect to each reactant? 2. Write the rate expression for the reaction.3. Calculate, K4. What is the rate of the reaction when [H+]= 0.933 M and [CH3COCH3]= 3[H+]= 10[I-] ?arrow_forwardA second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants? The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C. Evaluate the Arrhenius parameters of the reaction. A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmº mol2 s¹. Calculate the time required for the concentration of A to change from 0.077 mol dm3 to 0.021 mol dm³.arrow_forward
- Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O Sarrow_forwardBenzoyl peroxide (C14H10O4) is widely used in acne treatments. It degrades by 1st-order kinetics and has a half-life of 9.8×103 days at 25 °C.(a) What is the rate constant for this reaction at 25 °C? (b) How many years will it take for 10% of the benzoyl peroxide to degrade?arrow_forwardConsider 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.arrow_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 LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Kinetics: Initial Rates and Integrated Rate Laws; Author: Professor Dave Explains;https://www.youtube.com/watch?v=wYqQCojggyM;License: Standard YouTube License, CC-BY