Bundle: Physical Chemistry, 2nd + Student Solutions Manual
2nd Edition
ISBN: 9781285257594
Author: David W. Ball
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 20, Problem 20.84E
Interpretation Introduction
Interpretation:
The value of the
Concept introduction:
The Michaelis-Menten kinetics is given by the expression as shown below.
Where,
•
•
•
•
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
For the following reaction C2H5Br + KOH C2H5OH + KBr
it is determined that doubling the C2H5Br concentration causes the rate to double, what is the order with respect to C2H5Br? It is also determined that doubling the KOH concentration has no effect on the rate, what is the order with respect to KOH? Write the rate law expression for this reaction. What would the units for k be if time was expressed in units of seconds?
Determine the rate law and the value of k for the following reaction using the data provided:
[S2O82-]
[I-]
Initial Rate (M/s)
0.30
0.42
3.38
0.62
0.42
6.65
0.62
0.21
3.33
Rate = 36 [S2O82⁻] [I⁻]
Rate = 23 [S2O82⁻] [I⁻]1/2
Rate = 120 [S2O82⁻]2 [I⁻]
Rate = 86 [S2O82⁻] [I⁻] 2
Rate = 195 [S2O82⁻]2 [I⁻]2
S2O82- + 3I- → 2 SO42- + I3-
The rate of a reaction was experimentally determined to double if the concentration of
reactant A is doubled, and is determined to increase 9 times when the concentration of
reactant B is tripled. What is the rate law expression described above?
Chapter 20 Solutions
Bundle: Physical Chemistry, 2nd + Student Solutions Manual
Ch. 20 - Prob. 20.1ECh. 20 - The oxidation-reduction reaction between iron...Ch. 20 - The oxidation-reduction reaction between iron...Ch. 20 - The rate of the reaction...Ch. 20 - For a certain reaction between NO and O2, the rate...Ch. 20 - For a reaction between SO2 and Cl2, the rate law...Ch. 20 - Consider the chemical reaction A+B+Cproducts...Ch. 20 - For the chemical reaction...Ch. 20 - Explain how a species might be part of a rate law...Ch. 20 - Refer to Example 20.2 and explain whether any...
Ch. 20 - Rate law experiments dont always give data in the...Ch. 20 - Prob. 20.12ECh. 20 - What must the units on k be for the following rate...Ch. 20 - What must the units on k be for the following rate...Ch. 20 - The reaction 2O33O2 has first-order kinetics and a...Ch. 20 - Digestive processes are first-order processes. The...Ch. 20 - Prob. 20.18ECh. 20 - Derive equation 20.15.Ch. 20 - Prob. 20.20ECh. 20 - To a very good approximation, the cooling of a hot...Ch. 20 - Assume that thermal decomposition of mercuric...Ch. 20 - Prob. 20.23ECh. 20 - Prob. 20.24ECh. 20 - Derive equation 20.22.Ch. 20 - a Write a rate law and an integrated rate law for...Ch. 20 - Derive an expression for the half-life of a a...Ch. 20 - Prob. 20.28ECh. 20 - Rewrite equation 20.27 so that it has the form of...Ch. 20 - One can also define a third-life, t1/3, which is...Ch. 20 - The decomposition of NH3: 2NH3N2+3H2 is a...Ch. 20 - Prob. 20.32ECh. 20 - Prob. 20.33ECh. 20 - When ionic compounds crystallize from a...Ch. 20 - An aqueous reaction that uses the solvent H2O as a...Ch. 20 - The rate law for the reaction...Ch. 20 - If a reaction has the same rate constant, what...Ch. 20 - List at least four experimentally determined...Ch. 20 - Prob. 20.39ECh. 20 - Prob. 20.40ECh. 20 - Prob. 20.41ECh. 20 - Prob. 20.42ECh. 20 - What is the value of the equilibrium constant of a...Ch. 20 - Prob. 20.44ECh. 20 - Prob. 20.45ECh. 20 - Show how equation 20.33 reduces to a simpler form...Ch. 20 - Write expressions like equation 20.37 for a set of...Ch. 20 - Prob. 20.48ECh. 20 - Prob. 20.49ECh. 20 - Prob. 20.50ECh. 20 - Prob. 20.51ECh. 20 - Prob. 20.52ECh. 20 - Prob. 20.53ECh. 20 - Prob. 20.54ECh. 20 - For what values of time, t, will 210Bi and 206Pb...Ch. 20 - Prob. 20.56ECh. 20 - An interesting pair of consecutive reactions...Ch. 20 - Find limiting forms of equation 20.47 for a k1>>k2...Ch. 20 - Prob. 20.59ECh. 20 - Prob. 20.60ECh. 20 - Prob. 20.61ECh. 20 - Prob. 20.62ECh. 20 - At room temperature (22C), the rate constant for...Ch. 20 - Recently, researchers studying the kinetics of...Ch. 20 - A reaction has k=1.771061/(Ms) at 25.0C and an...Ch. 20 - Prob. 20.66ECh. 20 - Prob. 20.67ECh. 20 - Prob. 20.68ECh. 20 - Nitric oxide, NO, is known to break down ozone,...Ch. 20 - a Suggest a mechanism for the bromination of...Ch. 20 - Prob. 20.71ECh. 20 - Prob. 20.72ECh. 20 - Determine a rate law for the chlorination of...Ch. 20 - Determine a rate law for the chlorination of...Ch. 20 - A proposed mechanism for the gas-phase...Ch. 20 - Prob. 20.76ECh. 20 - The nitration of methanol, CH3OH, by nitrous acid...Ch. 20 - Prob. 20.78ECh. 20 - Many gas-phase reactions require some inert body,...Ch. 20 - Prob. 20.80ECh. 20 - Carbonic anhydrase, an enzyme whose substrate is...Ch. 20 - Show that another form of the Michaelis-Menten...Ch. 20 - Prob. 20.83ECh. 20 - Prob. 20.84ECh. 20 - Prob. 20.85ECh. 20 - Prob. 20.86ECh. 20 - Pyrolysis involves heating compounds to break them...Ch. 20 - Prob. 20.88ECh. 20 - Label the elementary processes for the reaction...Ch. 20 - Prob. 20.90ECh. 20 - What are the rate laws of mechanisms 1 and 2 for...Ch. 20 - Estimate G for an elementary process whose rate...Ch. 20 - Prob. 20.93ECh. 20 - Prob. 20.94ECh. 20 - Prob. 20.95ECh. 20 - For the following two reactions H+Cl2HCl+Cl...Ch. 20 - Prob. 20.97ECh. 20 - Prob. 20.98ECh. 20 - Prob. 20.99ECh. 20 - Consider a reaction that has two parallel pathways...Ch. 20 - Consider a set of first-order consecutive...Ch. 20 - Prob. 20.102E
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
- Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the rate law? What is k in a rate law, and what are orders in a rate law? Explain.arrow_forwardExplain how a species might be part of a rate law but not part of a balanced chemical reaction.arrow_forwardCobra venom helps the snake secure food by binding to acetylcholine receptors on the diaphragm of a bite victim, leading to the loss of function of the diaphragm muscle tissue and eventually death. In order to develop more potent antivenins, scientists have studied what happens to the toxin once it has bound the acetylcholine receptors. They have found that the toxin is released from the receptor in a process that can be described by the rate law Rate = k [acetylcholine receptortoxin complex] If the activation energy of this reaction at 37.0C is 26.2 kJ/mol and A = 0.850 s1. what is the rate of reaction if you have a 0.200M solution of receptor-toxin complex at 37.0C?arrow_forward
- Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forward2. The rate law expression determined above can be used to evaluate proposed mechanisms for this hydrogen peroxide decomposition reaction. Any valid mechanism must be consistent with the rate expression. For example, a catalyst such as the I used here does not appear in the overall chemical equation, but if its concentration shows up in the rate expression, it must be a part of the mechanism at some step. A two-step mechanism suggested for the present reaction is: H₂O2 + I¯¯ →→→→H₂O + IO (slow) IO + H₂O2 →→ O2 + H₂O + I¯¯ (fast) Is this a valid mechanism? Is it consistent with the rate expression? Consistent with the stoichiometry of the reaction? What role does 10 play in the mechanism? Normal B|I\U X₂ X² → The valid mechanism would be rate = k [H₂0₂][1]. 131313 fx l 3. If we are actually studying this roaction by the method of initial BE Saved Tx OGarrow_forwardG.49.arrow_forward
- For the past 10 years, the unsaturated hydrocarbon 1,3-butadiene (CH2 = CH – CH = CH,) has ranked 38th among the top 50 industrial chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: CH,- CH, CH =CH The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0 x 10-4 s1 at 150 °C in a 0.53-L flask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 °C with an initial pressure of 55 torr.arrow_forwardExperimental data show that the rate law for the reaction 2 HgCl2(aq) + C2O4 2 -(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) is: rate = k[HgCl2][C2O4 2 -]2How will the rate of reaction change if the concentration of C2O4 2 - is tripled and the concentration of HgCl2 is doubled?arrow_forwardLet the rate of the reaction 2 NH3N2 + 3 H2 be expressed as -Δ[NH3]/Δt. Which of the following is the correct expression for the rate of the reaction in terms of Δ[H2]/Δt? Δ[NH3]/Δt = 1/3 Δ[H2]/Δt Δ[NH3]/Δt = 3/2 Δ[H2]/Δt Δ[NH3]/Δt = 2/3 Δ[H2]/Δt Δ[NH3]/Δt = 1/2 Δ[H2]/Δt Δ[NH3]/Δt = 2 Δ[H2]/Δtarrow_forward
- A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: A + B rightleftharpoons C; B + C-> D (fast) (slow) Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^ ^ 3*[D]).arrow_forwardA reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. Part A The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: B+ C C ( fast) + D (slow) A +B The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^3* [D]). • View Available Hint(s) Hνα ΑΣφ ? rate =arrow_forwardWrite why is True if the statement conforms to the concept of rate law and also write why is False if it does not. The balanced equation can be used to determine the rate of reaction.The slowly reactive or unreactive species in a reaction can be identified using rate law.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: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningPhysical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
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
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Enzymes - Effect of cofactors on enzyme; Author: Tutorials Point (India) Ltd;https://www.youtube.com/watch?v=AkAbIwxyUs4;License: Standard YouTube License, CC-BY
Enzyme Catalysis Part-I; Author: NPTEL-NOC IITM;https://www.youtube.com/watch?v=aZE740JWZuQ;License: Standard Youtube License