Chemistry: Structure... -Masteringchem.
2nd Edition
ISBN: 9780134449234
Author: Tro
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 14, Problem 82E
The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower must the activation barrier be when sucrose is in the active site of the enzyme? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical and a temperature of 25°C.)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
Chemistry: Structure... -Masteringchem.
Ch. 14 - Explain why lizards become sluggish in cold...Ch. 14 - Why are reaction rates important (both practically...Ch. 14 - Using the idea that reactions occur as a result of...Ch. 14 - Using the idea that reactions occur as a result of...Ch. 14 - What units are typically used to express the rate...Ch. 14 - Why is the reaction rate for reactants defined as...Ch. 14 - Explain the difference between the average rate of...Ch. 14 - Consider a simple reaction in which a reactant A...Ch. 14 - How is the order of a reaction generally...Ch. 14 - For a reaction with multiple reactants, how is the...
Ch. 14 - Explain the difference between the rate law for a...Ch. 14 - Write integrated rate laws for zero-order,...Ch. 14 - What does the term half-life mean? Write the...Ch. 14 - How do reaction rates typically depend on...Ch. 14 - Prob. 15ECh. 14 - What is an Arrhenius plot? Explain the...Ch. 14 - Explain the meaning of the orientation factor in...Ch. 14 - Explain the difference between a normal chemical...Ch. 14 - In a reaction mechanism, what is an elementary...Ch. 14 - What are the two requirements for a proposed...Ch. 14 - What is an intermediate within a reaction...Ch. 14 - What is a catalyst? How does a catalyst increase...Ch. 14 - Explain the difference between homogeneous...Ch. 14 - What are the four basic steps involved in...Ch. 14 - What are enzymes? What is the active site of an...Ch. 14 - What is the general two-step mechanism by which...Ch. 14 - Consider the reaction. 2HBr(g)H2(g)+Br2(g) Express...Ch. 14 - Consider the reaction 2N2O(g)2N2(g)+O2(g) Express...Ch. 14 - For the reaction 2A(g)+B(g)3C(g) determine the...Ch. 14 - For the reaction A(g)+12B(g)2C(g) determine the...Ch. 14 - Consider the reaction. Cl2(g)+3F2(g)2ClF3(g)...Ch. 14 - Consider the reaction. 8H2S(g)+4O2(g)8H2O(g)+S8(g)...Ch. 14 - Consider the reaction: C4H8(g)2C2H4(g) The...Ch. 14 - Consider the reaction: NO2(g)NO(g)+12O2(g) The...Ch. 14 - Consider the reaction. H2(g)+Br2(g)2HBr(g) The...Ch. 14 - Consider the reaction. 2H2O2(aq)2H2O(l)+O2(g) The...Ch. 14 - This graph shows a plot of the rate of a reaction...Ch. 14 - This graph shows a plot of the rate of a reaction...Ch. 14 - What are the units of k for each type of reaction?...Ch. 14 - This reaction is first order in N2O5:...Ch. 14 - A reaction in which A, B, and C react to form...Ch. 14 - A reaction in which A, B, and C react to form...Ch. 14 - Consider the tabulated data showing initial rate...Ch. 14 - Consider the tabulated data showing initial rate...Ch. 14 - The tabulated data were collected for this...Ch. 14 - The tabulated data were collected for this...Ch. 14 - Indicate the order of reaction consistent with...Ch. 14 - Indicate the order of reaction consistent with...Ch. 14 - The tabulated data show the concentration of AB...Ch. 14 - The tabulated data show the concentration of N2O5...Ch. 14 - The tabulated data show the concentration of...Ch. 14 - Prob. 52ECh. 14 - This reaction was monitored as a function of time:...Ch. 14 - This reaction was monitored as a function of time:...Ch. 14 - Prob. 55ECh. 14 - Prob. 56ECh. 14 - Prob. 57ECh. 14 - Prob. 58ECh. 14 - The diagram shows the energy of a reaction as the...Ch. 14 - Prob. 60ECh. 14 - Prob. 61ECh. 14 - Prob. 62ECh. 14 - Prob. 63ECh. 14 - The rate constant (k) for a reaction is measured...Ch. 14 - The tabulated data shown here were collected for...Ch. 14 - Prob. 66ECh. 14 - The tabulated data were collected for the...Ch. 14 - Prob. 68ECh. 14 - A reaction has a rate constant of 0.0117/s at...Ch. 14 - A reaction has a rate constant of 0.000122/s at...Ch. 14 - Prob. 71ECh. 14 - Prob. 72ECh. 14 - Prob. 73ECh. 14 - Prob. 74ECh. 14 - Prob. 75ECh. 14 - Prob. 76ECh. 14 - Consider this three-step mechanism for a...Ch. 14 - Prob. 78ECh. 14 - Prob. 79ECh. 14 - Prob. 80ECh. 14 - Suppose that a catalyst lowers the activation...Ch. 14 - The activation barrier for the hydrolysis of...Ch. 14 - The tabulated data were collected for this...Ch. 14 - Prob. 84ECh. 14 - Consider the reaction: A+B+CD The rate law for...Ch. 14 - Consider the reaction: 2O3(g)3O2(g) The rate law...Ch. 14 - At 700 K acetaldehyde decomposes in the gas phase...Ch. 14 - Prob. 88ECh. 14 - Dinitrogen pentoxide decomposes in the gas phase...Ch. 14 - Cyclopropane (C3H6) reacts to form propene (C3H6)...Ch. 14 - Iodine atoms combine to form I2 in liquid hexane...Ch. 14 - Prob. 92ECh. 14 - The reaction AB(aq)A(g)+B(g) is second order in AB...Ch. 14 - The reaction 2H2O2(aq)2H2O(l)+O2(g) is first order...Ch. 14 - Consider this energy diagram: a. How many...Ch. 14 - Consider the reaction in which HCI adds across the...Ch. 14 - The desorption of a single molecular layer of...Ch. 14 - The evaporation of a 120-nm film of n-pentane from...Ch. 14 - Prob. 99ECh. 14 - Prob. 100ECh. 14 - Prob. 101ECh. 14 - Consider the two reactions: O+N2NO+NEa= 315 kJ/mol...Ch. 14 - Anthropologists can estimate the age of a bone or...Ch. 14 - Prob. 104ECh. 14 - Consider the gas-phase reaction: H2(g)+I2(g)2HI(g)...Ch. 14 - Consider the reaction:...Ch. 14 - Prob. 107ECh. 14 - Prob. 108ECh. 14 - A certain substance X decomposes. Fifty percent of...Ch. 14 - Prob. 110ECh. 14 - Prob. 111ECh. 14 - Prob. 112ECh. 14 - Prob. 113ECh. 14 - Prob. 114ECh. 14 - Prob. 115ECh. 14 - Prob. 116ECh. 14 - Phosgene (Cl2CO), a poison gas used in World War...Ch. 14 - The rate of decomposition of N2O3(g) to NO2(g) and...Ch. 14 - At 473 K, for the elementary reaction...Ch. 14 - Prob. 120ECh. 14 - Prob. 121ECh. 14 - A particular reaction, Aproducts has a rate that...Ch. 14 - Prob. 123ECh. 14 - A certain compound, A, reacts to form products...Ch. 14 - Methane (CH4) is a greenhouse gas emitted by...Ch. 14 - This graph shows the concentration of the reactant...Ch. 14 - Prob. 2SAQCh. 14 - Prob. 3SAQCh. 14 - Prob. 4SAQCh. 14 - Prob. 5SAQCh. 14 - Prob. 6SAQCh. 14 - Prob. 7SAQCh. 14 - Prob. 8SAQCh. 14 - The rate constant of a reaction is measured at...Ch. 14 - Prob. 10SAQCh. 14 - The mechanism shown here is proposed for the...Ch. 14 - Prob. 12SAQCh. 14 - These images represent the first-order reaction AB...Ch. 14 - Prob. 14SAQCh. 14 - Prob. 15SAQ
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
- When enzymes are present at very low concentration, their effect on reaction rate can be described by first-order kinetics. Calculate by what factor the rate of an enzyme-catalyzed reaction changes when the enzyme concentration is changed from 1.5 107 M to 4.5 106 M.arrow_forwardThe precipitation of egg albumin in water at 100C has an activation energy of 52.0 kJ/mol. By what percent does the rate of precipitation decrease if the water is at 92C?arrow_forwardBacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?arrow_forward
- 11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?arrow_forwardThe decomposition of NH3 to N2 and H2 was studied on two surfaces: Surface Ea (kJ/mol) W 163 Os 197 Without a catalyst, the activation energy is 335 kJ/mol. a. Which surface is the better heterogeneous catalyst for the decomposition of NH3? Why? b. How many times faster is the reaction at 298 K on the W surface compared with the reaction with no catalyst present? Assume that the frequency factor A is the same for each reaction. c. The decomposition reaction on the two surfaces obeys a rate law of the form Rate=k[NH3][H2] How can you explain the inverse dependence of the rate on the H2 concentration?arrow_forwardCompare the functions of homogeneous and heterogeneous catalysts.arrow_forward
- The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?arrow_forwardThe hydrolysis of the sugar sucrose to the sugars glucose and fructose follows a first-order rate equation for the disappearance of sucrose. C12H22O11(aq)+H2O(l)C6H12O6(aq)+C6H12O6(aq) Rate =k[C12H22O11] In neutral solution, k=2.11011 at 27 C. (As indicated by the rate constant, this is a very slow reaction. In the human body, the rate of this reaction is sped up by a type of catalyst called an enzyme.) (Note: That is not a mistake in the equation—the products of the reaction, glucose and fructose, have the same molecular formulas, C6H12O6, but differ in the arrangement of the atoms in their molecules). The equilibrium constant for the reaction is 1.36105 at 27 C. What are the concentrations of glucose, fructose, and sucrose after a 0.150 M aqueous solution of sucrose has reached equilibrium? Remember that the activity of a solvent (the effective concentration) is 1.arrow_forwardThe rate equation for the hydrolysis of sucrose to fructose and glucose Cl2H22O11(aq) + H2O () 2 C6Hl2O6(aq) is [sucrose]/t = k[C12H22O11]. After 27 minutes at 27 C, the sucrose concentration decreased from 0.0146 M to 0.0132 M. Find the rate constant, k.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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