Homework Help is Here – Start Your Trial Now!
Science
Chemistry
± Half-life (kinetics) for First Order Reactions < 10 of 18> I Review | Constants | Periodic Table Half-life equation for first-order reactions: The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be 0.693 reached. where t2 is the half-life in seconds (s), and k is the rate constant inverse seconds (s1) The integrated rate law for a first-order reaction is: [A] = [A]oe Part A Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial JA What is the half-life of a first-order reaction with a rate constant of 7.40x10-4 s12 value. Then we could substitute for [A] and rearrange the equation to: Express your answer with the appropriate units. > View Available Hint(s) 4/2 = 0.603 This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life, ? Value Units

± Half-life (kinetics) for First Order Reactions < 10 of 18> I Review | Constants | Periodic Table Half-life equation for first-order reactions: The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be 0.693 reached. where t2 is the half-life in seconds (s), and k is the rate constant inverse seconds (s1) The integrated rate law for a first-order reaction is: [A] = [A]oe Part A Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial JA What is the half-life of a first-order reaction with a rate constant of 7.40x10-4 s12 value. Then we could substitute for [A] and rearrange the equation to: Express your answer with the appropriate units. > View Available Hint(s) 4/2 = 0.603 This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life, ? Value Units

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 6PS: 6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were...
See similar textbooks
icon
Related questions
Question
+ Half-life (kinetics) for First Order Reactions 10 of 18 I Review | Constants | Periodic Table Half-life equation for first-order reactions: The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. 0.693 t1/2 = k where t/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s1). The integrated rate law for a first-order reaction is: [A] = [A]ge-kt Part A Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial [A], for [A] and What is the half-life of a first-order reaction with a rate constant of 7.40x10-4 s1? value. Then we could substitute S 2 rearrange the equation to: Express your answer with the appropriate units. tr/2 = 0.693 • View Available Hint(s) This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. ? Value Units
Transcribed Image Text:+ Half-life (kinetics) for First Order Reactions 10 of 18 I Review | Constants | Periodic Table Half-life equation for first-order reactions: The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. 0.693 t1/2 = k where t/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s1). The integrated rate law for a first-order reaction is: [A] = [A]ge-kt Part A Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial [A], for [A] and What is the half-life of a first-order reaction with a rate constant of 7.40x10-4 s1? value. Then we could substitute S 2 rearrange the equation to: Express your answer with the appropriate units. tr/2 = 0.693 • View Available Hint(s) This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. ? Value Units
Expert Solution
steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Rate Laws
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS