Homework Help is Here – Start Your Trial Now!
Science
Chemistry
The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H₂O₂ and has k = 0.041 min-¹ in the rate -1 law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O2 concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min.

The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H₂O₂ and has k = 0.041 min-¹ in the rate -1 law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O2 concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.50QE
See similar textbooks
icon
Related questions
Question
The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H2O2 and has k = 0.041 min -1 in the rate law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O₂ concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min. How much time will it take for the H₂O2 1, concentration to decrease by ? Answer in units of min. How much time will it take for the H₂O2 concentration to decrease by 83%? Answer in units of min.
Transcribed Image Text:The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H2O2 and has k = 0.041 min -1 in the rate law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O₂ concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min. How much time will it take for the H₂O2 1, concentration to decrease by ? Answer in units of min. How much time will it take for the H₂O2 concentration to decrease by 83%? Answer in units of min.
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

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: 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 & 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 Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS