Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: A possible mechanism for the decomposition of hydrogen peroxide isH2O2 → 2OHH2O2 + OH → H2O + HO2HO2 + OH → H2O + O2Using your results from Exercise 37, specify which step is the rate-determining step

Problem

A possible mechanism for the decomposition of hydrogen peroxide is

H2O→ 2OH
H2O2 + OH → H2O + HO2
HO2 + OH → H2O + O2

Using your results from Exercise 37, specify which step is the rate-determining step. What is the overall balanced equation for the reaction?

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Exercise 37. The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature:

Assuming that

determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [H2O2] at 4000. s after the start of the reaction.