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: In the lower atmosphere, one of the mechanisms proposed for the decomposition of ozone to produce oxygen, 2 O3 ⟶ 3 O 2, is(1) O3 ⇌ O 2 + O(2) O + O 3 ⟶ 2 O 2 Use the steady-state approximation to writ

Problem

In the lower atmosphere, one of the mechanisms proposed for the decomposition of ozone to produce oxygen, 2 O3 ⟶ 3 O 2, is

(1) O3 ⇌ O 2 + O

(2) O + O 3 ⟶ 2 O 2 

Use the steady-state approximation to write the rate law, assuming that step 2 is the rate-determining step.

The experimentally determined rate law is rate = k[O 3]2/[O2]. How can the rate law derived in (a) be rewritten to explain the known rate law?