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: The mechanism shown here is proposed for the gas phase reaction, 2 N2O5 → 4 NO2 + O2. What rate law does the mechanism predict?N2 O5 ⇌ NO2 + NO3          Fast, k1 (forward), k-1 (reverse),NO2 + NO3 →

Problem

The mechanism shown here is proposed for the gas phase reaction, 2 N2O5 → 4 NO2 + O2. What rate law does the mechanism predict?
N2 O5 NO2 + NO3          Fast, k1 (forward), k-1 (reverse),
NO2 + NO3NO2 + O2 + NO          Slow
NO + N2O5 → 3 NO2          Fast

a) Rate = k[N2O5]
b) Rate = k[N2O5]2
c) Rate = k[N2O5]0
d) Rate = k[NO2][NO3]