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
Problem

The proposed mechanism for a reaction is

NO + O3 => NO3 + O     Fast

NO3 + O => NO2 + O2   Slow

Which of the following would be a rate law for the reaction?

a. rate = k [NO][O3]

b. rate = k [NO] [O] [NO] [O3]

c. rate = k [NO3] [O] 

d. rate = k [NO]

e. rate = k [NO] [NO3]

Solution

We're being asked to determine the rate law for the proposed mechanism.

NO + O3 → NO3 + O     Fast

NO3 + O → NO2 + O2   Slow


When a reaction mechanism is given, the rate law can be determined using the slow step in the reaction mechanism.

  • Rate law only involves the reactants
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