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 reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:O3(g) + NO(g) → O2(g) + NO2(g)The rate law for this reaction is:rate of reaction = k[O3][NO]a.

Problem

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:

O3(g) + NO(g) → O2(g) + NO2(g)

The rate law for this reaction is:

rate of reaction = k[O3][NO]

a. Given that k = 3.66x10 6 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O 3]0 = 2.25x10-6 M and [NO]0 = 4.37x10-5 M, owing to continuous production from separate sources. (M s-1)






b. Calculate the number of moles of NO2(g) produced per hour per liter of air. (mol h -1  L-1)