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 rate law for the reactionNO2(g) + CO(g) ⟶NO(g) + CO2(g)is rate = k[NO2]2; one possible mechanism is shown in Section 16.6.(b) Consider the following alternative mechanism:(1) 2NO2(g) ⟶ N2(g) + 2O2


The rate law for the reaction

NO2(g) + CO(g) ⟶NO(g) + CO2(g)

is rate = k[NO2]2; one possible mechanism is shown in Section 16.6.

(b) Consider the following alternative mechanism:

(1) 2NO2(g) ⟶ N2(g) + 2O2(g)         [slow]
(2) 2CO(g) + O2(g) ⟶2CO2(g)        [fast]
(3) N2(g) + O2(g) ⟶2NO(g)            [fast]

Is the alternative mechanism consistent with the rate law? Is one mechanism more reasonable physically? Explain.