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 2NO(g) + O2(g) ⟶ 2NO2(g) is rate = k[NO]2[O2]. In addition to the mechanism in the text (Section 16.6), the following ones have been proposed:I        2NO(g) + O2(g) ⟶2NO2(g)
II       2NO(g) ⇌ N2O2(g)                          [fast]
         N2O2(g) + O2(g) ⟶2NO2(g)           [slow]
III      2NO(g) ⇌ N2(g) + O2(g)                  [fast]
         N2(g) + 2O2(g) ⟶ 2NO2(g)            [slow]
(b) Which of these mechanisms is most reasonable? Why?

Solution: The rate law for 2NO(g) + O2(g) ⟶ 2NO2(g) is rate = k[NO]2[O2]. In addition to the mechanism in the text (Section 16.6), the following ones have been proposed:I        2NO(g) + O2(g) ⟶2NO2(g)II      

Problem

The rate law for 2NO(g) + O2(g) ⟶ 2NO2(g) is rate = k[NO]2[O2]. In addition to the mechanism in the text (Section 16.6), the following ones have been proposed:

I        2NO(g) + O2(g) ⟶2NO2(g)
II       2NO(g) ⇌ N2O2(g)                          [fast]
         N2O2(g) + O2(g) ⟶2NO2(g)           [slow]
III      2NO(g) ⇌ N2(g) + O2(g)                  [fast]
         N2(g) + 2O2(g) ⟶ 2NO2(g)            [slow]

(b) Which of these mechanisms is most reasonable? Why?