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 overall equation and rate law for the gas-phase decomposition of dinitrogen pentoxide are2 N2O5(g) ⟶ 4 NO2(g) + O 2(g)               rate = k[N  2O5]Which of the following can be considered valid mechanisms for the reaction?I – One-step collisionII – 2 N 2O5(g) ⟶ 2 NO 3(g) + 2 NO 2(g)     [slow]      2 NO 3(g) ⟶ 2 NO 2(g) + 2 O (g)     [fast]               2 O  (g) ⟶ O 2(g)      [fast]III – N 2O5(g) ⇌ NO 3(g) + NO 2(g)     [fast]       NO 2(g) + N 2O5(g) ⟶ 3 NO 2(g) + O(g)     [slow]                 NO 3(g) + O(g) ⟶ NO2(g) + O2(g)     [fast]IV – 2 N 2O5(g) ⇌ 2 NO 2(g) + N2O3(g) + 3 O (g)     [fast]        N 2O3(g) + O(g) ⟶ 2 NO 2(g)     [slow]        2 O (g) ⟶ O 2(g)     [fast]V – 2 N2O5(g) ⟶ N4O10(g)               [slow]       N 4O10(g) ⟶ 4 NO2(g) + O 2(g)     [fast]

Problem

The overall equation and rate law for the gas-phase decomposition of dinitrogen pentoxide are

2 N2O5(g) ⟶ 4 NO2(g) + O 2(g)               rate = k[N  2O5]

Which of the following can be considered valid mechanisms for the reaction?

I – One-step collision

II – 2 N 2O5(g) ⟶ 2 NO 3(g) + 2 NO 2(g)     [slow]

      2 NO 3(g) ⟶ 2 NO 2(g) + 2 O (g)     [fast]

               2 O  (g) ⟶ O 2(g)      [fast]

III – N 2O5(g) ⇌ NO 3(g) + NO 2(g)     [fast]

       NO 2(g) + N 2O5(g) ⟶ 3 NO 2(g) + O(g)     [slow]

                 NO 3(g) + O(g) ⟶ NO2(g) + O2(g)     [fast]

IV – 2 N 2O5(g) ⇌ 2 NO 2(g) + N2O3(g) + 3 O (g)     [fast]

        N 2O3(g) + O(g) ⟶ 2 NO 2(g)     [slow]

        2 O (g) ⟶ O 2(g)     [fast]

V – 2 N2O5(g) ⟶ N4O10(g)               [slow]

       N 4O10(g) ⟶ 4 NO2(g) + O 2(g)     [fast]