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 reaction of nitrogen dioxide with carbon monoxide NO2(g) + CO(g) => CO2(g) + NO(g) has been studied and the following mechanism has been proposed:

NO2(g) + NO2(g) => NO3(g) + NO(g) slow

NO3(g) + CO(g) => NO2(g) + CO2(g) fast

What rate law corresponds to this mechanism?

A. rate = k[NO2][CO]/[CO2][NO]

B. rate = k[NO2][CO]

C. rate = k[NO2]2 

D. rate = k[NO2]

E. rate = k[CO2][NO]/[NO2][CO]

Solution

Determine the overall order of the reaction by analyzing the provided elementary reactions:

1. NO2(g) + NO2(g) → NO3(g) + NO(g)                (slow)

2. NO3(g) + CO(g) → NO2(g) + CO2(g) fast

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