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 of the reactionNO2 (g) + CO (g) → NO (g) + CO2(g)depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected:Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 x 104 s after the start of the reaction.

Solution: The rate of the reactionNO2 (g) + CO (g) → NO (g) + CO2(g)depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected:Determine t

Problem

The rate of the reaction

NO2 (g) + CO (g) → NO (g) + CO2(g)

depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected:

Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 x 104 s after the start of the reaction.