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 decomposition of N2O3(g) to NO2(g) and NO(g) is followed by measuring [NO2] at different times. The following data are obtained.[NO2] (mol/L)  0    0.193    0.316    0.427     0.784t (s) 

Problem
The rate of decomposition of N2O3(g) to NO2(g) and NO(g) is followed by measuring [NO2] at different times. The following data are obtained.
[NO2] (mol/L)  0    0.193    0.316    0.427     0.784
t (s)  0     884   1610  2460  50,000 

The reaction follows a first-order rate law. Calculate the rate constant. Assume that after 50,000 s all the N2O3(g) had decomposed.