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 data shown below were collected for the following first-order reaction: N2O(g) → N2(g) + 1/2 O2(g) Temperature (K)  Rate Constant  (1/s)8003.24 x 10 - 59000.0021410000.061411000.955Use an Arrheniu

Problem
The data shown below were collected for the following first-order reaction: N2O(g) → N2(g) + 1/2 O2(g)
 Temperature (K Rate Constant  (1/s)
8003.24 x 10 - 5
9000.00214
10000.0614
11000.955


Use an Arrhenius plot to determine the activation barrier for the reaction.