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: For the decomposition of nitrous oxide at 565°C, the rate of the reaction is determined by measuring the disappearance of N2O. 2N2O → 2N2 + O2 At the beginning of the reaction, the concentration of N 2O is 1.01 M. After 21.2 min the concentration has dropped to 0.419 M. What is the rate of the reaction? 

Problem

For the decomposition of nitrous oxide at 565°C, the rate of the reaction is determined by measuring the disappearance of N2O. 

2N2O → 2N2 + O2 

At the beginning of the reaction, the concentration of N 2O is 1.01 M. After 21.2 min the concentration has dropped to 0.419 M. 

What is the rate of the reaction? 

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