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: Consider the following reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g)      rate = k[N2O5]  If the initial concentration of N2O5 is 0.80 M, the concentration after 5 half-lives is a) 0.050 M b) 0.025 M

Problem

Consider the following reaction:

2 N2O(g) → 4 NO(g) + O(g)      rate = k[N2O5

If the initial concentration of N2O5 is 0.80 M, the concentration after 5 half-lives is

a) 0.050 M

b) 0.025 M

c) 0.032 M

d) 0.11 M

e) 0.16 M