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 reaction: 2N2O5 (g) → 4NO2 (g) + O2 (g) the rate constant is k = 2.8×10 −3 sec −1, if the initial concentration of N2O5 is 1.58 mol/L, the concentration of N2O5 after 5 min. is a) 0.27 mol/

Problem

For the reaction:

2N2O5 (g) → 4NO2 (g) + O2 (g)

the rate constant is k = 2.8×10 −3 sec −1, if the initial concentration of N2O5 is 1.58 mol/L, the concentration of N2O5 after 5 min. is

a) 0.27 mol/L

b) 1.55 mol/L

c) 1.47 mol/L

d) 0.68 mol/L

e) 0.75 mol/L