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: 2NO2(g) →  2NO(g) + O2(g) rate = k[NO2]2 When the initial concentration of NO2 is 100 mM, it takes 55 s for 90% of the NO2 to react. Calculate the rate constant.  a) 0.042 M -1-1  b) 1.8 x 10 -5-1-1  c) 1.6 M -1-1  d) 1.6 x 10 -3 M -1s -1 e) 0.13 M -1s -1  

Solution: Consider the following reaction: 2NO2(g) →  2NO(g) + O2(g) rate = k[NO2]2 When the initial concentration of NO2 is 100 mM, it takes 55 s for 90% of the NO2 to react. Calculate the rate constant.  a

Problem

Consider the following reaction:

2NO2(g) →  2NO(g) + O2(g) rate = k[NO2]2

When the initial concentration of NO2 is 100 mM, it takes 55 s for 90% of the NO2 to react. Calculate the rate constant. 

a) 0.042 M -1-1 

b) 1.8 x 10 -5-1-1 

c) 1.6 M -1-1 

d) 1.6 x 10 -3 M -1s -1

e) 0.13 M -1s -1