Ch.13 - Chemical KineticsSee 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 2A + B → products determine the rate law for the reaction given the following data:  Initial Concentration M,           Initial Rate, M·s–1   A          B 0.10       0.10                           2.0 x 10   –2 0.20       0.10                           8.0 x 10   –2 0.30       0.10                           1.8 x 10   –1 0.20       0.20                           8.0 x 10   –2 0.30       0.30                           1.8 x 10   –1 a) rate = k [A] b) rate = k [A][B] c) rate = k[A] [B] 0 d) rate = k[A]2 e) rate = k[B]2

Problem

For the reaction

2A + B → products

determine the rate law for the reaction given the following data: 

Initial Concentration M,           Initial Rate, M·s–1

  A          B

0.10       0.10                           2.0 x 10   –2

0.20       0.10                           8.0 x 10   –2

0.30       0.10                           1.8 x 10   –1

0.20       0.20                           8.0 x 10   –2

0.30       0.30                           1.8 x 10   –1

a) rate = k [A]

b) rate = k [A][B]

c) rate = k[A] [B] 0

d) rate = k[A]2

e) rate = k[B]2