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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
Intro to Chemical Kinetics
Energy Diagrams
Factors Influencing Rates
Average Rate of Reaction
Stoichiometric Rate Calculations
Instantaneous Rate
Collision Theory
Arrhenius Equation
Rate Law
Reaction Mechanism
Integrated Rate Law

Average (General) Rate is the change in the concentration of a compound over a period of time.

Average Rate

Concept #1: Average Rate of Reaction

Example #1: Provide the expressions for rate of disappearance of reactants and rate of appearance of products for the following reaction: 2 C3H7OH (l) + 9 O2 (g) ⟶ 6 CO2 (g) + 8 H2O (g)

Example #2: Calculate the average rate of change in concentration of NO in the first 5 seconds of the reaction if the concentration dropped from 1.3 M to 1.09 M.

 2 NO (g) + 2 H2 (g) ⟶ N2 (g) + 2 H2O (g)

Practice: Consider the following reaction: 2 H2O2 (aq) → 2 H2O (l) + O2 (g)

Calculate the rate of the reaction between 25 sec and 65 sec.