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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

Catalyst is a substance that increases the rate of reaction by lowering the Activation Energy (Ea) of a reaction.

Catalyzed vs Uncatalyzed Reactions

Concept #1: Catalyzed vs Uncatalyzed Reactions

Example #1: A certain reaction has an enthalpy value of –20 kJ and an activation energy of 40 kJ. A catalyst is found that lowers the activation energy of the reaction by 10 kJ. What is the total difference in energy between the products and the transition state?

Practice: Which of the following statements is true regarding the energy diagram provided? 

i. The reaction is endothermic.

ii. Activation energy would be less than + 10 kJ after a catalyst is added.

iii. The reaction absorbs energy.

iv. Activation energy would be greater than + 10 kJ after a catalyst is added.

a) I only            b) II only      c) I and III         d) II, III and IV