Clutch Prep is now a part of Pearson
Ch.7 Energy, Rate and EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Sections
Nature of Energy
First Law of Thermodynamics
Endothermic & Exothermic Reactions
Bond Energy
Thermochemical Equations
Heat Capacity
Thermal Equilibrium (Simplified)
Hess's Law
Rate of Reaction
Energy Diagrams
Chemical Equilibrium
The Equilibrium Constant
Le Chatelier's Principle
Solubility Product Constant (Ksp)
Spontaneous Reaction
Entropy (Simplified)
Gibbs Free Energy (Simplified)

Entropy is the disorder or chaos associated with a system’s inability to convert thermal energy into mechanical work.

Entropy and 2nd Law

Concept #1: Entropy

The Second Law of Thermodynamics states that there is a natural tendency of systems (chemical reactions) to move towards a state of disorder.

Example #1: The second law of thermodynamics leads us to conclude:

Concept #2: Entropy: Physical and Chemical Changes

Increase in temperature, moles of gas and bond breaking causes an increase in Entropy (+∆S).

Example #2: Which one of the following processes produces a decrease in the entropy of the system?

Practice: Predict how the entropy of the substance is affected in the following processes:

CH4 (g, 125°C)   →   CH4 (g, 200°C)

Practice: Which reaction is most likely to have a positive ∆S of system?

Practice: Which of the following processes shows a decrease in entropy of the system?