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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
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)

The First Law of Thermodynamics states that energy cannot be created nor destroyed, but instead is transferred. 

Understanding the First Law of Thermodynamics

Concept #1: First Law of Thermodynamics

Example #1: A chemist wishing to determine the final temperature of 30.0 g of a metal ore places it into an insulated beaker containing 615.5 g of water at 42.18 ºC. It is determined that the metal gains 19.11 kJ of energy. From the information provided, determine the system and the surroundings.

Concept #2: Heat and Work

Heat is the flow of thermal energy while work is the movement of reacting molecules.

Concept #3: Heat and Work Chart

Practice: What are the signs of q and w when a system loses heat while doing work on the surroundings?