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Chemistry Chapter 6 Notes

by: Meghan Skiba

Chemistry Chapter 6 Notes CH 104

Marketplace > University of Alabama - Tuscaloosa > CH 104 > Chemistry Chapter 6 Notes
Meghan Skiba

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About this Document

Chapter 6 notes from Chemistry 104
Introductory Chemistry
Stephen Woski
Class Notes
Chemistry, Organic Chemistry
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This 2 page Class Notes was uploaded by Meghan Skiba on Sunday October 9, 2016. The Class Notes belongs to CH 104 at University of Alabama - Tuscaloosa taught by Stephen Woski in Fall 2016. Since its upload, it has received 4 views.


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Date Created: 10/09/16
Chemistry 104 Chapter 6 Notes Energy Changes, Reaction Rates, and Equilibrium Energy Chemical bonds store potential energy Compounds with lower potential energy are more stable than compounds with higher potential energy Reactions that form products that have lower potential energy than the reactants are more ideal Units of Energy Calorie (calorie or kilocalorie – kcal) Joule (joule – J or kilojoule – kJ ) 1 calorie = 4.184 J 1,000 J = 1 kJ 1,000 cal = 1 kcal 1 kcal = 4.184 kJ Bond Dissociation Energies Bonding lowers energy of system Breaking bonds requires added energy BUT… not all bonds are created equal Endothermic vs Exothermic Endothermic (H is positive) Heat is absorbed Bonds broken in reactants are stronger than bonds formed in the products Products are higher in energy than the reactants Exothermic (H is negative) Heat is released Bonds formed in the products are stronger than bonds broken in reactants Products are lower in energy than the reactants Le Chatelier’s Principle Adding reactant – Equilibrium favors products Removing reactant – Equilibrium favors reactants Adding product – Equilibrium favors reactants Removing product – Equilibrium favors products Increasing temperature – Endothermic reaction; equilibrium favors products Exothermic reaction; equilibrium favors reactants Decreasing temperature – Endothermic reaction; equilibrium favors reactants Exothermic reaction; equilibrium favors products Increasing pressure – Equilibrium favors the side that has fewer molecules Decreasing pressure – Equilibrium favors the side that has more moles


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