CHEM 206
Concordia
Course Overview
Lessons & Practice
I. Welcome
1. Review
2.2hr- 1.I. Chapter Intro
1.7.1. Reaction Stoichiometry1.7.2. Practice: Balancing 1.7.3. Moles1.7.4. Example: Reaction Stoichiometry 1.7.5. Steps for doing Stoichiometry Problems1.7.6. Practice: Stoichiometry (Similar to a question asked on a previous year's midterm) 1.7.7. Practice: Hydrate Question (Similar to a question asked on a previous year's midterm)1.7.8. Example: Stoichiometry
1.8.1. Concentration of Solutions1.8.2. Example: Converting Molarity to Mole Fraction1.8.3. Example: Converting Mole Fraction to Molarity1.8.4. Example: Calculating Molarity from Combined Solutions1.8.5. Practice Question: Calculating Molarity from Mass1.8.6. Practice Question: Calculating Mole Fraction from Molarity
2. Thermochemistry
1.8hr3. Thermodynamics
42min3.2.1. Gibbs Free Energy and Spontaneity3.2.2. Spontaneity 3.2.3. Example: Spontaneity of a Reaction3.2.4. Predicting Spontaneity Based off Entropy3.2.5. Chemical Equilibrium and ΔG Equations3.2.6. DeltaGo and K 3.2.7. Example3.2.8. Chemical Equilibrium and ΔG Practice 3.2.9. Chemical Equilibrium and ΔG Practice #23.2.10. Chemical Equilibrium and ΔG Practice #33.2.11. Van't Hoff Practice Problem
4. Intermolecular Forces and Properties of Liquids
1hr5. Solutions
34min6. Kinetics
2hr6.2.1. Rate Laws6.2.2. Example: Determining Reaction Order6.2.3. Determining the Rate Law From Experimental Data 6.2.4. Shortcut to Find Units of k Quicker 6.2.5. Practice: Experimental Rate Law 6.2.6. Practice: Determining Rate Law Exponents6.2.7. Practice: Rate Law6.2.8. Practice: Units of the Rate Constant, K
6.3.1. Integrated Rate Laws for Various Orders 6.3.2. Example: Plotting a Straight Line with the Integrated Rate Laws 6.3.3. Practice: Integrated Rate Laws Practice6.3.4. Integrated Rate Laws Cheatsheet6.3.5. First Order Reactions6.3.6. Second Order Reactions6.3.7. Half-life for Various Orders 6.3.8. Practice: Half-Life 6.3.9. Practice: Radioactive Decay in Smoke Detectors
6.4.1. Arrhenius Equation6.4.2. Example: Arrhenius Equation 6.4.3. Example: Arrhenius Equation6.4.4. Practice: Arrhenius Equation6.4.5. How Do We Measure Ea6.4.6. Practice: Determining the Activation Energy6.4.7. 3 Neccessary Steps For a Reaction to Occur 6.4.8. Collision Theory6.4.9. Collision Theory Represented By A Graph6.4.10. Transition State Theory 6.4.11. Additional Notes on the Arrhenius Equation
7. Equilibrium
2.3hr8. Acids and Bases
2.3hr- 8.I. Chapter Intro
8.3.1. Acids and their Equations8.3.2. Practice8.3.3. Acids With Different Numbers of Protons8.3.4. Percent Ionization or Dissociation8.3.5. Example8.3.6. Bases and their Equations8.3.7. Example8.3.8. Example8.3.9. Relationships Between the Strength of an Acid/Base and its Conjugate Base/Acid8.3.10. How to Determine the Stronger Acid by Looking at Conjugate Bases8.3.11. Types of Acid or Base Reactions and pH Calculations Summary8.3.12. Acid Base Equations Cheatsheet8.3.13. Acid/Base Important Relationships Cheatsheet
9. Titrations
1.4hr10. Buffers
32min11. Solubility Equilibria
1.3hr11.1.1. Solubility11.1.2. Example: Ksp11.1.3. Practice: Calculating Molar Solubility11.1.4. Practice: Solubility11.1.5. Solubility Chart 11.1.6. Q vs K to Predict Solubility11.1.7. Solubility Products11.1.8. Example11.1.9. Example11.1.10. Example: Will A Precipitate Form?11.1.11. Practice: Solubility and Equilibrium11.1.12. Practice
CHEM 206 Flashcards
1/114
Kinetics
The study of the rates of chemical reactions.
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