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In this course, you will :
- introduces the concept of chemical equilibrium and its application to a variety of chemical reactions The quantitative aspects of equilibrium are thoroughly discussed, including the law of mass action and the relationship between equilibrium constants and concentrations and pressures of substances.
- Much of the discussion focuses on problem-solving techniques for determining the value of the equilibrium constant or the concentrations of substances at equilibrium. ICE (initial-change-equilibrium) tables are introduced as a problem-solving tool, with several examples of their application provided.
- To begin, the concept of weak acids and bases is investigated, as well as the equilibrium constants associated with their ionisation in water and how the value of the equilibrium constant is related to the acid or base's strength.
- continues and expands on the equlibria theme You will investigate buffers, acid/base titrations, and insoluble salt equilibria.
- The prediction of whether a reaction will occur spontaneously under a given set of conditions is the overarching theme of thermodynamics. For this purpose, entropy and free energy are defined and used.
Syllabus :
1. Kinetics
- The Rate of Chemical Reactions
- Comparing Rate of Change for Reactants and Products
- Obtaining a Rate Law from Experimental Data Equations
- The Rate Law
- Obtaining a Rate Law from Experimental Data
- Rate Law Calculations
- First-Order Kinetics and the Integrated Rate Law
- Graphic 1st Order
- First-Order Kinetics and the Half-Life
- Second-Order Reactions
- Graphics 2nd Order
- Collision Theory
- Activation Energy
- The Arrhenius Equation
- Graphic Activation Energy
- Reaction Mechanisms
- RDS Fast Equilibrium
- Rate Determining Step
- Catalysis
2. Chemical Equilibrium
- Dynamic Equilibrium
- Law of Mass Action
- Law of Mass Action for Combined Reactions
- Relationship Between Kc and Kp
- Calculating the Equilibrium Constant
- Finding Kc
- Reaction Quotient
- Predicting Reaction Progress with the Reaction Quotient
- Calculating Equilibrium Concentrations
- Le Chatelier's Principle
- How Changes Shift the Equilibrium
3. Acid-Base Equilibria
- Acids and Bases
- pH and Kw
- Finding Kw
- Acid Strength
- Finding pH1
- Strong and Weak Bases
- Calculating equilibrium concentrations of a weak base
- Ions as Acids and Bases
- Acid-base properties of aqueous salts
- Types of Acids
- Polyprotic Acids
4. Aqueous Equilibria
- Buffers and the Common Ion Effect
- pH of Buffer Solutions
- Aqueous Equilibria Worked Example
- Buffer Action
- Aqueous Equilibria Worked Example
- Buffer: Preparation and Capacity
- Strong Acid - Strong Base Titration
- Titrations Involving Either a Weak Acid or a Weak Base
- Aqueous Equilibria Worked Example
- Polyprotic Acid Titrations
- Indicators
- Solubility Equilibria
- Molar Solubility and the Solubility Product
- Aqueous Equilibria Worked Example
- Molar Solubility and the Common Ion Effect
- Aqueous Equilibria Worked Example
- Aqueous Equilibria Worked Example
- The Effect of pH on Solubility
- Precipitation Reaction and Selective Precipitation
- Aqueous Equilibria Worked Example
5. Thermodynamics
- Review of Thermochemistry
- Enthalpy of Reaction Refresher
- Spontaneous vs. Nonspontaneous
- Standard versus Nonstandard Free Energy Change
- The Second Law of Thermodynamics
- Entropy
- Entropy of the Universe
- Gibbs Free Energy
- Gibbs Free Energy Example Problem
- The Third Law of Thermodynamics
- Calculating Standard Entropy Change
- Thermodynamics Worked Example
- Calculating Standard Free Energy Change
- Thermodynamics Worked Example
- Comparing ∆G° and K
- Thermodynamics Worked Example
- Thermodynamics Worked Example
- Spontaneous vs Nonspontaneous Example Problem
