Ch.6 - Chemical EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
The Equilibrium State
The Reaction Quotient
Le Chatelier's Principle
Chemical Thermodynamics: Enthalpy
Chemical Thermodynamics: Entropy
Chemical Thermodynamics: Gibbs Free Energy
Solubilty Product Constant
Protic Acids and Bases
The pH Scale
Acid Strength

Entropy represents the quantity of a system's thermal energy that couldn't be converted into mechanical work. 

Understanding Entropy

Concept #1: Entropy represents the amount of disorder, chaos or randomness in our system. 

Concept #2: As the distance between molecules increases there will be an increase in entropy. 

Concept #3: When comparing the entropy of ionic compounds it is best to examine their lattice energies. 

Entropy Calculations

Example #1: Predict the sign of entropy for each of the following processes?

a) Iat 90oC and 5.0 atm  →  I2 at 50oC and 10.0 atm

b) NH4Cl(s) →  HCl(g) +  NH3(g)

c) CH4(g)  +  2 O2(g)  →   CO2(g)  +  2 H2O(l) 

Example #2: When an aqueous solution containing Al3+ at 25°C is mixed with an aqueous solution of hydroxide at 25°C an immediate precipitate of insoluble aluminum hydroxide is formed: 

Al3+ (aq) + 3 OH – (aq)  →  Al(OH)3 (s)


Practice: Which of the following has the greatest entropy, S?