Ch. 17 - Chemical ThermodynamicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Given the hypothetical reaction. 4 X(s) + 6Y(s) → 4Z (s) + 9A(g) Calculate Δ S for this reaction at 25°C, given the following absolute entropies: S°J/(K-mol) X (s) 40.72 Y(s) 28.64 Z(s) 66.92 A(g) 54.

Problem
Given the hypothetical reaction. 
4 X(s) + 6Y(s) → 4Z (s) + 9A(g) 
Calculate Δ S for this reaction at 25°C, given the following absolute entropies: 
S°J/(K-mol) 
X (s) 40.72 
Y(s) 28.64 
Z(s) 66.92 
A(g) 54.98