Ch. 17 - Chemical ThermodynamicsSee 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: Calculate the change in the standard entropy of the system, ΔS°, for the synthesis of ammonia from N2(g) and H2(g) at 298 K.  S° (N2) = 191.5 J/mol•K S° (H2) = 130.6 J/mol•K S° (NH3) = 192.5 J/mol•K

Problem

Calculate the change in the standard entropy of the system, ΔS°, for the synthesis of ammonia from N2(g) and H2(g) at 298 K. 

S° (N2) = 191.5 J/mol•K

S° (H2) = 130.6 J/mol•K

S° (NH3) = 192.5 J/mol•K