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: HI has a boiling point of –35.4°C with a standard enthalpy of vaporization of 21.16 kJ/mol. Calculate the standard entropy of vaporization of HI.a) 598 J/K·molb) 68.6 J/K·molc) 75.2 J/K·mold) 0.068 J/

Problem

HI has a boiling point of –35.4°C with a standard enthalpy of vaporization of 21.16 kJ/mol. Calculate the standard entropy of vaporization of HI.

a) 598 J/K·mol

b) 68.6 J/K·mol

c) 75.2 J/K·mol

d) 0.068 J/K·mol

e) 89.0 J/K·mol