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: The following equation represents the decomposition of a generic diatomic element in its standard state.1/2X2 (g) ⇌ X (g)Assume that the standard molar Gibbs energy of formation of X(g) is 4.82 kJ·mol–1 at 2000 K and –58.08 kJ·mol–1 at 3000 K.a. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.b. Assuming that ΔH°rxn is independent of temperature, determine the value of ΔH°rxn from these data. 

Problem

The following equation represents the decomposition of a generic diatomic element in its standard state.

1/2X2 (g) ⇌ X (g)

Assume that the standard molar Gibbs energy of formation of X(g) is 4.82 kJ·mol–1 at 2000 K and –58.08 kJ·mol–1 at 3000 K.

a. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.





b. Assuming that ΔH°rxn is independent of temperature, determine the value of ΔH°rxn from these data.