Ch.11 - Liquids, Solids & Intermolecular ForcesWorksheetSee 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.1/2 X2(g) → X(g)Assume that the standard molar Gibbs energy of formation of X(g) is 4.76 kJ•mol-

Solution: The following equation represents the decomposition of a generic diatomic element in its standard state.1/2 X2(g) → X(g)Assume that the standard molar Gibbs energy of formation of X(g) is 4.76 kJ•mol-

Problem

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

1/2 X2(g) → X(g)


Assume that the standard molar Gibbs energy of formation of X(g) is 4.76 kJ•mol-1 at 2000. K and - 65.63 kJ•mol-1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.

K at 2000. K = _____

K at 3000. K = _____






Assuming that delta H°rxn, is independent of temperature, determine the value of Δ H°rxn from these data.

ΔH°rxn = ______ kJ mol-1