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: To examine the extent that water spontaneously decomposes to its elements at room temperature, consider that the standard Gibbs energy of formation (∆G ̊f) of H2O (l) is –237.20 kJ/mol. Use this information to calculate the equilibrium constant for the decomposition of water at 298 K: 2 H2O (l) ⇄ 2 H2 (g) + O2 (g) a) 7.0 x 10 –84 b) 2.6 x 10 –42 c) 0.91 d) 3.8 x 1041 e) 1.4 x 1083

Problem

To examine the extent that water spontaneously decomposes to its elements at room temperature, consider that the standard Gibbs energy of formation (∆G ̊f) of H2O (l) is –237.20 kJ/mol. Use this information to calculate the equilibrium constant for the decomposition of water at 298 K:

2 H2O (l) ⇄ 2 H2 (g) + O2 (g)

a) 7.0 x 10 –84

b) 2.6 x 10 –42

c) 0.91

d) 3.8 x 1041

e) 1.4 x 1083