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: For the process O2 (g) → 2 O (g), ΔH ° = + 498 kJ. What would be predicted for the sign of ΔSrxn   and the conditions under which this reaction would be spontaneous? ΔSrxn                             Spontaneous             a)     positive            at low temperatures only             b)     positive            at high temperatures only             c)     negative           at high temperatures only             d)     negative           at low temperatures only

Problem

For the process O(g) → 2 O (g), Δ° = + 498 kJ. What would be predicted for the sign of ΔSrxn   and the conditions under which this reaction would be spontaneous?

ΔSrxn                             Spontaneous

            a)     positive            at low temperatures only

            b)     positive            at high temperatures only

            c)     negative           at high temperatures only

            d)     negative           at low temperatures only