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: For the reaction 2 SO3(g) → 2 SO2(g) + O2(g) ∆H◦r = +198 kJ·mol−1 at 298 K. Which statement is true for this reaction? 1. The reaction will not be spontaneous at any temperature. 2. The reaction will not be spontaneous at high temperatures. 3. ∆G◦r will be negative at high temperatures.  4. ∆G◦r will be positive at high temperatures. 5. The reaction is driven by the enthalpy.

Problem

For the reaction

2 SO3(g) → 2 SO2(g) + O2(g)

∆Hr = +198 kJ·mol−1 at 298 K. Which statement is true for this reaction?

1. The reaction will not be spontaneous at any temperature.

2. The reaction will not be spontaneous at high temperatures.

3. ∆Gr will be negative at high temperatures. 

4. ∆Gr will be positive at high temperatures.

5. The reaction is driven by the enthalpy.