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: Consider the equation carefully, and think about the sign of ∆S for the reaction it describes. NH4Br (s) → NH3 (g) + HBr (g) ∆H = +188.3 kJ. Which response describes the thermodynamic spontaneity of

Problem

Consider the equation carefully, and think about the sign of ∆S for the reaction it describes.

NH4Br (s) → NH3 (g) + HBr (g) ∆H = +188.3 kJ.

Which response describes the thermodynamic spontaneity of the reaction?

1. The reaction is spontaneous only at relatively high temperatures.

2. All responses are correct

3. The reaction is spontaneous at all temperatures.

4. The reaction is not spontaneous at any temperatures.

5. The reaction is spontaneous only at relatively low temperatures.