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 reaction 2 C(s) + 2 H2(g) → C2H4(g)  ∆H°r = +52.3 kJ · mol−1 and ∆S°r =−53.07 J · K−1· mol−1 at 298 K. This reaction will be spontaneous at 1. no temperature.  2. temperatures below 985 K.

Problem

For the reaction

2 C(s) + 2 H2(g) → C2H4(g) 

∆H°r = +52.3 kJ · mol−1 and ∆S°r =−53.07 J · K−1· mol−1 at 298 K. This reaction will be spontaneous at

1. no temperature. 

2. temperatures below 985 K.

3. temperatures above 985 K.

4. temperatures below 1015 K.

5. all temperatures.