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: Without doing any calculations, determine the sign of ΔSsurr for each of the following chemical reactions.a. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g), ΔH˚rxn = –2044 kJb. N2(g) + O2(g) → 2 NO(g), ΔH˚rxn = +182.6 kJc. 2 N2(g) + O2(g) → 2 N2O(g), ΔH˚rxn  = +163.2 kJd. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g), ΔH˚rxn = –906 kJ

Problem

Without doing any calculations, determine the sign of ΔSsurr for each of the following chemical reactions.
a. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g), ΔH˚rxn = –2044 kJ
b. N2(g) + O2(g) → 2 NO(g), ΔH˚rxn = +182.6 kJ
c. 2 N2(g) + O2(g) → 2 N2O(g), ΔH˚rxn  = +163.2 kJ
d. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g), ΔH˚rxn = –906 kJ