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 following reaction at constant P. Use the information here to determine the value of ΔSsurr at 298 K.   N2(g) + 2 O2(g) → 2 NO2(g) ΔH = +66.4 kJ   a) ΔSsurr = +223 J/K b) ΔSsurr = -223 J/K c) ΔSsurr = -66.4 J/K d) ΔSsurr = +2656 kJ/K  

Problem

Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 298 K.

 

N2(g) + 2 O2(g) → 2 NO2(g) ΔH = +66.4 kJ

 

a) ΔSsurr = +223 J/K

b) ΔSsurr = -223 J/K

c) ΔSsurr = -66.4 J/K

d) ΔSsurr = +2656 kJ/K