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 298 K:2C (graphite) + O2 (g) → 2CO (g)  Delta H = -110.5 kJCalculate:Delta S(sys) J/KDelta S (surr) J/KDelta S (Univ) J/K

Solution: Consider the following reaction at 298 K:2C (graphite) + O2 (g) → 2CO (g)  Delta H = -110.5 kJCalculate:Delta S(sys) J/KDelta S (surr) J/KDelta S (Univ) J/K

Problem

Consider the following reaction at 298 K:

2C (graphite) + O2 (g) → 2CO (g)  Delta H = -110.5 kJ

Calculate:

Delta S(sys) J/K
Delta S (surr) J/K
Delta S (Univ) J/K

Solution

#1) To calculate for ΔSsys, we need the S˚ of each compound in the reaction.

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