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: The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system (the iron and oxygen).What can we conclude about the entropy change of the surroundings?

Solution: The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system (the iron and oxygen).What can we conclude about the entropy change of the surroundings?

Problem

The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system (the iron and oxygen).

What can we conclude about the entropy change of the surroundings?

Solution

We are asked what we can conclude about the entropy change of surroundings accompanying the rusting of iron which is spontaneous and is accompanied by a decrease of entropy of the system (the iron and oxygen).

 4Fe(s) + 3O2(g) → 2Fe2O3(s)

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