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Ch.1 - Introduction: Matter, Energy, and Measurement

Ch.2 - Atoms, Molecules, and Ions

Ch.3 - Chemical Reactions and Reaction Stoichiometry

BONUS: Lab Techniques and Procedures

BONUS: Mathematical Operations and Functions

Ch.4 - Reactions in Aqueous Solution

Ch.5 - Thermochemistry

Ch.6 - Electronic Structure of Atoms

Ch.7 - Periodic Properties of the Elements

Ch.8 - Basic Concepts of Chemical Bonding

Ch.9 - Molecular Geometry and Bonding Theories

Ch.10 - Gases

Ch.11 - Liquids and Intermolecular Forces

Ch.12 - Solids and Modern Materials

Ch.13 - Properties of Solutions

Ch.14 - Chemical Kinetics

Ch.15 - Chemical Equilibrium

Ch.16 - Acid-Base Equilibria

Ch.17 - Additional Aspects of Aqueous Equilibria

Ch.18 - Chemistry of the Environment

Ch.19 - Chemical Thermodynamics

Ch.20 - Electrochemistry

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Ch.22 - Chemistry of the Nonmetals

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Brown - Chemistry:The Central Science 14th Edition

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Chapter 19, Problem 89

The reaction 2 Mg(s) + O₂(g) ⟶ 2 MgO(s) is highly spontaneous. A classmate calculates the entropy change for this reaction and obtains a large negative value for ΔS°. Did your classmate make a mistake in the calculation? Explain.

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Chapter 19, Problem 89

The reaction 2 Mg(s) + O2(g) ⟶ 2 MgO(s) is highly spontaneous. A classmate calculates the entropy change for this reaction and obtains a large negative value for ΔS°. Did your classmate make a mistake in the calculation? Explain.

The reaction 2 Mg(s) + O₂(g) ⟶ 2 MgO(s) is highly spontaneous. A classmate calculates the entropy change for this reaction and obtains a large negative value for ΔS°. Did your classmate make a mistake in the calculation? Explain.