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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

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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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Brown - Chemistry:The Central Science 14th Edition

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Chapter 15, Problem 24c

Consider the following equilibrium: 2 H₂(𝑔) + S₂( 𝑔) ⇌ 2 H₂S(𝑔) 𝐾_𝑐= 1.08×10⁷ at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H₂(𝑔) + 1/2 S₂( 𝑔) ⇌ H₂S(𝑔)

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Chapter 15, Problem 24c

Consider the following equilibrium: 2 H2(𝑔) + S2( 𝑔) ⇌ 2 H2S(𝑔) 𝐾𝑐 = 1.08×107 at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H2(𝑔) + 1/2 S2( 𝑔) ⇌ H2S(𝑔)

Consider the following equilibrium: 2 H₂(𝑔) + S₂( 𝑔) ⇌ 2 H₂S(𝑔) 𝐾_𝑐= 1.08×10⁷ at 700°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H₂(𝑔) + 1/2 S₂( 𝑔) ⇌ H₂S(𝑔)