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Ch.1 - Chemical Tools: Experimentation & Measurement

Ch.2 - Atoms, Molecules & Ions

Ch.3 - Mass Relationships in Chemical Reactions

BONUS: Lab Techniques and Procedures

BONUS: Mathematical Operations and Functions

Ch.4 - Reactions in Aqueous Solution

Ch.5 - Periodicity & Electronic Structure of Atoms

Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory

Ch.7 - Covalent Bonding and Electron-Dot Structures

Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure

Ch.9 - Thermochemistry: Chemical Energy

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Ch.11 - Liquids & Phase Changes

Ch.12 - Solids and Solid-State Materials

Ch.13 - Solutions & Their Properties

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Ch.15 - Chemical Equilibrium

Ch.16 - Aqueous Equilibria: Acids & Bases

Ch.17 - Applications of Aqueous Equilibria

Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium

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Ch.22 - The Main Group Elements

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Chapter 18, Problem 124d

Consider the Haber synthesis of gaseous NH₃ (∆H°_f = -46.1 kJ/mol; ∆G°_f = -16.5 kJ/mol: (d) What are the equilibrium constants K_p and K_c for the reaction at 350 K? Assume that ∆H° and ∆S° are independent of temperature.

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Chapter 18, Problem 124d

Consider the Haber synthesis of gaseous NH3 (∆H°f = -46.1 kJ/mol; ∆G°f = -16.5 kJ/mol: (d) What are the equilibrium constants Kp and Kc for the reaction at 350 K? Assume that ∆H° and ∆S° are independent of temperature.

Consider the Haber synthesis of gaseous NH₃ (∆H°_f = -46.1 kJ/mol; ∆G°_f = -16.5 kJ/mol: (d) What are the equilibrium constants K_p and K_c for the reaction at 350 K? Assume that ∆H° and ∆S° are independent of temperature.