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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

Ch.21 - Nuclear Chemistry

Ch.22 - Chemistry of the Nonmetals

Ch.23 - Transition Metals and Coordination Chemistry

Ch.24 - The Chemistry of Life: Organic and Biological Chemistry

Brown - Chemistry:The Central Science 14th Edition

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Chapter 5, Problem 44d

Consider the following reaction: 2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252.8 kJ (d) How many kilojoules of heat are released when 38.5 g of CH₄(g) reacts completely with O₂(g) to form CH₃OH(g) at constant pressure?

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Chapter 5, Problem 44d

Consider the following reaction: 2 CH3OH(g) → 2 CH4(g) + O2(g) ΔH = +252.8 kJ (d) How many kilojoules of heat are released when 38.5 g of CH4(g) reacts completely with O2(g) to form CH3OH(g) at constant pressure?

Consider the following reaction: 2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252.8 kJ (d) How many kilojoules of heat are released when 38.5 g of CH₄(g) reacts completely with O₂(g) to form CH₃OH(g) at constant pressure?