Ch.6 - Thermochemistry WorksheetSee 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: Complete combustion of 1 mol of acetone (C 3H6O) liberates 1790 kJ:C3H6O (l) + 4 O 2 (g) → 3 CO2 (g) + 3 H2O (l)     ΔH° = -1790 kJUsing this information together with data from Appendix C, calculate the enthalpy of formation of acetone. 

Problem

Complete combustion of 1 mol of acetone (C 3H6O) liberates 1790 kJ:
C3H6O (l) + 4 O (g) → 3 CO(g) + 3 H2O (l)     ΔH° = -1790 kJ

Using this information together with data from Appendix C, calculate the enthalpy of formation of acetone.