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: The thermite reaction, in which powdered aluminum reacts with iron oxide, is highly exothermic:2Al(s) + Fe2O3(s) → Fe(s) + 2Al2O3(s)Use standard enthalpies of formation to find ΔH˚rxn for the thermite reaction.Standard Thermodynamic Quantities for Selected Substances at 25 oC Reactant or productΔH˚f(kJ/mol)Al(s)0.0Fe2O3(s)-824.2Al2O3(s)-1675.7Fe(s)0.0

Problem

The thermite reaction, in which powdered aluminum reacts with iron oxide, is highly exothermic:
2Al(s) + Fe2O3(s) → Fe(s) + 2Al2O3(s)

Use standard enthalpies of formation to find ΔH˚rxn for the thermite reaction.

Standard Thermodynamic Quantities for Selected Substances at 25 o

Reactant or productΔH˚f(kJ/mol)
Al(s)0.0
Fe2O3(s)-824.2
Al2O3(s)-1675.7
Fe(s)0.0