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: A large part of the driving force in a thermite reaction is based on the stability of aluminum oxide, as reflected in ΔH° of the following reaction: 2Al (s) + 3/2 O2 (g) → Al2O3 (s) ΔH° =  - 1669.8 k

Problem

A large part of the driving force in a thermite reaction is based on the stability of aluminum oxide, as reflected in ΔH° of the following reaction:

2Al (s) + 3/2 O(g) → Al2O(s) ΔH° =  - 1669.8 kJ/mol

 

If 27 g of aluminum reacts with oxygen to form Al 2O3(s), how much heat is released assuming the reaction goes to completion?