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: Given the thermochemical equation: 4 Fe(s) + 3 O2(g) ⟶ 2 Fe2O3(s)         ΔHrxn = –1652 kJ mol–1 What is the ΔH for the reaction when 500.0 g of Fe2O3 (molar mass = 160. g mol−1 ) is formed.A. –5162.5 kJ B. 2581 kJ C. 5162.5 kJ D. –2581 kJ E. –2065 kJ

Problem

Given the thermochemical equation: 4 Fe(s) + 3 O2(g) ⟶ 2 Fe2O3(s)         ΔHrxn = –1652 kJ mol–1 

What is the ΔH for the reaction when 500.0 g of Fe2O3 (molar mass = 160. g mol−1 ) is formed.

A. –5162.5 kJ 

B. 2581 kJ 

C. 5162.5 kJ 

D. –2581 kJ 

E. –2065 kJ

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