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: What mass of iron(II) oxide must be used in the reaction given by the equation below to release 28.8 kJ? 6FeO (s) + O2 (g) = > 2Fe3O4 (s)    ΔH° = -635 kJ Calculate your answer in g. Enter it with

Problem

What mass of iron(II) oxide must be used in the reaction given by the equation below to release 28.8 kJ? 

6FeO (s) + O2 (g) = > 2Fe3O4 (s)    ΔH° = -635 kJ 

Calculate your answer in g. Enter it with two decimal places and no units.