Ch.3 - Chemical ReactionsWorksheetSee 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: Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2 Mg (s) + O2(g)      →       2 MgO (s) When 10.1 g of Mg reacts with 10.5 g

Problem

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:

2 Mg (s) + O2(g)      →       2 MgO (s)

 

When 10.1 g of Mg reacts with 10.5 g O2 , 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield and percent yield for the reaction.