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: Be sure to answer all parts.Methanol (CH4O), which is used as a fuel in high-performance racing cars, burns in the presence of O2 to form CO2 and H2O. The molar masses for all substances are given und

Problem

Be sure to answer all parts.

Methanol (CH4O), which is used as a fuel in high-performance racing cars, burns in the presence of O2 to form CO2 and H2O. The molar masses for all substances are given under the balanced equation. 

2CH4O (l)       +   3O 2 (g)         →   2CO 2 (g)        +  4H 2O(g) 

32.04 g/mol       32.00 g/mol       44.01 g/mol        18.02 g/mol 

a. What is the theoretical yield of CO 2 from 35.0 g of methanol? 

b. What is the percent yield of CO 2 if 26.8 g of CO 2 are formed?