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 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?

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?

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