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: O2 and CH4 react according to the following unbalanced chemical equation: O2 + CH4 → __CO + __H2 Given 2.15 g of O2 and 2.12 g of CH4, answer the following questions: (For the calculations, provide an

Problem

O2 and CH4 react according to the following unbalanced chemical equation: 

O2 + CH4 → __CO + __H2 

Given 2.15 g of O2 and 2.12 g of CH4, answer the following questions: (For the calculations, provide answers with 3 significant figures.) 

1. Balance the chemical equation using the lowest integer coefficients. 

__O2 + __CH4 → CO + H2

2. Calculate the mass (in g) of the excess reagent remaining after the reaction is complete. 

3. Calculate the theoretical yield of CO (in g) from the reaction. 

4. Determine the percent yield of CO if 3.05 g of CO is actually produced from the reaction. 

(Please do NOT include in your answer.)

5. What is the limiting reagent?