Ch.14 - Chemical EquilibriumSee 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

Equilibrium Expressions

See all sections
Sections
Chemical Equilibrium
ICE Chart
Le Chatelier's Principle
The Reaction Quotient
Additional Practice
Equilibrium Expressions

Solution: Consider the following reaction and its equilibrium constant:                FeO(s) + CO(g) ⇌ Fe(s) + CO2(g)          Keq = 0.67        If the equilibrium concentration of CO is measured at 0.40 M, what is the equilibrium concentration of CO 2?        A)  0.40 M    B)  1.1 M    C)  0.67 M    D)  0.27 M    E)  1.7 M  

Problem

Consider the following reaction and its equilibrium constant:

                FeO(s) + CO(g) ⇌ Fe(s) + CO2(g)          Keq = 0.67

        If the equilibrium concentration of CO is measured at 0.40 M, what is the equilibrium concentration of CO 2?

        A)  0.40 M    B)  1.1 M    C)  0.67 M    D)  0.27 M    E)  1.7 M