Ch.14 - Chemical EquilibriumWorksheetSee 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: At a certain temperature, K c equals 1.4 × 10 2 for the reaction:2 CO (g) + O 2 (g) ⇌ 2 CO 2 (g).If a 2.50-L flask contains 0.400 mol of CO 2 and 0.100 mol of O 2 at equilibrium, how many moles of CO

Problem

At a certain temperature, equals 1.4 × 10 2 for the reaction:

2 CO (g) + O (g) ⇌ 2 CO (g).

If a 2.50-L flask contains 0.400 mol of CO 2 and 0.100 mol of O 2 at equilibrium, how many moles of CO are also present in the flask?        

A) 0.169 mol           B) 0.028 mol                  C) 0.107 mol                              D) 0.0114 m