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

Solution: Consider the following reaction at equilibrium: 2CO2 (g) <---> 2CO (g) + O2 (g) ΔH° = -514 kJ Le Chatelier's principle predicts that adding O2 (g) to the reaction container will __________. a

Problem

Consider the following reaction at equilibrium:

2CO2 (g) <---> 2CO (g) + O2 (g) ΔH° = -514 kJ

Le Chatelier's principle predicts that adding O2 (g) to the reaction container will __________.

a. decrease the partial pressure of CO2 (g) at equilibrium
b. decrease the value of the equilibrium constant
c. increase the partial pressure of CO2 (g) at equilibrium
d. increase the value of the equilibrium constant
e. increase the partial pressure of CO (g) at equilibrium