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: In an experiment to study the formation of HI(g),H2(g) + I2(g) ⥫⥬ 2HI(g)H2(g) and I2(g) were placed in a sealed container at a certain temperature. At equilibrium, [H 2] = 6.50×10−5 M, [I2] = 1.06×10−

Problem

In an experiment to study the formation of HI(g),
H2(g) + I2(g) ⥫⥬ 2HI(g)
H2(g) and I2(g) were placed in a sealed container at a certain temperature. At equilibrium, [H 2] = 6.50×10−5 M, [I2] = 1.06×10−3 M, and [HI] = 1.87×10−3 M. Calculate Kc for the reaction at this temperature.