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

Solution: The equilibrium constant for the reaction below at 25°C is 4.8 x 10 -6. Calculate the equilibrium concentration (mol/L) of Cl2 (g) if the initial concentration of ICI (g) is 1.33 mol/L. There is no I2 or Cl2 initially present. 2 ICI (g) ⇌ I2 (g) + Cl2 (g)a.) 2.9 x 10 -3b.) 5.8 x 10 -3c.) 3.2 x 10 -6d.) 6.4 x 10 -6e.) 343

Problem

The equilibrium constant for the reaction below at 25°C is 4.8 x 10 -6. Calculate the equilibrium concentration (mol/L) of Cl2 (g) if the initial concentration of ICI (g) is 1.33 mol/L. There is no I2 or Cl2 initially present. 

2 ICI (g) ⇌ I2 (g) + Cl2 (g)

a.) 2.9 x 10 -3

b.) 5.8 x 10 -3

c.) 3.2 x 10 -6

d.) 6.4 x 10 -6

e.) 343