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

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

Solution: Consider the reaction: 2NH3 (g) ⇌ N2 (g) + 3H2 (g) Select the equilibrium constant expression. (A) Kc = [NH3]2/[N2][H2]3 (B) Kc = [N2]2/[H2][NH3] (C) Kc = [N2][H2]3/[NH3]2 What is the numerical value


Consider the reaction: 

2NH3 (g) ⇌ N2 (g) + 3H2 (g) 

Select the equilibrium constant expression. 

(A) Kc = [NH3]2/[N2][H2]3 

(B) Kc = [N2]2/[H2][NH3

(C) Kc = [N2][H2]3/[NH3]2 

What is the numerical value of Kc for the reaction if the concentrations at equilibrium are 0.19 M NH3, 5.0 M N2, and 0.60 M H2

Express your answer using two significant figures.