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: Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:[N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 x 10-18 M.2N2(g) + O2(g) ⇌ 2N2O(g)A) 2.2 x 10-19B) 4

Problem

Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows:

[N2]eq = 3.6 M, [O2]eq = 4.1 M, [N2O]eq = 3.3 x 10-18 M.

2N2(g) + O2(g) ⇌ 2N2O(g)

A) 2.2 x 10-19

B) 4.5 x 1018

C) 2.0 x 10-37

D) 5.0 x 1036

E) 4.9 x 10-17