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: At a certain temperature, the Kc of the reaction below is 1.5 x10 −11. If 0.10 mol N2 and 0.10 mol O2 are reacted together in a 1.00 L container, how much NO is present at equilibrium?N2 (g) + O2 (g) ⇌ 2 NO (g) Kc = 1.5x10−11A. 1.5x10−13 MB. 0.20 MC. 3.9x10−7 MD. 1.9x10−5 M

Problem

At a certain temperature, the Kc of the reaction below is 1.5 x10 −11. If 0.10 mol N2 and 0.10 mol Oare reacted together in a 1.00 L container, how much NO is present at equilibrium?
N2 (g) + O2 (g) ⇌ 2 NO (g) Kc = 1.5x10−11

A. 1.5x10−13 M

B. 0.20 M

C. 3.9x107 M

D. 1.9x10−5 M