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

Solution: At 25ºC, Kp ≈  1 x 10 -31 for the reactionN2(g) + O2(g) ⇌ 2NO(g)a. Calculate the concentration of NO, in molecules/cm 3, that can exist in equilibrium in air at 25ºC. In air, PN2 = 0.8 atm and PO2 = 0

Problem

At 25ºC, Kp ≈  1 x 10 -31 for the reaction

N2(g) + O2(g) ⇌ 2NO(g)

a. Calculate the concentration of NO, in molecules/cm 3, that can exist in equilibrium in air at 25ºC. In air, PN2 = 0.8 atm and PO2 = 0.2 atm.

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