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

Solution: The two most abundant atmospheric gases react to a tiny extent at 298 K in the presence of a catalyst:         N 2(g) + O2(g) ⥫⥬ 2NO(g)            K p = 4.35×10−31(a) What are the equilibrium pressure

Problem

The two most abundant atmospheric gases react to a tiny extent at 298 K in the presence of a catalyst:
         N 2(g) + O2(g) ⥫⥬ 2NO(g)            K p = 4.35×10−31
(a) What are the equilibrium pressures of the three gases when the atmospheric partial pressures of O2 (0.210 atm) and of N2 (0.780 atm) are put into an evacuated 1.00-L flask at 298 K with the catalyst?