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: Consider the reaction shown below at 2200 °CN2 (g) + O2 (g) ↔ 2 NO (g)        K c = 0.0505A student adds 0.375 mol of N2 and 0.375 mol of O2 to a 2.50 L flask and then allows the reaction to come to equilibrium. What are the equilibrium concentrations of all reactants and products? 

Problem

Consider the reaction shown below at 2200 °C

N2 (g) + O2 (g) ↔ 2 NO (g)        K c = 0.0505

A student adds 0.375 mol of N2 and 0.375 mol of O2 to a 2.50 L flask and then allows the reaction to come to equilibrium. What are the equilibrium concentrations of all reactants and products?