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: A 1.000 L vessel is filled with 2.000 moles of N 2, 1.000 mole of H2, and 2.000 moles of NH3. N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g)When the reaction comes to equilibrium, it is observed that the concentration of H2 is 2.34 moles/L. What is the numerical value of the equilibrium constant Kc?

Problem

A 1.000 L vessel is filled with 2.000 moles of N 2, 1.000 mole of H2, and 2.000 moles of NH3

N(g) + 3 H(g) ⇌ 2 NH(g)

When the reaction comes to equilibrium, it is observed that the concentration of H2 is 2.34 moles/L. What is the numerical value of the equilibrium constant Kc?