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 formation of ammonia in two experiments. (a) To a 1.00-L container at 727°C, 1.30 mol of N 2 and 1.65 mol of H2 are added. At equilibrium, 0.100 mol of NH3 is present. Calculate the equil

Problem

Consider the formation of ammonia in two experiments. 

(a) To a 1.00-L container at 727°C, 1.30 mol of N 2 and 1.65 mol of H2 are added. At equilibrium, 0.100 mol of NH3 is present. Calculate the equilibrium concentrations of N 2 and H2, and find Kc for the reaction: 

2NH3(g) ⇌ N2(g) + 3H2(g) 

(b) In a different 1.00-L container at the same temperature, equilibrium is established with 8.34 x 10−2 mol of NH3, 1.50 mol of N2, and 1.25 mol of H2 present. Calculate Kc for the reaction: 

NH3(g) ⇌ 1/2N2(g) + 3/2H2(g) 

What is the relationship between the Kc values in parts (a) and (b)? Why aren’t these values the same?