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 following reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g)Complete the following table. Assume that all concentrations are equilibrium concentrations in M. T (K)  [N2]left[ {{f{N}}_{f{2}} } ight][H2]left[ {{f{H}}_{f{2}} } ight][NH3]left[ {{f{NH}}_{f{3}} } ight]Kcleft[ {{f{K}}_{f{c}} } ight]5000.1150.1050.439  –5750.110–0.1309.67750.130  0.140  –0.0584  Find Kc at 500 K.

Problem
Consider the following reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Complete the following table. Assume that all concentrations are equilibrium concentrations in M.
 T (K)  [N2][H2][NH3]Kc
5000.1150.1050.439  
5750.1100.1309.6
7750.130  0.140  0.0584  


Find Kc at 500 K.