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

Equilibrium Expressions

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Sections
Chemical Equilibrium
ICE Chart
Le Chatelier's Principle
The Reaction Quotient
Additional Practice
Equilibrium Expressions

Solution: The methane used to obtain H2 for NH3 manufacture is impure and usually contains other hydrocarbons, such as propane, C3H8. Imagine the reaction of propane occurring in two steps:C3H8(g) + 3H2O(g) ⥫⥬

Problem

The methane used to obtain H2 for NH3 manufacture is impure and usually contains other hydrocarbons, such as propane, C3H8. Imagine the reaction of propane occurring in two steps:
C3H8(g) + 3H2O(g) ⥫⥬ 3CO(g) + 7H 2(g)
             K p = 8.175×1015 at 1200. K
CO(g) + H2O(g) ⥫⥬ CO2(g) + H2(g)
             K p = 0.6944 at 1200. K

(d) What percentage of the C3H8 remains unreacted?