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: You are a member of a research team of chemists discussing plans for a plant to produce ammonia:   N2(g) + 3H2(g) ⇌ 2NH3(g)(a) The plant will operate at close to 700 K, at which K p is 1.00 x 10−4, an

Problem

You are a member of a research team of chemists discussing plans for a plant to produce ammonia:   

N2(g) + 3H2(g) ⇌ 2NH3(g)

(a) The plant will operate at close to 700 K, at which K p is 1.00 x 10−4, and employs the stoichiometric 1/3 ratio of N2/H2. At equilibrium, the partial pressure of NH 3 is 50. atm. Calculate the partial pressures of each reactant and Ptotal.