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
Additional PracticeSummary

Solution: Enter your answer in the provided box.Consider the reaction 2NO (g) + O2 (g) ⇋ 2NO2(g) At a certain temperature, an equilibrium mixture consists of 0.0220 mole O 2, 0.0410 mole NO, and 0.973 mole of N

Problem

Enter your answer in the provided box.

Consider the reaction 

2NO (g) + O2 (g) ⇋ 2NO2(g) 

At a certain temperature, an equilibrium mixture consists of 0.0220 mole O 2, 0.0410 mole NO, and 0.973 mole of NO2. Calculate Kp for the reaction, given that the total pressure is 0.200 atm.

Solution
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