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Lecture

EquilbriumLecture Notes
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Department
Chemistry
Course
CHEM 112
Professor
John Carran
Semester
Fall

Description
W13L1 – Principles of Chemical Equilibrium • Note: most reactions are at equilbrium • Q = K not at equilibrium Equilibrium displays all of these characteristic: • Closed system – nothing is entering or leaving the system • System shows no macroscopic evidence of change • Reached through spontaneous process • Dynamic • Constant temperature – same equilibrium constant will be obtained regardless of the direction from which it was approached Even though a reaction is at equilibrium, meaning both a forward and reverse reaction exists, the equilibrium constant will be different if they are written out separately Reactions can wither appear to go to completion, seem to go partially, or “don’t seem to go at all. “ In each case, equilibrium will eventually be reached (may take a very long time) Types of equilibrium Systems: • Homogenous gas phase system – all species are at a gaseous phase • Heterogeneous mixtures – mixtures of solid/gas or solid/aqueous s
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