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Chapter 15

CHEM 112 Chapter Notes - Chapter 15: Partial Pressure, Inert Gas, Endothermic Process


Department
Chemistry
Course Code
CHEM 112
Professor
John Carran
Chapter
15

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Week 13 Notes
15-2: Equilibrium constant Expression
Initially only the forward reaction occurs, but once some product is formed,
the reverse reaction starts to occur
Amount of reactants and products remains constant throughout time
Why do we apply equilibrium constants with activities?
oWhen gases do not obey ideal laws, equilibrium constants may vary
with pressure or temperature, but activities get rid of this
Numerator is product of activities
Denominator is reactants on left side
15-3: relationships involving equilibrium constants
relationship of K to the balanced chemical equation
When we reverse an equation, we invert the value of K
When we multiply the coefficients in a balanced equation by a common
factor, we raise the equilibrium constant to the corresponding power
When we divide the coeffcients in a balanced equation by a common factor,
we take the corresponding root of the equilibrium constant
Equilibrium vapour pressures are just values of kP
15-4: Magnitude of Equilibrium Constant
large value of K signifies forward reaction (goes to completion)
small value of K means the reaction does not occur to a significant extent
15-5: Predicting direction of net change
predicting direction of net change in establishing equilibroium is important because
1. at times we do not need detailed equilibrium calculations, but only a
qualitative description of the changes that occur n establishing equilibrium
fromma given set of initial conditions
2. in some calculations, it is helpful to determine direction of net change as a
first step
reaction quotient (Q): any set of initial activities in a reaction mixture as a ratio
Q=K means reaction is at equilibrium
Qc<kc net change occurs from left to right (direction of forward reaction)
QC>KC net change occurs from right to left (direction of reverse reaction)
15-6: Le Chateliers Principle
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