Chapter 16: Equilibria Flashcards

1
Q

product favored reaction

A

once equilibrium is reached, there is a greater concentration of prodcuts than reactants

K > 1

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2
Q

equilibrium constant expression

A

Keq = [C]c [D]d / [A]a [B]b

for the rxn. aA + bB <–> cC + dD

*don’t include pure solids or pure liquids (water)

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3
Q

reactant favored reaction

A

once equilibrium is reached, there is a greater concentration of reactants than products

K < 1

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4
Q

Reaction Quotient, Q

A

Same as equilibrium constant expression, except the concentrations are not equilibrium concentrations

Q = K equilibrium

Q < K reactants must be converted to products to reach equilibrium

Q > K products must be converted to reactants to reach equilibrium

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5
Q

quadratic equation

A
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6
Q

method of successive approximations

A

100 x K < [A]0

When K is very small, you can remove x, b/c [A]0 - x is approximately equal to x.

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7
Q

equilibrium constants and stoichiometric coefficients

A

When stoichimoetric coefficients are multiplied by some factor, the equilibirum constant for the new expression is the old equilibrium constant raised to the power of the multiplication factor.

A Rxn and its reverse:

K2 = 1 / K1

Adding 2 equations:

multiply equilibrium constants

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8
Q

Le Chatelier’s Principle

Vol.

Temp.

A

Changing temp., concentration or volume (for a system with gases) will cause the system to change in such a manner as to reduce / counteract the effect of the change.

Change in vol:

Vol. decrease: (increased pressure) shifts toward side with less molecules in gas phase

Vol. increase: (decreased pressure) shifts toward side with larger # of gas molecules

No change in gas molecules: vol. change has no effect

Change in Temp.

Increase: endothermic direction

Decrease: exothermic direction

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9
Q

endothermic

A

heat is a “reactant”

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10
Q

exothermic

A

heat is a “product”

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11
Q

Kp = Kc(RT)change in number of moles

A

R = .08206

T = Kelvin temp.

change in number of moles of gas for the rxn. as written (moles of products - moles of reactants)

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