Comparing
Rate Law, Equilibrium Expression, Acid/Base Equilibrium Expression
and Solubility
Product
Constant |
Expression and Others |
What is not in the expression |
Factors that affect the constant |
Factor that affect the |
Manipulating multiple equations |
Rate |
Rate=k[A]a
[B]b (Rate Law) Exponents need to be determined experimentally |
Products |
Temperature Catalyst (think Arrhenius equation, activation energy and kinetics/
orientation) |
Rate Physical state Concentration Temperature Catalyst |
Reverse the reaction =1/k Add reactions we get a new k |
Equilibrium constant |
Keq =[C]c
[D]d [A]a
[B]b (Kc or Kp see
related equations) Exponents found by coefficients |
Solids and liquids (for aqueous and gas reactions) |
Temperature Not catalyst because equal both directions |
Equilibrium Position shifts according to Le Chatelier’s Principle Temperature Concentrations Pressure for gases by changing volume Not catalyst because effects are equal in both directions |
Reverse reaction = 1/K Double the all the coefficients K2 Triple K3 etc. Add reactions multiply K’s |
Acid/ Base constant |
Ka or Kb =[C]c
[D]d [A]a [B]b Exponents found by coefficients |
Solids and liquids (for aqueous and gas reactions) |
Temperature |
Equilibrium Position shifts according to Le Chatelier’s Principle Temperature Concentrations Not catalyst because equal effects in both directions |
|
Related Equations for
Rate, Equilibrium, and Acid Base Equilibrium
Rate Integrated rate law graphs can determine
rate order. Integrated rate laws are used to determine how
concentrations change with time. |
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Order |
Rate
Law |
Integrated
Rate Equation |
Equation
in form y=mx+b |
Linear
Plot |
Slope |
Units
for k |
Half
life |
|
0 |
rate
= k |
[A]0 -
[A]t = kt |
[A]t = -kt + [A]0 |
[A]
vs. time |
-k |
M
/ s |
t½ = [Ao] / 2k |
|
1 |
rate
= k [A] |
ln
([A]t/[A]0) = - kt or [A]t=[A] 0ekt |
ln[A]t = -k t + ln[A]0 |
ln
[A] vs. time |
-k |
s-1 |
t½ = 0.693 / k |
|
2 |
rate
= k [A]2 |
(1/[A]t)
- (1/[A]0) = kt |
1/[A]t = kt + 1/[A]0 |
(1/[A])
vs. time |
k |
M-1 s-1 |
t½ = 1 / k
[Ao] |
|
Arrhenius equation k = Ae-Ea/RT |
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Equilibrium |
Kc
= [C]c [D]d Kp = Pcc PDd [A]a [B]b
PAa PBb Kp=Kc(RT)Δn |
Le Chatelier note: Remember solids or liquids are not in the
equilibrium expression and do not affect equilibrium. Gasses not in reaction do not affect
equilibrium at constant volume. |
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Acid Base |
Kw = 1x10-14 Kw=Ka(Kb) pH+pOH=14 |
|
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