Henry's Law
Sgas=kh x Pgas
where Sgas=solubilty, Kh= henry's law constant (M/atm), and Pgas= partial pressure (atm)
Molarity
M=mol/L
Molality
m=moles solute/kg solvent
Percent by Mass
mass solute x 100/ mass solution
Parts per million
ppm= mass solute x 10^6/ mass solution
Parts by volume
Volume solute x multiplication factor/ volume solution
Where multiplication factor = 10^6, 10^9, etc...
mole fraction
Xsolute= n solute/ n solute + n solvent
mole percent
mole fraction(X) x 100%
Raoult's Law
Psolution= Xsolvent x Pdegreessolvent
Where Psolution= vapor pressure, Xsolvent= mole fraction, and Pdegreessolvent= vapor pressure
Vapor Pressure Lowering
DeltaP=i x Xsolute x Pdegreessolvent
Where i = van't hoff factor, Xsolute = mole fraction, and Pdegreessolvent = vapor pressure
Freezing Point Depression
Delta T= i x kf x m
Where i= Van't hoff factor, kf= freezing point constant, and m= molality
Boiling Point Elevation
Delta T= i x kb x m
Where i=Van't Hoff factor, kb= boiling point constant, and m= molality
Vapor pressure of a solution containing 2 volatile components
PA=XA + PdegreesA
PB=XB + PdegreesB
Ptotal= PA + PB
Osmotic Pressure
pi= iMRT
Where i= van't hoff factor, M= Molarity, R= .08206 L x atm/ mol x K, and T=K
Van't Hoff factor
i= moles of particles in solution/moles of formula units dissolved
Rate Reaction
For an equation aA + bB ---> cC + dD, the rate is defined as:
rate= 1/-a x Delta [A]/ Delta T = 1/-b x Delta [B]/Delta T = 1/c x Delta[B]/ Delta T = 1/d x Delta [D]/ Delta T
Rate Law for a single reactant
Rate = k [A]^n
Rate Law for a multiple reactant
Rate = K[A]^n[B]^m
Integrated Rate Law for zero-order
[A]= -kt + [A]0
units of k= M x s^-1
Integrated Rate Law for first-order
ln[A]= -kt + ln[A]0
units of k = s^-1
Integrated Law for Second-order
1/[A]= kt + 1/ [A]0
units of k = m^-1 x s^-1
Half Life for First-Order
t1/2= .693/k
.693=ln(2)
Half life for Zero-order
t1/2= [A]0/2k
Half Life for Second Order
t1/2= 1/ k[A]0
Arrhenius Equation/ Activation Energy
k= A e^-Ea/RT
Where k= constant, A= frequency factor, Ea=Activation Energy, R= 8.314J/mol x K, T=K
Linearized form of the Arrhenius Equation
lnk= -Ea/R x (1/T) + lnA
Two-point form of the Arrhenius Equation
ln(k2/k1)= Ea/R x (1/T1-1/T2)
Collision Theory from the Arrhenius Equation
k=pz x e^-Ea/RT
Where p= orientation factor, z= collision frequency (amount of collisions/unit of time)