Review
The examination is scheduled for Thurs., Dec 1. The exam will have two sections,
that is, it will follow a format similar to the last examination. During the problem
solving part, you will again be provided with a sheet of equations that you may need
to solve a particular problem but you may be asked to derive an eqn. in one or more
instance. There will be more eqns. than you need. You will be expected to know
basic equations like the ideal gas law. If you set up the problem correctly you will
get major credit.
The review sheets follow. They are words and concepts that should be very familiar
to you. As before, I will take the multiple choice questions from these sheets. Also
the problem solving will be problems based on concepts taken from problems
assigned for homework, given on a quiz, and listed on the review sheets. Look over
the sheets and ask questions about them on Tuesday.
Definitions: (The meanings of these words and phrases should be very familiar.
A = Ao + RTln aA
critical point
triple point
Chemical Potential
Phase Diagram
(phase 1) = (phase 2) etc
A(phase 1) = A(phase 2) etc
Colligative properties
boiling pt. elevation constant
vapor pressure
vapor pressure lowering
freezing pt. depression
boiling pt. elevation
i = moles particles/mole solute
osmosis, reverse osmosis
osmotic pressure
molecular weight determination
vapor pressure lowering
Freezing point depression constant
Equilibrium Constant
Kp, Kc, Keq
Pressure Dependence of Gibbs Free energy activity of a pure solid or pure liquid
activities and the equilibrium constant
Standard States
Std. states for pure solids or liquids
Solvent and solute standard states
Molarity
Molality
Biochemists std state
Activity coefficient
mean ionic activity
Debye-Huckel Equation
ionic strength
mean ionic activity coefficient
reaction quotient
G and the reaction quotient
Acid Dissociation Constant
Base Dissociation Constant
Van’t Hoff’s Eqn.
G at equilibrium
+
pH = -log[H ]
glycolytic pathway and glycolysis
metabolism
function of ATP
function of NADH
Le Chatelier’s Principle
physiological conditions
Metabolic Regulation
diffusion
Fick's 1st and 2nd Laws
viscosity
Stokes Law
Einsteins Relationship
Diffusion coefficient
root mean square displacement
non-Newtonian viscosity
sedimentation
ultracentrifuge
concentration gradient
frictional coefficient
thermal transport
fluid mosaic model
transmembrane potential
surfactants
hydrophillic
lipid bilayer
transition temperature
headgroup
active transport
simple diffusion
Equilibrium Dialysis
Protein binding site
Ka, association constant
Schatchard Eqn.
fractional saturation of sites
binding constant
protein
Donnan Effect
sodium potassium pump
flux
velocity gradient
lipids
membrane transport
amphiphilic molecules
hydrophobic
membranes
DTA and DSC
hydrocarbon tails
surface tension
passive transport
facilitated diffusion
fractional saturation of sites
Kd, dissociation constant
Intrinsic dissociation constant
Cooperative Binding
Double Reciprocal plot
identical binding sites
macromolecule
Donnan Potential
ATP hydrolysis
Calculations
Should be able to calculate osmotic pressure, molecular weight of solute, concentration
Calculation of colligative properties or the Molar Mass from the Colligative Properties
Use of the definition of the Chemical Potentials
Expression for the molar Gibbs free energy of a gas
Calculation of the Equilibrium Constant from Gorxn or the reverse of this.
Calculating the Temp dependence of the equilibrium constant
Use of LeChatliers Principle
Relationship between Kp, Kc write expression for K in activities or Kp in partial pressures
Equilibrium Constant Calculations using ICE or Henderson-Hasselbach
Equilibrium Constant and G for coupled Eqns
Calculation of the activities or concentrations of the species present at equilibrium
Calculate the Diffusion coefficient, the viscosity, the friction coefficient
Calculate the mean squared displacement based on diffusion, also the specific viscosity
Use of Debye Huckel, calculation of ionic strength, mean ionic activity,
Calculation of the mean ionic activity coefficient
Calculation of G at conditions other than at equilibrium
Calculation of Go and the equilibrium constant, and find it at other temps.
Structure of Membranes
Explain the Donnan Effect.
Understand equilibrium dialysis and the use of the Schatchard Eqn.
Relationship for  when transmembrane potential is present
Understanding of how detergents work, lipid bilayers
Know about transition temperatures in membranes
Equations and Constants
dE = TdS - P dV H=E+PV G=H-TS
A=E-TS dG = VdP - SdT + adna + bdnb
 = o + RT ln(p/po)
a = a* + RT lnxa
 = o + RT ln a Pb = xbKb
Pb=mKb'
Pa = xaPa*
Tf = iKf m
b= iKbm
*
 = iMRT
ya = Pa/P
P = xBPA
a = x
P=Pb* + (Pa*-Pb*)xa
*
P = Pa + Pb + Pc + Pd + ….
aA = pA/pA
F = C-P+2
o
o
o
o
 =  + RT ln a  =  + RT ln(P/P )
a = a + RT lnaa
a = a* + RT lnxa
o
o
RT ln(ain/aout) + ZFV =   = (r + + s - ) + v RTln a+- Kp = Kc (RT) n Po -  n
m+- = (m+r m-s )1 / v
v=r+s
m+- = m [rr ss ]1 / v
a+- = a+r a-s
a+- = +- m+- +- = (+r -s )1 / v
log +- = -/ z+z- / AI½ A = 0.509
2
o
o
o
I = ½ i zi (mi /m ) G =H -TSo Go = - RT ln(K) G = Go + RT lnQ
ln[K(T2)/K(T1)] = -o/R (1/T2 - 1/T1) <x2 >=2Dt <d2 > = 6Dt D = kT/f
f = 6r
Y[L] + KY = n[L] Y = ([PL]) /([P] + [PL]) Y/[L] = n/K - Y/K 1/Y = 1/n + k/(n [L])
Ki = ( i / (n-i+1))
R = 8.314 J/(mol K) R = 0.08206 L atm/(mol K) 1atm = 760 Torr 1 atm = 14.7 psi
1atm = 101325 Pa 1 bar = 105 Pa g = 9.81 m/s2 1L = 0.001 m3 K = oC + 273.15
k = 1.38 x 10- 2 3 J/K Nav = 6.022x102 3