1. CHAPTER 19: FIGURE 19A.2
PHYSICAL CHEMISTRY: THERMODYNAMICS, STRUCTURE, AND CHANGE 10E | PETER ATKINS | JULIO DE PAULA
© W. H. FREEMAN AND COMPANY
PHYSICAL CHEMISTRY: QUANTA, MATTER, AND CHANGE 2E| PETER ATKINS| JULIO DE PAULA | RONALD FRIEDMAN
© W. H. FREEMAN D COMPANY

2. CHAPTER 19: FIGURE 19A.6
PHYSICAL CHEMISTRY: THERMODYNAMICS, STRUCTURE, AND CHANGE 10E | PETER ATKINS | JULIO DE PAULA
© W. H. FREEMAN AND COMPANY
PHYSICAL CHEMISTRY: QUANTA, MATTER, AND CHANGE 2E| PETER ATKINS| JULIO DE PAULA | RONALD FRIEDMAN
© W. H. FREEMAN D COMPANY

3. Transport Properties in Liquids
Situation in liquids is qualitatively different from a gas, a certain amount of energy is necessary just to move a molecule  activation energy Ea to escape the interaction with its neighbors (e.g. by breaking H-bonds).
probability of a molecule having Ea (i.e. able to move)
mobility of a particle inversely prop. to viscosity  of the liquid   viscosity of a liquid decreases with increasing T

4. Transport properties of electrolyte solutions
Conductance G: the inverse of electrical resistance R of a solution
where A = sample cross sectional area;
l = sample length;
e = electrical conductivity (do not confuse with compressibility or thermal conductivity) [Ge] = S (Siemens) = -1 = CV-1s-1 [e] = Sm-1
Molar conductivity m = e/c where c = molar concentration of electrolyte [m] = Sm2mol-1; typical values m  102 Sm2mol-1

5. Transport properties of electrolyte solutions
Kohlrausch Law:
Note:
Kohlrausch law is empirical, works best at low concentrations and for strong electrolytes
m0 is the limiting molar conductivity (i.e. m for c  0) m0 = ++ + -- (law of independent migration of ions) where +/- is the number of cations/anions per electrolyte unit, +/- is the limiting molar conductivity of the cations/anions