volumrtric equilibrium concentration of solute in liquid surface, measured ar temperature and prt:s>ure of experiment. dimensio:iles> = concentration of solute in bulk of liquid. g.-mole 'cc. = value of (,, a t time / I and t?. rejpecrively. g.-mole 'cc. = volume of ga\. measured ar temperature and pressure of exlieriincnr. absorbed in time interval zc, cc. = tip to tip lcng1h of stirrer blade, cni. = dilluqivity of solute in liquid. s q . c m . sec. = c\;prrirnental cnergy of activation, cal. g.-mole = apparrnt experimental energy of activation. cal. ' g.-inole. = rncrgy of activation per methylene group. cal. 'g.mole = a1)parent energy of activation per meth>-lene group. cal. g.-mole = crier$!- of activation per methylene group based on efIrctive number of carbon atoms. cal. g.-mole = cnrrq). of activation d u e to head and terminal methyl $roup. cal. g.-mole .oefficirnt. erg. g.-mole t>-factor defined b>-Equation 9. dimensionless = mass trancfei coefficient in liquid phase in absence of jurfacrants. c m . 'sec. = m a \ < transfer coefficient in liquid phase in presence of surfactants. cm. 'sec. = total hydrodynamic resistance to mais transfer defined by Equation 3. sec. cm. = interfacial resistance to mass transfer d u e to presence of suriactauts. x c . 'cm. = interfacial resistance to mass transfer due to presence of potential energy barrier. sec. 'cm. = diameter of reaction vessel. c m . = molecular \\eight. g. g.-mole = rate of stirrinq. rev. sec. = rate of absorption. g.-mole '(sq. cm.)(sec.) = Reynold5 number = &\-d* ' Y = gas constant. erg '(OK.) (g.-mole) or cal.;'(OK.) X (g , -mole) = temperature. OK. or " C . =
t
I.' Le' Y
11
time. sec. or min. volume of liquid phase. cc. constant time interval. t ? - f l . sec. or min = kinematic viscosity. s q . c m . 'sec. = surface presjure of film. d>-ne cm. = = =
literature Cited
(1) Archer, R. .I.. La Mer, V. K.. J . Phys. Cheni. 59, 200 (1955). (2) Bainbridge. J.: Curry. F. H.; Goodridge. F.: unpublished kvork. (3) Barnrs, G.: La Mer, V. K.. "Retardation of 1:vaporation by Monolayers. Transport Processes.'' p. 9. .Academic Press, New l-ork. 1962. (4) Blank. Xi.,Ibid., p. 75, (5) Bricktiell, D . , Ph.D. thesis, King's College, University of Durham. England. 1960. (6) , , Brooks. .I. H., '.Retardation of Evaporation b y Monolavers. Transport Processes." p. 259. Academi'c Press. New York: 19 52. (7) Copeland. L. E., Harkins, \V. D., Bo)-d, G. E.. J . ChPm. Phys. 10, 357 (1942). (8) Davies. .I. T.. Iiideal. E. K . , "Interfacial Phenomena." p. 314, Academic Press, New York. 1961. (9) Downing. A. L., Truesdale, G. A,: J . '4ppl. Chem. 5 , 570 (1955). (10) Glasstone. S.,Laidler. K. J., Eyring. H.: "Theory of Rate Processes," pp, 510 ff.: McGraw-Hill, Ne\\ York, 1941. (11) Goodridge. F.. Rricknell, D.. Trans. Inst. Chern. Enyrs. (London) 40, 54 (1962).
(12) Goodridge. F.. Taylor. M. D.. unpublished work. (13) Guggenhrim. E. A , . Phii. .\fa
