The radii of hydrated K+ and Li + ions (Stokes radius) are 0. 125 and 0.273 nm, respectively [20). In each composite membrane, P to K + ion is about two times as large as that to Li + ion below Te, being inversely proporlional to the radius of hydrated ion.This result indicates that the permeation characteristic is mainly controlled by the diffusion process because the ratio of diffusion coefficients for K + and Li + ions estimated by Stokes' equation of motion is comparable to the experimental ratio of P K + and P Li +. In contrast, P K + is almost equal to P Li + above Te in spite of a large difference between the radii of hydrated ions. Therefore, holes or vacancies with the sufficient size for diffusion of K + and Li + ions must be formed in the Iiposomes in a liquid crystalline state. Then, the magnitude of permeation of K + or Li + ions through liquid crystalline domain becomes comparable. The magnitude of P to cations for the cationic composite membrane (PYC/DOAB system) were greater nearly ten times as much as that for the anionic one (PYC/SDDP system) as shown in Fig. 12. Permeating ions are easily incorporated into the fix-charged membrane with an opposite sign. Furthermore, the mobility of the cation within the anionic composite membrane is lower than that within the cationic one, since the permeating cations interact with the fixed charge of the anionic membrane strongly. Therefore, P K + and P Li + for the anionic composite membrane were much less than those for cationic one because of the lower permeability of Cl ion and the strong interaction of the cation with didodecylphosphate anion.The reaction (1) has been studied at room temperature in an isothermal discharge flow reactor. Methylene-radicals and oxygen-atoms have been monitored with a Far-Infrared Laser Magnetic Resonance spectrometer. The rate constant of reaction (1) was evaluated from the pseudo first order decay of CH 2 in the presence of a large excess of O-atoms. The influence of side and consecutive reactions has been investigated in a computer simulation of the reaction system. -The final result for the rate constant of reaction (1) is k t (296 K) = (8.1 ± 3.0) . 10 13 cm 3/mol s .The experimental value is compared to theoretical predictions for the high pressure recombination rate constant of CH 2 and O.