The Chemistry of Persulfate. I. The Kinetics and Mechanism of the Decomposition of the Persulfate Ion in Aqueous Medium¹

Hg0 absorption in potassium persulfate solution

“…This is probably due to the low KPS concentration. The energy of O-O bond is 33.5 kJ/mol and the activation energy is (121±12) kJ/mol (Price and Clifton, 1996), which is in reasonable agreement with 130 kJ/mol in previous work (Kolthoff and Miller, 1951) when potassium persulfate decomposed to radical 4 (SO ), − ⋅ whose potential was as high as 2.6 V (Kolthoff and Miller, 1951). Due to the high activation energy, reaction rate is quite slow at room temperature and acceptable rate can only be achieved over 50 °C.…”

“…The reactions of persulfate ions with various organic and inorganic compounds have been extensively studied (Kolthoff and Miller, 1951;House, 1962;Berlin, 1986). Persulfate oxidation is generally conducted under heat-, photo-or metal-catalyzed conditions because the oxidation rates can be greatly accelerated.…”

Adsorption of different amphiphilic molecules onto polystyrene latices

“…Lx(HEMA) is a styrene/NaSS and a hydrophilic polymer (2-hydroxyethylmethacrilatum) copolymer and it was synthesized following previous work [8,10]. The surface charge comes from the NaSS, but for several reasons [11,12], some weak acid groups are present on the surface. Subsequently, the surface charge is weakly dependent on the pH.…”

The Inhibitory and Catalyzing Effects of Different Materials on the Thermal Decomposition of Potassium Peroxydisulphate in Aqueous Solution at 70 OC

“…The thermal decomposition of potassium peroxydisulphate was the subject of study of many workers (Morgan & Christ, 1927;Fronaeus & Ostman, 1955;Kolthoff & Miller, 1951), all they suggested that the decomposition follows a first order kinetics. Early workers (Green & Mason, 1910) studying the thermal decomposition of potassium peroxydisulphate found that the decomposition in aqueous solution was accelerated by rise of temperature and depends on the concentration of solution.…”

“…Levi and Migliorini (Levi, Migliorini, & Gazz, 1963) observed that peroxydisulphate solutions which were stable at 35 O C are decompose catalytically by the hydrogen and the hydroxyl ions as well as platinum black and lead. Fronaeus and Ostman (Fronaeus & Ostman, 1955) and Kolthoff and Miller (Kolthoff & Miller, 1951) showed that the rate constant of the decomposition was independent of the ionic strength but in acid solution there is a negative salt effect. Vasudeva (Vasudeva, 1969) noticed that in aqueous solution potassium peroxydisulphate decomposes slowly at 60 O C and the decomposition shows auto-inhibition in the beginning and then follows first order kinetics.…”