Peroxydisulfate and Peroxymonosulfate

The iron(III)-catalyzed oxidation of hydrazine with S20 involves formation of mixed hydrazine-peroxydisulfate iron(III) complexes [equations (21)-(23)], with values for the rate constants k and k2 of 

2x10 s and 4.9x10 s, respectively, at 45°C and 0.1 Af ionic strength. The protonated complex [FeS20g(N2H4)(N2Hs)] was also 

Oxidation of VO by HSO5 has a simple rate law [equation (28)] with /t = 12.8M s and A// = 12 kcal mol and A5 = -11 cal K mol and the mechanism was shown to involve SO4 radicals using cerium(III) and azide as radical traps. The clean behavior of HSOJ 

Oxidations of a number of metal ion species by fluoroxysulfate, S04F involve reaction (29) in the rate-determining step with a second-order rate constant of 1.3 x 10 M s at 17 C and A/7 6.1 kcalmoF and A5 -23 cal K moF. In the absence of Ag , the reactions are slow and complex. 

Although not a reaction of a peroxy compound, the Ag -catalyzed oxidation of H2O by Ce(IV) is included because it involves production of Ag(II), the active H2O oxidant, by reaction with CeOH with a second-order rate constant of 4.0 x s at 30°C.  

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