Tn. Das et al., REDUCTION POTENTIAL OF THE TERT-BUTYLPEROXYL RADICAL IN AQUEOUS-SOLUTIONS, The journal of physical chemistry. A, Molecules, spectroscopy, kinetics, environment, & general theory, 102(1), 1998, pp. 280-284
Rate constants for oxidation of tert-butyl hydroperoxide anion (t-BuO2
-) by several oxidants were determined by pulse radiolysis. Rapid oxid
ation was found with N-3 . (4.4 x 10(8) L mol(-1) s(-1)) and . O- (2.6
x 10(8) L mol(-1) s(-1)), but others (Br-2(.-), I-2(.-), ClO2., CO3.-
, C6H5N(CH3)(2)(.+)) reacted much more slowly. Since the reduction pot
entials of these oxidants are much higher than that estimated for t-Bu
O2., the observed rate constants suggest that the self-exchange rate f
or t-BuO2./t-BuO2- is very slow and that it would be difficult to esta
blish rapid equilibrium by pulse radiolysis with a suitable redox pair
. Therefore, to determine the reduction potential for this peroxyl rad
ical, the forward and reverse rate constants for reaction 6, t-BuO2. Fe(CN)(6)(4-)reversible arrow t-BuO2- + Fe(CN)(6)(3-), were measured
independently. The forward rate constant was measured by kinetic spect
rophotometric pulse radiolysis in N2O-saturated solutions containing h
igh concentrations of N-3(-) (1 mol L-1), t-BuO2- (0.4 mol L-1), and v
arying concentrations of Fe(CN)(6)(4-) (0.012-0.036 mol L-1) at pH 13.
7. The rate constant k(6) was found to be 2.5 x 10(2) L mol(-1) s(-1).
Such a low rate constant was possible to measure by pulse radiolysis
only because the self-decay of t-BuO2. is very slow compared to those
of other peroxyl radicals. The reverse reaction rate constant was meas
ured by mixing the reactants and following the disappearance of Fe(CN)
(6)(3-) in the presence of spin traps to remove the peroxyl radicals f
rom the equilibrium. A rate constant of k(-6) = 1.4 x 10(-2) L mol(-1)
s(-1) was derived. By taking the reduction potential of Fe(CN)(6)(3-)
/Fe(CN)(6)(4-) as 0.459 V vs NHE for the conditions used in these expe
riments, we calculate E(t-BuO2./t-BuO2-) = 0.71 V and E(t-BuO2./t-BuO2
H) = 1.05 V at pH 7 and 1.47 V at pH 0. The rate constants for oxidati
on of Fe(CN)(6)(4-) and other compounds by various peroxyl radicals we
re then utilized for the estimation of the reduction potentials of the
se peroxyl radicals.