Table 1.
reaction | parameterb | model | experimentalc |
---|---|---|---|
KET (298 K) | 0.055(7) | 0.18(3) | |
ΔH°ET | 2.9(1) | 2.8(1) | |
ΔS°ET | 4.1(4) | 6(2) | |
FeII(TPP) + O2 ⇌ FeIII(TPP)() | KO2 (250 K, M−1)d | (2.7–6.4) × 104 | (0.205–11.5) × 102e |
ΔH°O2 | −9.5(1) | −l0.5(7)e | |
ΔS°O2 | −16.9(4) | −32 (3)e | |
FeIII(TPP)() + pTsOH → FeIII(TPP)(O2H•)+ + pTsO− | kPT (298 K) | 1.5(3)×103 M−1 s−1 | 2.0(9)f × 105 M−1 s−1 |
ΔH‡PT | 12.0(1) | ||
ΔS‡PT | −3.1(2) | ||
FeII(TPP) + O2 + pTsOH → FeIII(TPP)(O2H•)+ + pTsO−g | kcat (298 K, M−2 s−1) = KO2kPT | (2–20) × 105h | (3.2–6.4) × 105i |
Optimized values from COPASI analysis of data at 253–303 K, 50–100 mM pTsOH, 30–50 μM Fe(TPP). COPASI values and experimental equilibrium parameters are given with the uncertainty in parentheses representing 1 standard deviation.
values in kcal mol−1; ΔS° and ΔH° values in cal K−1 mol−1.
Direct experimental measurements of equilibrium parameters from optical spectra and van ′t Hoff analyses (sections I and II).
Values extrapolated from thermodynamic parameters from kinetic data (model) or lower-temperature equilibrium measurements (experiment).
The 95% confidence limits from a t test are for at 298 K, 0.21 to 110 M−1; for −9.6 to −11.8 kcal mol−1; and for −28 to −38 cal K−1 mol−1, SI Section 3.4).
Calculated as where was defined as the mean value, 5 M−1.
Chemical steps involved in defining the catalytic rate constant, kcat, determined electrochemically.
Calculated as
Calculated from foot-of-the-wave analysis, vide infra.