. Author manuscript; available in PMC: 2014 Dec 10.

Published in final edited form as: Biochemistry. 2013 Nov 22;52(49):8855–8865. doi: 10.1021/bi401364v

Table 2.

Extended Arrhenius analysis fit results (T₀ = 25°C)^b

Thermodynamic Term	Step 1		Step 2
	Forward	Backward	Forward	Backward
ΔH₀^‡ (kcal·mol⁻¹)	11.7 [11.0, 11.8]	22.8 [22.3, 23.6]	13.5 [13.1, 15.2]	25.2 [23.8, 25.4]
ΔC_p^‡ (cal·mol⁻¹K⁻¹)	−404 [−527, −349]	104 [40, 256]	−335 [−428, −23]	702 [640, 889]
ΔS_0,Min^‡ (cal·mol⁻¹K⁻¹)	108 [105, 108]	121 [120, 124]	114 [113, 120]	120 [116, 121]
ΔG_0,Max^‡ (kcal·mol⁻¹)	−20.4 [−20.4, −20.4]	−13.4 [−13.4, −13.3]	−20.6 [−20.7, −20.6]	−10.7 [−10.7, −10.6]

The thermodynamic terms ΔH₀^‡, ΔC_p^‡, ΔS_0,Minf^‡, and ΔG_0,Max^‡, an refer to the activation enthalpy, activation heat capacity, minimum activation entropy, and maximum activation free energy, respectively. The values of ΔH₀^‡ and ΔC_p^‡ are obtained by fitting the temperature-dependence of the kinetic rates (Table 1) to the extended Arrhenius equation (equation 1) using MATLAB. The values of ΔS_0,Min^‡ and ΔG_0,Max^‡ are obtained using ΔH₀^‡ in equation 2 and the relations in the materials and methods. 95% confidence intervals estimated using Monte Carlo analyses are shown in the brackets.