Table 2. Thermodynamics parameters of formation of binary complexes between MtSK and substrate(s) or product(s).
| KD (µM) | ΔH (kcal mol−1) | ΔS (cal mol−1 K−1) | ΔG (kcal mol−1) | -TΔS (kcal mol−1) | |
| SKH 283.15 K, Hepes | 45 (±13) | 0.66 (±0.04) | 22.2 (±6.5) | −5.6 (±1.6) | −6.2 (±1.8) |
| SKH 298.15 K, Hepes | 181 (±15) | −4.6 (±0.2) | 1.8 (±0.2) | −5.1 (±0.4) | −0.54 (±0.05) |
| SKH 313.15 K, Hepes | 235 (±9) | −8.9 (±0.1) | −11.9 (±0.4) | −5.2 (±0.2) | 3.7 (±0.1) |
| SKH 298.15 K, Pipes | 135 (±8) | −3.5 (±0.1) | 5.7 (±0.3) | −5.2 (±0.3) | −1.7 (±0.2) |
| SKH 298.15 K, Imidazole | 396 (±47) | −6.4 (±0.4) | −6.0 (±0.7) | −4.6 (±0.2) | 1.8 (±0.1) |
| ATP | 196 (±29) | −5.1 (±0.3) | −0.15 (±0.02) | −5.1 (±0.8) | 0.044 (±0.007) |
| ADP | 562 (±20) | −12.4 (±0.2) | −27 (±1) | −4.4 (±0.2) | 7.9 (±0.2) |
KD represents the equilibrium dissociation constant, ΔH is the binding enthalpy, ΔS is the binding entropy, ΔG is the Free Gibbs energy, and –TΔS is the negative term for temperature (in Kelvin) times binding entropy.