Table 1.

Basic thermodynamics of molecular interactions

ΔG = ΔGo + RT ln Q	Equation 1.1
$Q=\frac{f(\text{Concentrations}\text{of}\text{products})}{f(\text{Concentrations}\text{of}\text{reactants})}$ΔGo =−RT ln Ka	Equation 1.2
ΔG =ΔH − TΔS	Equation 1.3
$\mathrm{\Delta }{H}_{vH}=-R\frac{\delta ln{K}_a}{\delta (1/T)}$	Equation 1.4
$\mathrm{\Delta }{C}_p={\left(\frac{\delta \mathrm{\Delta }H}{\delta T}\right)}_P$	Equation 1.5
ΔH (T) =ΔH (TR) + ΔCp (T − TR)	Equation 1.6
$\mathrm{\Delta }S(T)=\mathrm{\Delta }S(T_R)+\mathrm{\Delta }{C}_{p}ln\left(\frac{T}{T_R}\right)$	Equation 1.7
$\mathrm{\Delta }G(T)=\mathrm{\Delta }H(T_R)-T\mathrm{\Delta }S(T_R)+\mathrm{\Delta }{C}_p\left\{(T-T_R)-Tln\left(\frac{T}{T_R}\right)\right\}$	Equation 1.8

ΔG^o, standard Gibbs free energy change; K_a, equilibrium binding constant (or binding affinity); ΔG, Gibbs free energy change; Q, reaction quotient; ΔH, enthalpy change; ΔS, entropy change; ΔH_vH, van’t Hoff enthalpy change; ΔC_p, heat capacity change; R, gas constant equal to 8.31451 J/K.mol; T, temperature of interest; T_R, arbitrary reference temperature. Description of the thermodynamic parameters and their interrelationship is provided in the text.