Molar heat capacities of 13 methyl esters of the linear carboxylic acids from methyl octanoate to methyl eicosanoate were measured from 5 K to 350 K. The derived thermodynamic functions S abs,m (T) and H m (T) -H(0) were calculated. A correlation function for the absolute entropy at 298.15 K was found to be S abs (n,298.15 K) ) {215.94 + 31.517n} J‚K -1 ‚mol -1 , with n being the number of carbon atoms in the parent carboxylic acid minus one. The heat capacity of the liquid phases in the temperature range of 250 K to 350 K can be described by C p (n,T) ) {103.16 + 16.273n + 0.04735n(T/K)} J‚K -1 ‚mol -1 , with a mean absolute percentage deviation of 0.3%.

Heat capacity measurements were made on n-nonadecane and n-eicosane from 10 K to 390 K with an adiabatic calorimeter. These measurements were used to calculate the entropy and the enthalpy relative to 0 K. The sum of the enthalpy of the solid-solid transition and of melting of n-nonadecane is 62659 ( 20 J‚mol -1 at the triple point, 305.00 K. The enthalpy of melting of n-eicosane was calculated to be 69922 ( 100 J‚mol -1 at the triple point, 309.65 K. The entropies were extrapolated from the liquid phase just above the melting point to 298.15 K and found to be respectively 715.8 and 748.1 J‚K -1 ‚mol -1 . The crystallization behavior of both compounds is discussed.