Low-temperature heat capacities of the solid coordination compound trans-Cu(Gly)(2) (.) H2O(s) were measured by a precision automated adiabatic calorimeter over the temperature range from T) 78 K to T) 381 K. The initial dehydration temperature of the coordination compound was determined to be T-D 329.50 K, by analysis of the heat-capacity curve. The experimental values of the molar heat capacities in the temperature region of 78-328 K were fitted to a polynomial equation of heat capacities (C-p,C-m) with the reduced temperatures (X), [X = f(T)], by a least-squares method. The smoothed molar heat capacities and thermodynamic functions of the complex transCu( Gly) 2, H2O( s) were calculated based on the fitted polynomial. The smoothed values of the molar heat capacities and fundamental thermodynamic functions of the sample relative to the standard reference temperature 298.15 K were tabulated with an interval of 5 K. Enthalpies of dissolution of {Cu(Ac)(2) (.) H2O(s) + 2Gly(s)} [Delta H-s(m)Theta (1)] and HAc(l) [Delta H-s(m)Theta (2)] in 100.00 mL of 2 mol (.) dm(-3) HCl and trans-Cu(Gly)(2) (.) H2O(s) [Delta H-s(m)Theta (3)] in the solvent [ HAc(l) + 2 mol (.) dm(-3) HCl] at T = 298.15 K were determined to be Delta H-s(m)Theta (1) = (13.59 +/- 0.03) kJ(.) mol(-1), Delta H-s(m)Theta (2) = -(0.93 +/- 0.03) kJ (.) mol(-1), and Delta H-s(m)Theta (3) = -(14.64 +/- 0.02) kJ (.) mol(-1) by means of an isoperibol solution-reaction calorimeter. The standard molar enthalpy of formation of the compound was determined as: Delta H-f(m) (0)(trans-Cu(Gly)(2) (.) H2O, s, 298.15 K)) -(1251.6 +/- 1.0) kJ, mol(-1), from the enthalpies of dissolution and other auxiliary thermodynamic data through a Hess thermochemical cycle.