Low-temperature heat capacities of the solid coordination compound Cr(C6H4NO2)(3)(s) have been measured by a precision automated adiabatic calorimeter over the temperature range T = 78 K to T = 391 K. The experimental values of the molar heat capacities in the temperature region 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 Cr(C6H4NO2)(3)(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 are tabulated with an interval of 5 K. Enthalpies of dissolution of {3C(6)H(5)NO(2)(s)} [Delta H-d(m)circle minus(1)] and Cr(C6H4NO2)(3)(s) [Delta H-d(m)circle minus(3)] in 100.00 mL of 0.1 mol . dm(-3) HCI and {Cr(OH)(3)(s)} [Delta H-d(m)circle minus(2)] in 100.00 mL of 0.1 mol . dm(-3) HCI solution containing certain amounts of nicotinic acid (named as solution A,) at T = 298.15 K were, respectively, determined to be [(14.44 +/- 0.14), -(34.47 +/- 0.26), and -(25.74 +/- 0.13)] kJ.mol(-1) by means of an isoperibol solution reaction calorimeter. The enthalpy change Delta H-r(m)(5) of the designed solid-state coordination reaction of Cr(OH)(3)(s) with nicotinic acid can be calculated as Delta H-r(m)(5) = (52.04 +/- 0.52) kJ.mol(-1) in accordance with a thermochemical cycle and the experimental results. The standard molar enthalpy of formation of the compound was determined as Delta H-f(m)circle minus[Cr(C6H4NO2)(3), s, 298.15 K] = -(1189.6 +/- 2.8) kJ.mol(-1), from the enthalpies of dissolution and other auxiliary thermodynamic data.