Calorimetry is recognized(1-8) as a noninvasive, nondestructive method for the determination of both the thermodynamic and the kinetic parameters associated with chemical reactions. The most immediate applications of the technique have been found in the determination of long-term stability data particularly for pharmaceuticals. However, the methods proposed required that calorimetric data (thermal power, Phi, watts recorded as a function of time) be analyzed iteratively to obtain the order of the reaction n, the rate constant k, and the enthalpy change of reaction Delta H-R. A necessary assumption in this process was that all of the sample placed into the calorimeter would react. This is obviously a severe constraint for the flexibility and application of the method. This paper reports a significant extension of the procedure that allows direct calculation of all of the above parameters. Moreover, the equations that are developed permit the determination of the actual quantity of the sample placed into the calorimeter that will react. Indeed, for successful determination of the desired kinetic, thermodynamic, and equilibrium parameters, it is not necessary, in principle, to have any knowledge about a sample other than its total mass. It is possible to determine, in addition to II, k, and Delta H-R, the equilibrium constant K for the reaction studied together with the associated values of the Gibbs function and entropy changes Delta (R)G and Delta S-R. Moreover, because the reaction is to be studied over a temperature range, the activation energy E-a is also accessible.