It is possible to predict the kinetics of a reaction by using temperature versus time data under adiabatic conditions. This method was used for the cytidine/acetic anhydride reaction using a RC1 Mettler Reaction Calorimeter.

The authenticity of the experimental adiabatic system was verified by determining the kinetic parameters of a known reaction (hydrolysis of acetic anhydride) and comparing them to literature values.

For example, the average experimental activation energy, heat of reaction, and ln k₀ values for the hydrolysis of acetic anhydride were 11.2 ±.5 kcal/gmole, -14.4 ± .2 kcal/gmole, and 12.74 ± .94 sec^-1, respectfully, while the average literature values were 12.0 ± 2.4 kcal/gmole, -14.3 ± .3 kcal/qmole, and 11.56 ± 1.47 sec^-1, respectfully. The reaction was first order.

The cytidine/acetic anhydride reaction (unknown system) was subjected to the same adiabatic analysis and the average experimental activation energy, heat of reaction, and ln k₀ values were 13.3 ± .2 kcal/gmole, -10.5 ± .1 kcal/gmole, and 15.68 ± .34 L/(gmole sec), respectfully.

To further verify the results for the unknown system,three isothernal runs were executed and sanples were analyzed for concentration by High Pressure Liquid Chronatography (HPLC). The concentration-time data were analyzed and an Arrhenius Plot was constructed yielding an activation energy of 13.2 kcal/ginole and a ln k₀ value of 15.14 L/(gTnole sec). The reaction was second order.