All thermal systems are subject to problems of thermal regulation. These can be understood through the use of thermochemical
systems, in particular for those in the liquid phase. A dynamic linear model was earlier applied to obtain both the reaction
enthalpy and the rate constant at constant temperature for the catalytic decomposition of hydrogen peroxide. This first model
did not yield a good fitting between the calculated and experimental data. The hypothesis that the rate constant was independent
of temperature was too strong.
In the present study, a more elaborate, non-linear model was developed, which takes into account the rate constant variations
as a function of temperature (Arrhenius law). This model allowed the activation energy to be determined. The calculated data
then successfully fitted the experimental data. The literature indicates that the first-order rate law is not valid for a
certain range of concentrations; the present model verified this.
The results of dynamic modelling confirm and increase the precision of results obtained in different ways. The developed model
is validated through these comparisons.