This paper deals with an experimental batch mode study of a chemical homogeneous reaction: the dichromate-catalysed hydrogen peroxide decomposition. The thermodynamic properties and the kinetic parameters of the reaction are simultaneously determined using a calorimetric approach. Various batch-operating modes (adiabatic, isoperibolic, or differential thermal analysis) are compared and it is shown that the determined parameters do not depend on the operating mode. A complete kinetic law is proposed. The reaction rate constant is assumed to follow the Arrhenius rate law. The Arrhenius parameters are determined as frequency factor k(o)= 1.39 x 10(9) s(-1) and activation energy E=54.9 kJ mol(-1). The measured enthalpy of reaction is Delta(r)H=-94 kJ mol(-1). The reaction order is between 0 and 2 in hydrogen peroxide according to operating conditions and depends linearly on the initial dichromate concentration. The reaction can be managed by two parameters: on one hand the released reaction heat directly depends on the hydrogen peroxide concentration, and on the other hand, the kinetic rate can be increased in increasing the dichromate concentration. (C) 2005 Elsevier B.V. All rights reserved.