Iranian Journal of Catalysis (IJC) Kinetics investigation of the synthesis reaction of 2,3-dihydroquinazolin-4(1H)-ones in the presence of acetic acid as a catalyst Volume 4 (2014) Issue 4, December 2014 2024 02 03 Kinetics investigation of the synthesis reaction of 2,3-dihydroquinazolin-4(1H)-ones in the presence of acetic acid as a catalyst EN Sayeyd Mosatfa Habibi-Khorassani Department of Chemistry Faculty of Science University of Sistan and Baluchestan Zahedan, Iran P.O. Box: 98135-674 Malek Taher Maghsoodlou Chemistry Department, Faculty of Science, University of Sistan and Baluchestan, Zahedan, Iran Mehdi Shahraki Department of Chemistry Faculty of Science University of Sistan and Baluchestan Zahedan, Iran P.O. Box: 98135-674 Marjan Hashemi Shahri Department of Chemistry Faculty of Science University of Sistan and Baluchestan Zahedan, Iran P.O. Box: 98135-674 Jasem Aboonajmi Department of Chemistry, College of Sciences, Shiraz University, Shiraz 71454, Iran Tahere Zarei Department of Chemistry Faculty of Science University of Sistan and Baluchestan Zahedan, Iran P.O. Box: 98135-674 Journal Article 2024 02 03 Acetic acid has been applied as an efficient catalyst and a green solvent for the two–component condensation reaction consisting of benzaldehyde, 2-amino-benzamide. The advantages of this protocol was excellent yield, short reaction time, mild reaction conditions, higher availability, low costs, more environmentally friendly, lack of need for column chromatography and simple work-up procedure. In addition, based on the spectral data, the partial order with respect to each reactant was one. Furthermore, useful information regarding the mechanism of the reaction was obtained from studies of the effect of solvent, concentration and catalyst on the rate of the reaction. The results showed that the first step of the mechanism was a rate-determining step. In the studied temperature range, the second order rate constant (lnk1, lnk1/T) depended on reciprocal temperature was in good agreement with the Arrhenius and Eyring equations. These data provided the suitable plots for calculating the activation energy (Ea = 52.80 kJmol-1) and the related kinetic parameters (ΔG‡ = 63.74 kJmol-1, ΔS‡ = -54.22 Jmol-1 and ΔH‡ = 50.28 kJmol-1) of the reaction.