The kinetic behavior of heterogeneous esterification of acetic acid with am
yl alcohol was investigated at temperatures from 303.15 K to 353.15 K over
an acidic cation exchange resin catalyst, Amberlyst 15. The kinetic data we
re correlated by a quasi-homogeneous model with which the apparent rate con
stants at each reaction temperature were determined. The activation energie
s of the forward and the backward reactions were found to be 51.74 kJ.mol(-
1) and 45.28 kJ.mol(-1), respectively. As evidenced from experimental resul
ts, the equilibrium conversion of acetic acid and the apparent equilibrium
constant increase with increasing temperature, implying that the esterifica
tion is endothermic.