A kinetic study of the hydrodenitrogenation of quinoline is performed in a batch reactor, over a NiMo(P)/gamma-Al2O3 sulfide catalyst, in the range of temperature of 340-360 degrees C and concentration of 1-2 wt % of quinoline. Liquid vapor mass transfer is considered in the reactor model, and the kinetic expression using Langmuir-Hinshelwood model considers competitive adsorption of reactants, products, and solvents. The activation energies of every elementary reaction and adsorption enthalpies of nitrogen compounds are calculated. The kinetic modeling shows that the hydrogenation of 1,2,3,4-tetrahydroquinoline into decahydroquinoline is the rate-determining step of the principal reaction pathway. The self-inhibition effect due to competitive adsorption of nitrogen-containing compounds is confirmed. The adsorption constants of nitrogen compounds decrease in the order saturated amines > NH3 > aromatic amines, showing that their adsorption strength is related to the basicity of molecules. Moreover, the kinetic model is validated by an additional experiment using ammonia as an inhibitor.