| The reaction kinetics of the chloroform photocatalytic oxidation in aqueous solution was studied using a recirculating batch reactor. Tests were performed using different CHCl$sb3$ initial concentrations and at an initial pH of 6.0. The initial rate of the photocatalytic reaction was determined. The initial rate of reaction increases with an increase in the initial concentration of CHCl$sb3$. The photocatalytic oxidation of chloroform follows first order kinetics under the experimental conditions used in this work with an apparent reaction constant of 2839 ml/g-min. The results were analyzed using a Langmuir-Hinshelwood kinetic model. The kinetic parameters in the expression of Langmuir-Hinshelwood model were: k (reaction constant) = 1317 gmol/g-min and K$sb{rm A}$ (adsorption constant) = 1.8 ml/g-min. The adsorption constant is small compared with the reaction constant which implies that, at the conditions used, the CHCl$sb3$ is weakly adsorbed over TiO$sb2$. The apparent reaction rate constant is equivalent to the product of the reaction constant and the adsorption constant (k$rmsb{ap} approx kKsb{A}).$ The value obtained by multiplying the Langmuir-Hinshelwood parameters (2464 ml/g-min) is similar to the value of $rm ksb{ap},$ which shows that this result is model independent.;Preliminary experiments of the photocatalytic oxidation of acetone, salicylic acid, tetrahydrofuran (THF), and chloroform (CHCl$sb3$) in aqueous solution were performed in a batch reactor. The order of the degradation rate for these compounds was the following: salicylic acid $>$ THF $>$ acetone $>$ CHCl$sb3.$ These results demonstrate that the photocatalytic oxidation is effective under these conditions for the degradation of these compounds. In addition, it was shown that the rate of degradation of CHCl$sb3$ increases with an increase in the intensity of the UV radiation. |
