Chemical Kinetics

Abstract

Chemical kinetics is the study of reaction rates and reaction mechanism. Reaction rate is the change in concentration of a product or a reactant with time. In this experiment, the effect of concentration to reaction rate was studied through measuring the reaction time of the reaction of Na2S2O3 and HCl in different concentrations. From the results obtained, it was concluded that the rate of reaction is directly proportional to the concentration. This can be explained by the collision theory. Since there are more particles, the chance of collision is higher thus, raising the rate of reaction. Using the Arrhenius theory that was based from collision theory, one can determine the activation energy. Activation energy is the minimum energy molecules must possess in order to form a product. Using the slope of Arrhenius equation, the plot of the activation energy was then formulated. Another set-up was done to test the effect of temperature to rate of reaction. This time, the reaction was carried in three different temperatures: in ice bath, at room temperature and at elevated temperature. From the data obtained, it shows that the rate of reaction is highest at elevated temperature and lowest at ice bath. Thus, it was concluded that rate of reaction is also directly proportional to temperature. On the next set-up, the effect of catalyst was demonstrated with the reaction of Titrate and Hydrogen peroxide. Also, autocatalyst was probed through the reaction of Permanganate and Oxalate. The results showed that a catalyst speeds up rate of reaction.