Reactions Essay

2045 WordsMar 16, 20139 Pages
Reaction Order and Rate Laws Abstract The purpose of the experiment is to determine the rate law for a reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3) and once found to calculate the k or specific rate constant of the reaction. To determine the reaction order and rate constant; two experiments with several trials of each will be conducted. First, the concentration of HCl will be changed while the concentration of Na2S2O3 is held constant. Next, the concentration of Na2S2O3 will be varied while the concentration of HCl is held constant. From this experimental data it is found that HCl is zero order in the reaction and Na2S2O3 is first order. It can be concluded from the data that the concentration of Na2S2O3 has more of an effect on the rate of the reaction because when the concentration of Na2S2O3 is doubled the reaction time doubles. Introduction Kinetics is an area of chemistry that deals with the rate reactants form products. There are several factors that influence reaction rate including “nature of reactants, surface area, temperature, catalysts and concentrations.” (Jeschofnig, n.d. pg.104) In this experiment we will look at how the concentration of the reactants affects the rate at which the reactions occur. A theory that applies to this experiment is the collision theory which simply put states, the more reactants there are, the more possibility of the reactants colliding, breaking the bonds, and rearranging to form products. In the experiment the concentration of reactants will be varied and the time it takes for a product to form will be recorded. From this data, the rate law which is way of expressing this relationship between concentration and formation of products using a rate constant is determined. Materials 24-well plate Dish detergent Distilled water Pencil White paper Cotton Swabs Paper towel

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