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### A Series Of Kinetic Reactions

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# A Series Of Kinetic Reactions

By | September 2010
Page 1 of 7
In this lab report, we went through a series of kinetic reactions to try and discover the reaction orders of different reactants that were involved with the reaction of Thiosulfate-Countered Oxidation of Iodide by Peroxydislufate, shown as S2O82-(aq) + 2S2O32-(aq) ( 2SO42-(aq) + S4O62-(aq).

However, before we could even begin to comprehend what exactly this reaction was doing or even what exactly we were looking for in this reaction, we needed to start from the beginning and learn more about what exactly kinetics is. In this lab, we were involved with Chemical Kinetics1. Chemical Kinetics is the study of rates of chemical processes. It also investigates how different experimental conditions can influence the speed of the reaction being studied as well as help in the construction of mathematical models that can describe the characteristics of a chemical reaction. A concept that was not directly brought up in class, but the principle was covered was the Law of Mass Action. This law states that the speed of a chemical reaction is proportional to the quantity of the reacting substances.

To further understand what Chemical Kinetics is, we needed to know what exactly a rate, or rate of reaction is2. A rate of reaction for a reactant or product is defined as how fast a reaction takes to place. For example, the oxidation of iron is a slow reaction that can take years, but the combustion or butane in a fire is a reaction that takes place in fractions of a second. For every chemical reaction, there is a rate equation3, which is an equation that links the reaction rate with concentrations or pressures of reactants and constant parameters. For every generic reaction A + B ( C, the rate is given as r = k [A] m[B]n. In which A and B is the concentration of the related reactants in molarities, k is the rate of proportionality constant, m is the reaction order for substance A, n is the reaction order for substance B, and r is rate at which the reaction takes to occur....

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