Formal Report- Kinetics of Reaction: the Iodine Clock Reaction

Topics: Chemical kinetics, Chemical reaction, Reaction rate Pages: 15 (4623 words) Published: February 4, 2013
factors affecting the kinetics of reaction between peroxodisulfate (vi) and iodide

d. del prado1 and j. belano2
1 department of food science and nutrition, college of home economics 2 department of food science and nutrition, college of home economics university of the philppines, diliman, quezon city 1101, philippines date submitted: january 7, 2013



In everyday life, several reactions are encountered, but still knowledge on how fast these occur and the factors affecting it were still insufficient. This study aimed to determine the different factors affecting the rate of reaction and how these factors affected it. An experiment named iodine clock reaction was done to answer the questions raised. In this study the reaction of iodide ion and peroxodisulfate (VI) ion was analyzed with the help of thiocyanate ion. The experiment was divided into three parts. First, second, and third parts of the experiment were used to examine the effects of the reactant concentrations, temperature and the presence of catalyst to the rate of reaction, respectively. The time before the reaction proceeded was recorded and calculations were done to obtain necessary information. It was identified that increasing the reactant concentration would increase the rate of reaction. Likewise, higher temperature increased the rate. Finally, the presence of catalyst had enormous effect on the reaction rate. It increased as the catalyst was added. Based on the results obtained, it can be concluded that said factors could increase the rate of reaction by increasing the temperature or reactant concentration or by adding a catalyst on the mixture. -------------------------------------------------


Until now it has been thought that in chemical reactions reactants combine with one another to form products, and that we can use a balanced equation in determining the amount of products formed. But this simple explanation does not tell us the rate of the reaction. [1]Rate of reaction refers to the speed at which reactants break down and recombine to form new substances. In order for a reaction to proceed, the reactant particles must collide and this is what so called the collision theory of chemical reactions. In addition to this theory, collision itself will not make a reaction to happen.[2][3] Molecules should be reactive and must be in their proper orientation. Moreover, enough energy must also be available in order to break the chemical bonds and the minimum amount of energy required to react is termed as the activation energy, Ea.

Why do fish get spoiled much slower inside the freezer than they do in markets? Rate of reactions differ from one another. Some reactions are so fast that they are already done as soon as the reactants are combined. Some may take minutes, days, months, and even years. What causes this wide range of reaction rates? [4]Several factors are influencing the speed of a reaction: concentration, temperature, presence of catalyst, and the physical state or nature of reactants involved. [5]In order to study the effect of those factors, the rate law or rate equation, which is the focal part of any kinetics study, will be of great importance. Rate law has this form: Rate = k[A]m[B]n

[A] and [B] are concentrations of the reactants expressed in molarity. Aside from that, there are also reaction orders, m and n, which tell us the effect of reactant concentration to the rate. k is the rate constant which is specific for a given reaction at a given /temperature. Always remember that data of the rate law – rate, reaction orders, and rate constant – should be obtained experimentally. In this study an experiment called the iodine clock rotation was done in...
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