Iodine Clock Reaction

An investigation on the activation energy for the iodine clock reaction
Introduction:
The iodine clock reaction is a presentation of chemical kinetics, which are the elements that affect the rate of chemical reactions. When the two colorless solutions are incorporated together, no reaction can be spotted. But after a short period of time, the solution turns into a dark blue solution. The term rate of reaction is stated as the decrease in the concentration of one of the reactions or the increase in the concentration of one of the products per unit time, measured by the mol dm-3s-1 . The iodine clock reaction shows that not all reactions are quick and unidirectional proceeds to completion.
Iodine Clock Reaction:
This reaction has many alterations, the alteration used in this investigation is hydrogen peroxide and includes the use of, sodium thiosulfate, potassium iodide, and hydrogen peroxide. The use of starch solution is essential in this experiment as it acts as an indicator for the experiment turning the color of the solution dark blue in the appearance of iodine ions. This allows the end of the reaction to be determined. The clock reaction is shaped by two different reactions. The first reaction is the slow reaction which is:
This is used as a delay mechanism in the reaction, without this, the solution will immediately turn blue/black. When the iodine is formed, it reacts with the sodium thiosulfate, where it gets reduced and forms tetrathionate ions and iodide