The Iodine Clock reaction is a prime example of where chemical kinetics can be observed. Iodine Clock reactions refers to a group of reactions which requires the combining of two colorless solutions to produce a new solution which remains colorless for a specific amount of time, which eventually changes to a deep blue color (Missouri University of science and technology, 2016). This is also known as the clock mechanism. The clock reaction can be observed in a Hydrogen Peroxide Iodine clock reaction in which the oxidation of Potassium Iodide is carried out by Hydrogen Peroxide.
H2O2(aq)+ 3 I-(aq) + 2 H+(aq) → I3-(aq)+ 2 H2O(aq)………..
I3-(aq) + 2 S2O32-(aq) → 3 I-(aq) + S4O62-(aq) …….
2 I3-(aq) + starch → starch-I5-complex + I- (aq) …………
(B. Z. Shakhashiri,1992)
The above equations describe the reaction mechanism for an Hydrogen Peroxide Iodine clock reaction. In reaction  it states that the iodide ions (I) are oxidized by hydrogen peroxide(H2O2 ) in an acidic solution to form triiodide ions (I3 ) and water( H2O) (B. Z. Shakhashiri,1992). Subsequently the triiodide ions (I3 ) are reduced back to iodide ions (I) by thiosulfate ions (S2O3) as indicated in r...
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The following experiment is to be carried out to investigate the effects of various variables including temperature, concentration and the use of catalyst on the rate of reaction of a Hydrogen Peroxide Iodine Clock reaction. It can be hypothesised that increasing the temperature in 10°C increments will increase the reaction rate by double and decreasing the temperature in 10°C increments will decrease the reaction rate by half. This is in accordance with the general rule about temperature increase for aqueous solutions. According to collision theory it can also be hypothesised that the increase in concentration of the hydrogen peroxide and sodium thiosulphate should increase the reaction rate too. The addition of a catalyst, iron chloride , will also increase the rate of the reaction as it will lower the activation energy needed for the reaction to happen.
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