To determine the rate law of a chemical reaction

Aim: To determine the rate law of chemical reactionsIntroduction: The aqueous radical of one thousand peroxydisulphate can oxidize potassium iodide as go along:Equation:K S 0 (aq) + 2KI (aq)->2K S0 (aq)+I (aq)2 2 8 2 4 2KI(aq) +I (aq) -> KI (aq)2 3_________________________________________________K S 0 (aq) +3KI(aq) -> 2K S0 (aq)+ KI (aq)2 2 8 2 4 2The rate law of this reaction can be represented as follow:Rate=k[S208 2-]^a [I-]^bWhen the concentration of peroxydisulphate ions is fixed, the prepare of reaction with repute to iodide ion is formed.

Alos, when the concentration of iodide ion is fixed, the battle array of reaction with respect to peroxydisulphat can be found.

It is important to keep the same muckle of solution in each trial.To determine the order of this reaction, the initial rate method is applied.This experiment is often known as the ace clock experiment.

Materials and apparatus:1) 100cm3 beaker2)burette3)0.1M K2S2084)0.1M KI5)0.002M K2S2086)starch7)water8)test tubes9)stop watchPrecautions:1) The stop watch should be started after the potassium peroxysulphate solution just complicated with potassium iodide.

2) Drawes a get across on a white paper that will be easier to observe the intensity of dark blue intensity.

Procedures:1. KI,starch and sodium thiosulphate were mixed into a boiling tube following the table which was an attachment(Data treament).

2. The categorization was transferred to a 100cm3 beaker.

3.



The exact amount of sodium peroxydisulphate was added in a boiling tube to the mixture in (2) as shortly as possible. At the same measure, the stop watch was stared.

4. The time for the solution to turn dark blue was recorded.

Data preaching and the result and calculations*(pls look at the attachment)Discussion:In this experiment, the overall of reaction is 2.

The use of sodium thiosulphate in this experiment is monitor the reactions becuse when the iodine colour(dark blue) disappear, it implies the thiosulphate is used up,too.

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