Kinetics Lab Report.docx - Clark 1 Kendra Clark Michael...

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Clark 1Kendra ClarkMichael Raphael ShabetaiCHEM 100823 March 2021Kinetics Lab ReportAbstractChemical kinetics study’s chemical reaction rates, factors affecting those rates, and themechanisms by which those reactions occur. Knowledge of chemical kinetics is critical for theoptimization of various industrial or domestic reactions. Acetone iodination reaction is the mostused reaction to study chemical kinetics. By varying the concentrations of reactants, this labdemonstrated that acetone iodination reaction rate depends on the reactants' concentration.IntroductionSeveral factors influence chemical reaction rates. Key among such factors are reactantconcentrations, the temperature, the reaction nature, and catalyst presence. One of the reactionscommonly used in reaction kinetics studies is the iodination of acetone. The formula gives therate law for the reaction:rate = k[acetone]a[H+]h[I2]iWhere a, h, and i are the reaction orders with respect to acetone, hydrogen ions, and iodine,respectively (Cloonan 23). The iodination of acetone is easily observable due to iodine's deepbrown color. As the reaction progresses, iodine is increasingly converted to iodine anion.Therefore, the deep brown color gradually disappears. This reaction rate can be determinedeasily by making iodine the limiting reactant in excess hydrogen ions and acetone. In such cases,the initial concentration of iodine is used up ultimately (Cloonan 23). Therefore, the reaction rate
Clark 2can be determined by monitoring the time taken for iodine's deep brown color to disappearcompletely. The rate can then be expressed as:Rate = Δ [I2

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Term
Fall
Professor
Pheobe Zito
Tags
Chemical reaction, Kendra Clark

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