ClockReaction_InitialRates_Student

ClockReaction_Initia - Vitamin C Clock Reaction Initial Rates Objective In this experiment you will determine the rate law for the reaction of H2O2

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Vitamin C Clock Reaction: Initial Rates Objective: In this experiment you will determine the rate law for the reaction of H 2 O 2 with iodide by using the initial rate measurements. H 2 O 2 + 3I - + 2H + I 3 - + 2H 2 O Starch is present in the reaction mixture as an indicator for the product, I 2 . When I 3 - binds to starch you see a dark blue-black color. The reaction in this experiment is called a clock reaction because instead of observing the gradual appearance of the product (I 3 - ), you will add another reagent, vitamin C, to use up I 2 (see reaction below) as fast as it is formed by the reaction with H 2 O 2 . I 3 - + C 6 H 8 O 6 (vitamin C) 2H + + 3I - + C 6 H 6 O 6 For a “clock experiment” to work, the process that uses up the product of the reaction of interest must be much faster than the reaction under study. Additionally, the reagent that reacts with the product must be present in limiting amount so that once the reagent is consumed an indicator (like starch) will change color.
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This note was uploaded on 01/03/2012 for the course CH 102 taught by Professor Hill,m during the Fall '08 term at Caltech.

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ClockReaction_Initia - Vitamin C Clock Reaction Initial Rates Objective In this experiment you will determine the rate law for the reaction of H2O2

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