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ClockReaction_InitialRates_Student

ClockReaction_InitialRates_Student - Vitamin C Clock...

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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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