ClockReaction_IntegratedRateLaws_Student

ClockReaction_IntegratedRateLaws_Student - Vitamin C Clock...

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Vitamin C Clock Reaction: Integrated Rate Laws Objective: In this experiment you will determine the rate order in H 2 O 2 and the rate constant for the reaction of H 2 O 2 with iodide. The concentration of reagent and reaction times will be calculated/measured. Plots of integrated rate laws will be performed to indentify the best fit for the data and assign the order in H 2 O 2 . 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 . As soon as vitamin C is gone, however, the I 2 will persist and you will see the expected dark blue-black starch- iodine 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_IntegratedRateLaws_Student - Vitamin C Clock...

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