[CHM 112] Lab Reports- Madelyn Alligood

[Andrew J. Pounds]

The rate is based off of the disappearance of peroxide which is tied to
the disappearance of thiosulfate by stoichiometry.  The color change
took place because all of the thiosulfate was consumed.  Therefore the
rate of loss of peroxide is the rate of loss of thiosulfate divided by 2.

The initial concentration of I- affects the rate, but when we measure
the rate it is always based on the disappearance of peroxide as
described above.  If you look at my spreadsheet, all of the rates/(for
both the peroxide and iodide trials)/ are calculated based on the
disappearance of [S2O32−]\mathrm{[S_2O_3^{2-}]} because that is what
caused the color change.

Let me know if you have other questions.

On 2/19/21 9:45 PM,  wrote:
> Dr. Pounds, this is  from CHM 112. I had a quick question for the
> Kinetics Concentration Effect Lab Report! When calculating the rates
> for the I- Effect, the way to set it up is (-1/2)(final concentration
> - initial concentration/ change in time), correct? I just want to be
> certain that I am calculating it correctly!
>
> Thank you
>

-- 
Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu)
Professor of Chemistry and Computer Science
Director of the Computational Science Program
Mercer University,  Macon, GA 31207   (478) 301-5627

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