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<div class="moz-cite-prefix">On 07/13/2015 07:25 PM, wrote:<br>
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cite="mid:C40B2F181831EF44A88CD73525827803130FFFABC6@MERCERMAIL.MercerU.local"
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<p>I'm having a little trouble finding the rate for the I-
effect. In order to find the rate, will I use [initial
H2O2]-[initial I-]/ delta t multiplied by -1/2 or just use <span
style="font-size: 12pt;">[initial H2O2]-[initial I-]/ delta</span><span
style="font-size: 12pt;"> t? I know stoichiometry comes into
play somewhere when finding the rate of reaction. </span></p>
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<br>
Whoa -- thats not how you do it. Remember, we are ALWAYS following
the rate of loss of peroxide. That is the same for ALL of the
experiments you did. The rate of loss of peroxide is tied to the
rate of loss of the thiosulfate ion via the reaction
stoichiometry. Remember -- for ALL the rates you divide the
diluted thiosulfate ion concentration by two and then divide that
value by the time. <br>
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<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D. (<a class="moz-txt-link-abbreviated" href="mailto:pounds@theochem.mercer.edu">pounds@theochem.mercer.edu</a>)
Professor of Chemistry and Computer Science
Mercer University, Macon, GA 31207 (478) 301-5627
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