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<div class="moz-cite-prefix">After determining the order with
respect to both reactants you have concentration and rate data for
eight separate experiments.</div>
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<div class="moz-cite-prefix"><math
xmlns="http://www.w3.org/1998/Math/MathML"><semantics><mstyle
mathvariant="normal"><mi mathvariant="normal">r</mi><mi
mathvariant="normal">a</mi><mi mathvariant="normal">t</mi><mi
mathvariant="normal">e</mi><mo>=</mo><mi
mathvariant="normal">k</mi><mo stretchy="false">[</mo><msup><mi>I</mi><mo>−</mo></msup><msup><mo
stretchy="false">]</mo><mi>a</mi></msup><mo
stretchy="false">[</mo><msub><mi>H</mi><mn>2</mn></msub><msub><mi>O</mi><mn>2</mn></msub><msup><mo
stretchy="false">]</mo><mi>b</mi></msup></mstyle><annotation
encoding="TeX">\mathrm{rate = k [I^-]^a[H_2O_2]^b}</annotation></semantics></math></div>
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<div class="moz-cite-prefix">you can plug in your rate and
concentrations (both for iodide and peroxide) as well as the
orders for each trial to determine a value for k, the rate
constant. The average of these eight rate constants is then
reported as the rate constant for the reaction.<br>
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<div class="moz-cite-prefix">On 2/20/21 1:25 PM, wrote:<br>
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<blockquote type="cite"
cite="mid:33b91767381142e9a144871dae9876a3@SA1PR01MB6528.prod.exchangelabs.com">
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Thank you!</div>
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<div style="font-family: Calibri, Arial, Helvetica, sans-serif;
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I had another question about the kinetics concentration lab. I
finished all the calculation except for finding the K value at
the end. I was not sure which equation to use for that.</div>
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<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D. (<a class="moz-txt-link-abbreviated" href="mailto:pounds_aj@mercer.edu">pounds_aj@mercer.edu</a>)
Professor of Chemistry and Computer Science
Director of the Computational Science Program
Mercer University, Macon, GA 31207 (478) 301-5627
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