[CHM 112] Help with Concentration Kinetics Lab

[Andrew J. Pounds]

For the concetration Kinetics Lab you will make TWO graphs.  Using the 
first set of data on the report form (the $I^-$ effect) you will plot 
the natural log of the rate on the Y axis and the natural log of the 
$I^-$ concentration on the X axis.  Determine the slope of this line. 
Then round the slope to the nearest whole number and that will be the 
order with respect to $I^-$.

Remember -- the rate you are measuring is always for the PEROXIDE so it 
is consistent between the first part of the lab and the second part of 
the lab.

For the second part of the lab repeat what you did in the first part but 
now plot where you look at the natural log of the rate on the Y axis and 
the natural log of the $H_2O_2$ concentration on the X axis.  Again 
determine the slope and then convert this to a whole number to determine 
the order with respect to peroxide.

Now -- in the last part of the lab you need to calculate the rate 
constant from all of your trials.  This is pretty easy, take each line 
of data and "solve for k"

\documentclass{article} \usepackage[utf8x]{inputenc} 
\usepackage[version=3]{mhchem} \pagestyle{empty} \begin{document} 
$\mathrm{RATE}$ = k [$I^-$]$^m $[$H_2O_2$]$^n$ %this is where your LaTeX 
expression goes \end{document}

Whey you have just determined the values for the reaction orders. You 
should get 8 values for k that should, theoretically, be close to each 
other.  Average all of them and report this value.


-- 
Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu)
Professor of Chemistry and Computer Science
Mercer University,  Macon, GA 31207   (478) 301-5627
http://faculty.mercer.edu/pounds_aj

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