chemical kinetics

chemical kinetics - Chemical Kinetics Author Sam Strobe Lab...

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Chemical Kinetics Author: Sam Strobe Lab Partners: Julie Zappia, Lisa Ardizzone, Christine Brennan Instructor: Chase Parker Chem 152, section 61 Date Work Performed: January 29 th , February 1 st Date Report Submitted: February 8 th Abstract The experimental rate law equation for the reaction of red dye #3 and sodium hypochlorite was determined to be rate= .132[dye][NaOCl]. Both the dye and bleach (NaOCl) were determined to be first order for the reaction. The orders of the reaction for both were determined by tracking their absorbances over time with absorption spectroscopy, and translating the absorbance values to concentration using Beer’s Law, to create concentration/time graphs. The linearity of the graphs of ln [ ] vs time confirmed the reaction order of both reactants.
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Introduction This lab was designed to teach us about chemical kinetics, the study of the progression of chemical reactions over time. In the experiment, we were to, through numerous steps, determine an experimental rate law for a reaction between food dye and bleach. To determine the reaction order for the dye and the bleach, we were to run several trials, reacting the dye and bleach, varying the concentration of the bleach through dilution, and using absorption spectroscopy to track absorbance vs. time. Based on the assumption that the concentration of bleach stayed constant within each trial, we held the dye concentration constant through the four trials, changing only the concentration of the bleach. Then, we would be able to turn the absorbance/time graph into a graph of concentration/time, using Beer’s Law (A= ε b C), which describes the linear relationship between absorbance and concentration. By tracking the concentration of dye and bleach in this manner, we would then be able to determine the reaction order for each, as well as calculate the instantaneous rate at a point. Once we had calculated a few instantaneous rates and correlated
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