Alcohol Oxidation

Topics: Chemical kinetics, Rate equation, Reaction rate Pages: 3 (832 words) Published: February 7, 2012
Introduction:
The purpose of this experiment is to monitor the rate of alcohol oxidation and study the reaction rates that are involved in chemical kinetics. The kinetic rate constant and order of the reaction will be found through this study. One of the main objectives we attempt to accomplish will be determining the maximum light absorbance of K2Cr2O7. We will use a LoggerPro apparatus to determine the absorbance. We will utilize Beer’s Law, which states that the absorbance is directly proportional to the concentration of a solution. Also, after performing the experiment, four graphs will be constructed from the data we collect. These graphs are Beer’s Law calibration curve, [K2Cr2O7] vs. time, Ln [K2Cr2O7] vs. time, and 1/[K2Cr2O7] vs. time. These graphs ought to show a trend relating to the concentration of the K2Cr2O7. By using a computer to plot and analyze the data, we will be more accurate and receive more information based on the reaction. Data:

| Absorbance | [K2Cr2O7]| Ln[K2Cr2O7]| 1/[K2Cr2O7]|
30| 0.583457| 0.00229| -6.07| 436.7|
60| 0.545668| 0.00214| -6.15| 467.3|
90| 0.51189| 0.00201| -6.2| 497.5|
120| 0.477355| 0.00187| -6.28| 534.8|
150| 0.447483| 0.00175| -6.35| 571.4|
180| 0.418738| 0.00164| -6.41| 609.8|
210| 0.394025| 0.00155| -6.47| 645.2|
240| 0.370999| 0.00146| -6.53| 684.9|
270| 0.350488| 0.00138| -6.59| 724.6|
300| 0.331227| 0.0013| -6.65| 769.2|
330| 0.313407| 0.00123| -6.7| 813|
360| 0.29599| 0.00116| -6.76| 862.1|
390| 0.281267| 0.0011| -6.81| 909.1|
420| 0.266467| 0.00104| -6.87| 961.5|
450| 0.252696| 0.00099| -6.92| 1010|
480| 0.239348| 0.00093| -6.98| 1075|
510| 0.228189| 0.00089| -7.02| 1123|
540| 0.217059| 0.00085| -7.07| 1176|
570| 0.206938| 0.00081| -7.12| 1234|
600| 0.198004| 0.00078| -7.16| 1282|
630| 0.189952| 0.00075| -7.2| 1333|
660| 0.182047| 0.00071| -7.25| 1408...
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