Chem102L_Exp13

Chem102L_Exp13 - Experiment 13 Chemical Kinetics SPRING...

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Experiment 13 – Chemical Kinetics Name Lab Day and Time TA Section Documentation GRADING RUBRIC Possible Points Points Received Introduction 5 Purpose of report Goals of the experiment Materials and Methods 5 Reference lab manual Only describe deviations Results and Discussion 70 Inserted titles for tables Inserted graphs into template Inserted captions for each graph Showed complete sample calculations Summarized all data in tables Answered questions completely Error analysis Laboratory Technique 20 TOTAL (100) TA Comments/Suggestions: SPRING 2008
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C HEMISTRY 102L R EPORT T EMPLATE EXPT. Chemical Kinetics: Reaction of Crystal Violet with Sodium Hydroxide 13 13 Introduction The purpose of this report is to summarize and analyze the data recorded during the course of reactions of differing concentrations of crystal violet with sodium hydroxide and to determine the order of reaction and rate constant, integral parts of the rate law, of this reaction. This data will be analyzed using two methods of chemical kinetics- the integrated rate laws and the initial rate method. The objective of the experiment was to gather data on the chemical reaction between crystal violet and sodium hydroxide so that the rate law could be fully calculated. Materials and Methods The procedure for this experiment was taken from the lab manual distributed by UNC. No deviations were made from the lab manual Results and Discussion When light is passed through a colored solution, certain wavelengths of the light are absorbed or reflected by the solution, unless the solution is colorless. As a reaction proceeds that yields a colorless product, the light will be absorbed or reflected less and less, enabling us to measure the progress of the reaction. The reaction studied in this experiment is the decolorization of crystal violet by sodium hydroxide. As the reaction proceeds, the sodium hydroxide reacts with the crystal violet, leaving a colorless solution. By using Beer’s law, a relationship between absorbance and concentration, the absorbance of the crystal violet at any concentration can be found, enabling us to monitor the amount of crystal violet left unreacted as the reaction occurs. Figure 1. Beer’s Law Plot of Absorbance (unit-less) versus Concentration (in 10 -6 M) for all four concentrations of crystal violet.
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Table 1. Analysis of Beer’s Law Plot (Linear Regression Data) Slope, m 0.0861 y-intercept, b -0.0491 Correlation coefficient, r 0.979 In order to determine the rate of the reaction, integrated rate laws are used. Depending on the order of the reaction, the rate law of the reaction can be graphed in a linear form, using the integral of the rate law, allowing the experimenter to find, through testing, the order of the reaction. Figures 2-4 below show the
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This note was uploaded on 03/21/2008 for the course CHEM 102 taught by Professor Todd during the Spring '08 term at UNC.

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Chem102L_Exp13 - Experiment 13 Chemical Kinetics SPRING...

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