The Reaction of a food dye with bleach
Introduction
The overall purpose of the experiment was to determine the order in respect to the blue dye and the rate constant (K). With these found however, the overall rate law in the reaction between blue food coloring and the bleaching agent within commercial Clorox can be found.
The orders in a rate law equation represent the relationship between the concentration of a given element or molecule and the overall rate, for example, when a reaction in respect to the concentration of an element is first order and the concentration is doubled so too would the rate of the reaction. Also, if the concentration has a second order in respect to it, the rate would be quadrupled, while a concentration with zero …show more content…
Discussion As stated before, the purpose of the experiment was to find the order in respect to the blue dye as well as the rate constant and concentration. The order in respect to the blue dye turned out to be first order which then makes the overall reaction second order. Maximum absorbance turned out to be 1.393 at 630 nanometers. Molar concentration was found to be 1.01 X 10-5 and Kobs from the graph was negative .293 while the rate constant was calculated to be 7.58 X 105. Wavelength of maximum absorbance was found by repeated testing of wavelengths until the max absorbance was found to be 1.393 at 630 nanometers. Using the Beers-Lambert law, maximum absorbance and the molar absorptivity of the blue dye (1.38 X 105 M-1cm-1) were used to calculate the molar concentration of the blue dye.
The order in respect to the blue food dye was found by plotting the data against three different graphs: absorbance vs. time for zero order, the natural log of absorbance vs. time for first order, and one over the absorbance vs. time for second order. The graph that created a linear plot (a straight line) indicated the order in respect to the blue
Introduction
The overall purpose of the experiment was to determine the order in respect to the blue dye and the rate constant (K). With these found however, the overall rate law in the reaction between blue food coloring and the bleaching agent within commercial Clorox can be found.
The orders in a rate law equation represent the relationship between the concentration of a given element or molecule and the overall rate, for example, when a reaction in respect to the concentration of an element is first order and the concentration is doubled so too would the rate of the reaction. Also, if the concentration has a second order in respect to it, the rate would be quadrupled, while a concentration with zero …show more content…
Discussion As stated before, the purpose of the experiment was to find the order in respect to the blue dye as well as the rate constant and concentration. The order in respect to the blue dye turned out to be first order which then makes the overall reaction second order. Maximum absorbance turned out to be 1.393 at 630 nanometers. Molar concentration was found to be 1.01 X 10-5 and Kobs from the graph was negative .293 while the rate constant was calculated to be 7.58 X 105. Wavelength of maximum absorbance was found by repeated testing of wavelengths until the max absorbance was found to be 1.393 at 630 nanometers. Using the Beers-Lambert law, maximum absorbance and the molar absorptivity of the blue dye (1.38 X 105 M-1cm-1) were used to calculate the molar concentration of the blue dye.
The order in respect to the blue food dye was found by plotting the data against three different graphs: absorbance vs. time for zero order, the natural log of absorbance vs. time for first order, and one over the absorbance vs. time for second order. The graph that created a linear plot (a straight line) indicated the order in respect to the blue