Kinetics of the Reactions of Crystal Violet with Sodium Hydroxide

Kinetics of the Reactions of Crystal Violet with Sodium Hydroxide

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Roshni Sheth CH 118-M3 February 3, 2010 Kinetics of the Reactions of Crystal Violet with Sodium Hydroxide 1. The Relationship Between Absorbance and Concentration Trial Absorbance Concentration 1 0.1169 5.00E-07 2 0.2269 2.00E-06 3 0.4416 5.00E-06 4 0.6736 8.00E-06 The equation represented here is Beer-Lambert’s law: A=Elc. This equation represents absorbance is equal to the extinction coefficient, E, times the path length of the cell, l, times the concentration, c. Since l is 1, the slope can represent the value of E, or the correlation coefficient. E=73986 The y-intercept is 0.0781. 2. The Rate Law Expression 0.2 M NaOH Time (seconds) Concentration (M) 0 1.15E-06 15 1.00E-06 30 7.69E-07 45 6.16E-07 60 4.62E-07
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0.1 M NaOH Time (seconds) Concentration (M) 0 1.39E-06 15 1.15E-06 30 1.00E-06 45 7.69E-07 60
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Unformatted text preview: 6.16E-07 Since the points of the first order graphs make straight lines, the rate law is of first order. 0.2 M: rate= 0.0154[NaOH] 0.1 M: rate=0.0135[NaOH] The rate law is useful in predicting the rate based on the concentration of vice-versa. 4. Description of the Reaction The data collected by the computer shows the relationship of Absorbance and Time in the second part of the reaction. When the 0.2 M solution was added to the cuvet of crystal violet, the color changed over time, which is how the absorbance changed over time. Using the correlation coefficient calculated in the first part of the experiment, the absorbencies were translated into concentration values, so the rate late could be determined....
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This note was uploaded on 06/28/2011 for the course CH 118 taught by Professor March during the Spring '09 term at University of Alabama at Birmingham.

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Kinetics of the Reactions of Crystal Violet with Sodium Hydroxide

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