In a cell, 0.50 mL of 0.75 M NaOCl and 2.50 mL of 5.50 x 10-6 M aqueous dye were mixed. The pseudo order was applied and the absorbance was measured as a function of time. By plotting ln [Tint] as a function of time in seconds, a graph with a linear trend is obtained whose slope is -0.0354 s-1. If the order with respect to NaOCl is 1, what is the value of the rate constant in M-1s-1?

In a cell, 0.50 mL of 0.75 M NaOCl and 2.50 mL of 5.50 x 10-6 M aqueous dye were mixed. The pseudo order was applied and the absorbance was measured as a function of time. By plotting ln [Tint] as a function of time in seconds, a graph with a linear trend is obtained whose slope is -0.0354 s-1. If the order with respect to NaOCl is 1, what is the value of the rate constant in M-1s-1?

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter15: Molecular Luminescence Spectrometry

Section: Chapter Questions

Problem 15.15QAP: The following lifetimes were measured for the chloride quenching of quinine sulfate given in Example...

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The following lifetimes were measured for the chloride quenching of quinine sulfate given in Example 15-1.The fluorescence intensities are given in the example. (a) Plot fluorescence intensity versus [Cl-]. (b) Plot the ratio of intensity to lifetime, F- versus [Cl-]. (c) Develop a normalization factor to correct the measured fluorescence intensity to that of the solution without quencher. (d) Plot on the same graph Fversus [Cl-] and Fcorr versus (CI-].
The chromium in an aqueous sample was determined by pipetting 10.0 ml. of the unknown into each of five 50.0-mL volumetric flasks. Various volumes of a standard containing 12.2 ppm Cr were added to the flasks, following which the solutions were diluted to volume. Unknown,mLStandard, mLAbsorbancc 10.00.00.201 10.010.0 0.292 10.020.0 0.378 10.030.0 0.467 10.040.0 0.554 (a) Plot the data using a spreadsheet. (b) Determine an equation for the relationship between absorbance and volume of standard. (c) Calculate the statistics for the least-squares relationship in (b). (d) I)ctcrmine the conccnt ration oÍCr in ppm in the sample. (e) Find the standard deviation of the result in (d).
What is the pathlength in centimeters when the molar absorptivity for a given absorbing species is 1.32 x 103 L mol-1 cm-1, the concentration is 0.000923 M, and the absorbance is 0.493?
. A student collects the following data for the absorbance of a complex measured in 1.00 cmspectrophotometric cells. The molar absorptivity (ε) of the complex under investigation is 2.25×103L/mol·cm. Calculate the concentration of the complex in solution at each time of the reaction.Time (min)MeasuredAbsorbanceComplex Concentration(M)0.000 1.50010.000 1.31320.000 1.12530.000 0.93840.000 0.750
5. A solution of certain dye has a calibration graph shown below when measured at 425 nm in 1.00cm cells. A sample of the dye with an unknown concentration has an absorbance of 0.733. Determine the molar absorptivity of the dye at 425 nm and the concentration of the dye in the unknown solution. Absorbance vs. Concentration 1.200 1.100 1.000 0.900 0.800 0.700 0.600 0.500 0.400 1.50E-05 2.50E-05 3.50E-05 4.50E-05 5.50E-05 6.50E-05 Dye Concentration (Mol/L)
In a cell, 0.50 mL of 0.75 M NaOCI and 2.50 mL of 5.50 x 10-6 M aqueous dye were mixed. The pseudo order was applied and the absorbance was measured as a function of time. By plotting In [Tint] as a function of time in seconds, a graph with a linear trend is obtained whose slope is -0.0354 s-1. If the order with respect to NaOCI is 1, what is the value of the rate constant in M-1s-1? а. 6.44 х 103 М-1s-1 b. 0.47 M-1s-1 С. 7.72 х 103 М-1s-1 d. 0.28M-1s-1
Chemistry Calculate the concentration of an anthracene solution which produced a fluorescence intensity (I) of 835 when the irradiance of the beam incident to the sample (Po) was 1.580 x 10' and the length of the medium (b) was 0.891 cm. Anthracene has a molar extinction coefficient (e) of 9.5 x 10 M-¹ cm. The proportionality constant k' for anthracene is 0.30. CO M
6. Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x A solution is prepared by diluting 2.79 mL of the blue dye stock solution to 25.00 mL. The measured absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical x 10 |M (b) What is the experimental molar concentration? [Blue]experimental x 10 M (c) What is the percent error? Percent error (blue) = %
A student conducted an experiment to determine the concentration of benzene in an ethanol solution. Use the UV spectrum of the solution in a 2.0 cm cell. Within the spectrum, there was a peak attributed to benzene at 260 nm, with an absorption of 0.69. In a reference source, the student found that the adsorption of the benzene strip with ethanol was 2.95 x 10-3 ppm cm-. What is the molar concentration of benzene in the sample (mm of benzene = 78.11 g/mol)
In the fluorination reaction of butadiene, the butadiene is adsorbed onto a catalyst C.To test the efficiency of the adsorption, the adsorption isotherm was determined.The volume of butadiene per gram of C varied as follows at constant temperature:p( kPa)- 13.3; 26.7 ; 40.0 ; 53.3 ; 66.7 ; 80.0V(cm3)-17.9 ; 33.0 ; 47.0 ; 60.8 ;75.3 ; 91.3At the temperature used, p* for butadiene is 200 kPa. Find a suitable isotherm for the data and determine Vmon. please assist.
Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x A solution is prepared by diluting 2.81 mL of the blue dye stock solution to 25.00 mL. The measure absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical | × 10 |M (b) What is the experimental molar concentration? [Bluelexperimental x 10 M (c) What is the percent error? Percent error (blue) =
During a spectroscopic evaluation of the several solutions of C6H5CH=CHCCl₂ in ethanol using a 1.0 cm spectrophotometric cell, different values of absorbance (A) were obtained, which are given in the following table: 105 x conc. mol dm-3 A time min A 0.446 0.080 0 0.560 C When the reaction of C6H5CH=CHCCl₂ with C₂H5O in an ethanolic medium is followed spectroscopically at a convenient wavelength (2), the following results are found: 0.812 0.145 40 0.283 1.335 1.711 0.240 0.305 80 0.217 120 2.105 0.378 0.168 140 0.149 The values of ε at λ and the rate constant for that reaction are: a. ε = 1.79x10-6 dm³ mol-¹ cm-¹ and k = 0.034 dm³ mol-¹ min-¹ b. ε = 1.79×104 dm³ mol-¹ cm-¹ and k = 0.034 dm³ mol-¹ min-¹ c. ε = 1.79x10-6 dm³ mol-¹ cm-1 and k = 8.9x10-³ dm³ mol-¹ min-¹ d. ε = 1.79×104 dm³ mol-¹ cm-¹ and k = 8.9x10-³ dm³ mol-¹ min¯¹