Use the References to access inmportant values if needed for this question.The temperature dependence of the reaction rate constant is given by the equation:E,Ink = In A -RTWhere:k= rate constantT = temperatureA = frequency factorE, = Energy of activationIn order to solve for the Energy of activation, E.. you must:Step OneAdd the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression:(Be sure that the answer field changes fromn light yellow to dark yellow before releasing your answer.)E,+ Ink-+ In A -RTDrag and drop your selection from the following list to complete the answer:In- InIn A- In APreviousNext

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Use the Rakerences to aecens important valuas if naeded for dis quastion. The temperature dependence of the reaction rate constant is given by the equation: E, Ink= In A- RT Where k rate constant T= temperature A= frequency factor E, – Energy of aetivation In order to sove for the Energy of activation, E., you must: Sle One Add the same enpression to each side of the equation to lesve the term that inchludes the variable by itself on the right-hand side of the expression: (Be sure that the answer feld changes from light yellow to dark pellow before neleazing your answer.) E. + Ink- + In A- Drag and drop your sdlection from the following list to complete the answer In A - In A

Use the Rakerences to aecens important valuas if naeded for dis quastion. The temperature dependence of the reaction rate constant is given by the equation: E, Ink= In A- RT Where k rate constant T= temperature A= frequency factor E, – Energy of aetivation In order to sove for the Energy of activation, E., you must: Sle One Add the same enpression to each side of the equation to lesve the term that inchludes the variable by itself on the right-hand side of the expression: (Be sure that the answer feld changes from light yellow to dark pellow before neleazing your answer.) E. + Ink- + In A- Drag and drop your sdlection from the following list to complete the answer In A - In A

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter4: Least-squares And Calibration Methods

Section: Chapter Questions

Problem 6P

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The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
Nitric oxide, NO, is known to break down ozone, O3, by the following bimolecular reaction: NO(g)+O3(g)NO2(g)+O2(g) If the activation energy of this reaction is 10.5kJ/mol and the pre-exponential factor is 7.91011cm3/(mols), a what is the rate constant of this reaction at 298K? b If the ozone concentration were 5.41012mol/cm3 and the NO concentration were 2.01012mol/cm3 conditions that might exist in a high-pollution area, what is the rate of this reaction?
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Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.