SVaaole untr you sign in againUse the References to access important values if needed for this question.The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion:2 Hgclz + C20, 2 cr + HgzClz + 2 co2Experiment(HgClale. M(C,0,. MInitial Rate, Ms0.3390.2812.73x1020.6780.2815.46x10430.3390.5611.09x103140.6782.18x100.561Complete the rate low for this reaction in the box below.Use the form k[A]"(B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.RateFrom these data, the rate constant isSubmit AnswerTry Another Version2 item attempts remainingNext

Given, Experiment HgCl2M C2O42-M Initial rate MS-1 1 0.339 0.281 2.73 × 10-4 2 0.678 0.281…

ces to acc important values if needed for this question. The following initial rate data are for the reaction of mercury(1) chloride with oxalate lon: 2 HgCl, + C30, 2 cr + Hg;Clz + 2 co2 Experiment (C,0, M Initial Rate, M r 2.73x10 5.4610 1.09x10 0.339 0.281 0.678 0.281 0.339 0.561 0.678 0.561 2.1810 Complete the rate law for this reaction in the box below. Use the form kEA)"(B)", where 1' is understood for m or n and concentrations taken to the zere power do not appear. Den't enter 1 for m or n. Rate From these data, the rate constant is Submit Answer Try Another Version 2 tem attempts remaining ( Ne)

ces to acc important values if needed for this question. The following initial rate data are for the reaction of mercury(1) chloride with oxalate lon: 2 HgCl, + C30, 2 cr + Hg;Clz + 2 co2 Experiment (C,0, M Initial Rate, M r 2.73x10 5.4610 1.09x10 0.339 0.281 0.678 0.281 0.339 0.561 0.678 0.561 2.1810 Complete the rate law for this reaction in the box below. Use the form kEA)"(B)", where 1' is understood for m or n and concentrations taken to the zere power do not appear. Den't enter 1 for m or n. Rate From these data, the rate constant is Submit Answer Try Another Version 2 tem attempts remaining ( Ne)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter30: Kinetic Methods Of Analysis

Section: Chapter Questions

Problem 30.16QAP

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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 following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
For the zero-order decomposition of ammonia on tungsten NH3(g) W 12 N2(g)+32 H2(g)the rate constant is 2.08104mol/Ls. (a) What is the half-life of a 0.250 M solution of ammonia? (b) How long will it take for the concentration of ammonia to drop from 1.25 M to 0.388 M?
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3