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)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
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.
The activation energy for the decomposition of cyclobutane (C4H8) to ethylene (C2H4) is 261 kJ/mol. If the system produces ethylene at the rate of 0.043 g/s at 500C, what is the rate if the temperature increases to 600C?
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?
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.
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
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
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.
What is the difference between average rate, initial rate, and instantaneous rate?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction: