The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 Rate k = AsO3³+ 2Ce4+. = 4+ [ASO3³] [C¹+] M M 0.0311 0.0622 0.0311 0.0622 3- + H₂O → AsO4³ + 2Ce³+ + 2H+ M-2.s -1 0 Complete the rate law 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. I 0.145 0.145 0.290 0.290 Initial Rate, -1 M.s 0.000345 0.000690 0.00138 0.00276

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 Rate k = AsO3³+ 2Ce4+. = 4+ [ASO3³] [C¹+] M M 0.0311 0.0622 0.0311 0.0622 3- + H₂O → AsO4³ + 2Ce³+ + 2H+ M-2.s -1 0 Complete the rate law 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. I 0.145 0.145 0.290 0.290 Initial Rate, -1 M.s 0.000345 0.000690 0.00138 0.00276

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

See similar textbooks

Similar questions

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.
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?
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
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 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.
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
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.
4 for each temperature . 4.8 c , 22.0c , 37.4c calculate 1/t and ln (rate ) . slope = -1.96E+03. activation energy 1.63E+04 J
For the reaction NH2SO2OH + H2O → NH4HSO4 In aqueous solution at 80.35oC, the following constants were observed at the indicated ionic strength μ x103 k (L/mol hr) 5.06 1.07 11.21 1.02 15.85 0.976 22.94 0.886 From these data ascertain: a.) the valence of the reacting ions and b.) the rate constant for the primary salt effect.
Combination # [IO3-]0 [H+]0 [I-]0 average dt(sec) Initial rate, M s-1 kR (including units) 1 0.010 0.00002 0.10 18.1 0.00055 2 0.020 0.00002 0.10 9.1 0.0022 3 0.010 0.00002 0.20 5.1 0.0020 4 0.010 0.00002 0.10 5.1 0.0020 1. Determine the orders x,y and z 2. Calculatethe rate constant, kR and average kR for combimnations 1-4 3. Write the experimenally determined rate law Rate =kR[IO3-]x [I-]y [H+]z
Calculate the magnitude of the diffusion-controlled rate constant at 320 K for the recombination of two atoms in water, for which η = 0.89 cP. Assuming the concentration of the reacting species is 1.5 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.
For the gas phase decomposition of cyclobutane,(CH2)4 -----> 2 C2H4the rate constant has been determined at several temperatures. When ln k in s-1 is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -3.15×104 K and a y-intercept of 35.9.The activation energy for the gas phase decomposition of cyclobutane is _____ kJ/mol.