The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution:OCr +I OI + CrExperiment[OCF], M7.67x10-37.67x10-31.53x10-21.53x10-2]. M2.43x10-34.86x10-32.43x10-34.86x10-3Initial Rate, Ms-11.24x10-312.48x10-32.48x10-34.95x10-34Complete the rate law for this reaction in the box below.Use the form k[A]mB]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or nRate =From these data, the rate constant is

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The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCt +I OI +CF Experiment 1 (OCr], M 7.67x10-3 7.67x10-3 1.53×10-2 1.53×10-2 1], M 2.43x10-3 4.86x10-3 2.43x10-3 4.86x10-3 Initial Rate, Ms 1.24x103 2.48x103 2.48×10-3 4.95x103 Complete the rate law for this reaction in the box below. Use the form k[A]"|B]" , where 'I' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCt +I OI +CF Experiment 1 (OCr], M 7.67x10-3 7.67x10-3 1.53×10-2 1.53×10-2 1], M 2.43x10-3 4.86x10-3 2.43x10-3 4.86x10-3 Initial Rate, Ms 1.24x103 2.48x103 2.48×10-3 4.95x103 Complete the rate law for this reaction in the box below. Use the form k[A]"|B]" , where 'I' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

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....

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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 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 oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
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.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
The first-order rate constant for the decomposition of a certain hormone in water at 25C is 3.42104day1. (a) If a 0.0200 M solution of the hormone is stored at 25C for two months, what will its concentration be at the end of that period? (b) How long will it take for the concentration of the solution to drop from 0.0200 M to 0.00350 M? (c) What is the half-life of the hormone?
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.