The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: _IO_IO_I+_100 Experiment [OCI], M Initial Rate, [I], M M. 8-1 1 0.00240 0.00313 5.36 × 10-4 2 0.00240 0.00626 1.07 x 10 -3 3 0.00479 0.00313 1.07 x 10-3 4 0.00479 0.00626 2.14 x 10-3 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 mor n. Rate= k = M-1 8 -1

The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: _IO_IO_I+_100 Experiment [OCI], M Initial Rate, [I], M M. 8-1 1 0.00240 0.00313 5.36 × 10-4 2 0.00240 0.00626 1.07 x 10 -3 3 0.00479 0.00313 1.07 x 10-3 4 0.00479 0.00626 2.14 x 10-3 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 mor n. Rate= k = M-1 8 -1

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.38E: List at least four experimentally determined parameters that you, an experimenter, can define when...

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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 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.)
For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.
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