The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO33- + 2 Ce4+ + H20- →ASO43- + 2 ce3+ + 2 H+ Experiment [Aso33"lo, M [Ce4+]o, M Initial Rate, M s*1 1 2.13x10-2 0.371 1.67x10-3 2 4.26x10-2 0.371 3.33x103 3 2.13x10-2 0.742 6.66x10-3 4 4.26x10-2 0.742 1.33x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[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. Rate = From these data, the rate constant is M-2s-1.

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: AsO33- + 2 Ce4+ + H20- →ASO43- + 2 ce3+ + 2 H+ Experiment [Aso33"lo, M [Ce4+]o, M Initial Rate, M s*1 1 2.13x10-2 0.371 1.67x10-3 2 4.26x10-2 0.371 3.33x103 3 2.13x10-2 0.742 6.66x10-3 4 4.26x10-2 0.742 1.33x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[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. Rate = From these data, the rate constant is M-2s-1.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Aso,3 + 2 Ce** + H20-Aso,3 + 2 Ce3* + 2 H* Initial Rate, M Experiment [Aso,3-], M [Ce**1, M Is 8.53x104 1.71x10-3 3.41x103 6.83x103 1 3.61x10-2 0.204 7.22x10-2 3.61x102 7.22x10-2 2 0.204 3 0.408 14 0.408 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. Rate = From these data, the rate constant is M2s1.
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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: OCr +I- OI + CI Experiment [OCI"]o, M , M Initial Rate, Ms™ -1 1.70×10-3 1.70×10-3 3.40x10-3 3.40x10-3 4.57×10-3 9.15×10-3 4.57x10-3 9.15×103 1 5.41x10-4 1.08×10-3 1.08×10-3 2.17x10-3 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 Rate = From these data, the rate constant is M's.
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If the [S2O32-] is initially 2.49 x 10-4 M, and the reaction takes 129 seconds for the solution to turn blue, what is the rate of the reaction expressed in terms of I2?
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