The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: 33+ 2Ce¹++ H₂O → AsO4³ +2Ce³+ + 2H+ 4+ AsO 3³ Experiment 1 2 3 4 [ASO3³] [C¹+] As M M 0.0328 0.0656 0.0328 0.0656 Initial Rate, M.S-¹ 0.00216 0.00431 0.00862 0.0172 0.359 0.359 0.718 0.718 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. Rate = K[AsO][Ce¹*] k= M-2.s-1

The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: 33+ 2Ce¹++ H₂O → AsO4³ +2Ce³+ + 2H+ 4+ AsO 3³ Experiment 1 2 3 4 [ASO3³] [C¹+] As M M 0.0328 0.0656 0.0328 0.0656 Initial Rate, M.S-¹ 0.00216 0.00431 0.00862 0.0172 0.359 0.359 0.718 0.718 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. Rate = K[AsO][Ce¹*] k= M-2.s-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: Experiment 1 2 3 4 3+ AsO3³ + 2Ce¹+ + H₂O → AsO4³ + 2Ce³+ + 2H+ Rate = k = [ASO3³] [Ce¹+] M M 0.0311 0.0622 0.0311 0.0622 M-2.s I 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. -1 0.145 0.145 0.290 0.290 Initial Rate, M.s-1 S 0.000345 0.000690 0.00138 0.00276
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