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 11.55PAE: The following rate constants were obtained in an experiment in which the decomposition of gaseous...

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